Ch.4 - Chemical Quantities & Aqueous ReactionsSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution Stoichiometry

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Sections
Molarity
Normality & Equivalent Weight
Solution Stoichiometry
Solubility Rules
Net Ionic Equations
Electrolytes
Redox Reaction
Balancing Redox Reactions
Activity Series
End of Chapter 4 Problems
Additional Practice
Dilution
Redox Reactions
Calculate Oxidation Number
Types of Chemical Reactions
Additional Guides
Net Ionic Equation
Oxidation Reduction (Redox) Reactions
Oxidation Number
LearnAdditional Practice
Next SectionSolubility Rules

Solution Chemistry involves combining the concepts of molarity and stoichiometry. 

Molarity and Chemical Reactions

Concept #1: Under solution chemistry our given information may be in units of mass, volume or molarity. 

Stoichiometry is used when given the known quantity of one compound and asked to find the unknown quantity of another compound or element. Now we throw molarity into the mix. 

Concept #2: When dealing with solution chemistry we use a new adjusted stoichiometric chart. 

This new Stoichiometric Chart is used anytime we are given the known quantity of a compound in units such as mL, L or M and asked to find the unknown quantity of another compound. 

Example #1: Molarity and Stoichiometry Calculation

By using our new Stoichiometric Chart we can now answer stoichiometric questions dealing with molarity. 

Using our new Stoichiometric Chart it is possible to now calculate the unknown volume of a compound through molarity. 

Practice: How many milliliters of 0.325 M HCl are needed to react with 16.2 g of magnesium metal?

2 HCl (aq) + Mg (s) ----> MgCl2 (aq) + H2 (g)

Knowing the volume and molarity of a compound allows us to determine the molarity of an unknown compound. 

Practice: What is the molarity of a hydrobromic acid solution if it takes 34.12 mL of HBr to completely neutralize 82.56 mL of 0.156 M Ca(OH)2?

2 HBr (aq) + Ca(OH)2 (aq) ----> CaBr2 (aq) + 2 H2O (l)

Practice: Iron (III) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation: Cr2O72- + 6 Fe2+ + 14 H+ -----> 2 Cr3+ + 6 Fe3+ + 7 H2O.  

If it takes 30.0 mL of 0.100 M K2Cr2O7 to titrate a 25 mL Fe2+ solution, what is the molar concentration of Fe2+?

Previous SectionNormality & Equivalent Weight
Next SectionSolubility Rules
Additional Problems
What volume of a 0.100 M HCl solution is required to exactly neutralize 25.0 mL of 0.235 M Ba(OH)2? The balanced equation is 2HCl(aq) + Ba(OH)2 → BaCl2 + 2H2O(l). a. 235 mL b. 117.5 mL c. 58.8 mL d. 29.4 mL e. 1.18 x 103 mL
What volume of 0.131 M BaCl2 is required to react completely with 42.0 mL of 0.453 M Na2SO4? This is the net ionic equation for the reaction. Ba2+(aq) + SO42-(aq) → BaSO4(s) a) 12.1 mL b) 72.6 mL c) 145 mL d) 290 mL
What volume (in mL) of 0.500 M KMnO 4 is required to react with 0.2506 g of Cu+ according to the equation: MnO4– + 5 Cu+ + 8 H+      ⇌       Mn2+ + 4H2O    a) 1.58 b) 15.8 c) 7.9 d) 0.176 e) 0.100
What volume of a 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution to the reaction below?   2 KCl (aq) + Pb(NO 3)2 (aq) → PbCl2 (s) + 2 KNO 3 (aq)   a. 97.4 mL b. 116 mL c. 43.0 mL d. 86.1 mL e. 58.1 mL
In the following redox reaction, dichromate ion, Cr 2O7 2- , oxidizes Fe2+ to yield the following products. Cr2O7 2- (aq) + 6 Fe 2+ (aq) + 14 H + (aq) → 2 Cr 3+ (aq) + 6 Fe 3+ (aq) + 7 H 2O (l) If it takes 35.0 mL of 0.250 M FeCl 2 to titrate 100 mL of a solution containing Cr 2O7 2- , what is the molar concentration of Cr2O7 2- ?  a. 0.015 M b. 0.053 M c. 0.027 M d. 0.045 M
Iron (III) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation below. How many microliters of a 0.250 M FeCl2 are needed to completely react with 8.24 g of a compound containing 31.3% weight K2Cr2O7?   Cr2O7 2- + 6 Fe 2+ + 14 H+ → 2 Cr3+ + 6 Fe 3+ + 7 H2O
Manganese in an ore can be determined by treating the ore with a measured, excess quantity of sodium oxalate (Na2C2O4) to reduce MnO2(s) to MnCl 2(aq) followed by determination of the unreacted sodium oxalate by titration with potassium permanganate. The equations for this two step process are:   MnO2(s) + Na2C2O4(aq) + 4HCl(aq) → 2MnCl 2(aq) + 2CO2(g) + 2H2O(l) +2NaCl(aq)   2KMnO4(aq) + 5Na2C2O4(aq) + 16HCl(aq) → 2MnCl 2(aq) + 10CO2(g) + 8H2O(l) + 10NaCl(aq)   If a sample is treated with 50.0 mL of 0.275 M Na 2C2O4(aq) and the unreacted Na 2C2O4(aq) requires 18.28 mL of 0.1232 M KMnO4(aq), calculate the number of grams of manganese in the sample. (NOTE: use the equations as written despite the fact they are not completely balanced) 
Consider the following reaction sequence for the determination of dissolved oxygen in water:   2MnSO4(aq) + 4NaOH(aq) + O 2(aq) → 2MnO2(s) + 2Na2SO4(aq) + 2H2O(l) MnO2(s) + 2H2SO4(aq) + 2NaI(aq) → MnSO 4(aq) + I 2(aq) + Na 2SO4(aq) + 2H 2O(l) I2(aq) + 2Na 2S2O3(aq) → Na 2S4O6(aq) + 2NaI(aq)   If 9.00 mL of 0.0240 M Na 2S2O3(aq) are used in the analysis, how many moles of dissolved oxygen were determined? a) 4.32 x 10-4 mol b) 2.70 x 10-5 mol c) 5.40 x 10-5 mol d) 2.16 x 10-4 mol e) 1.08 x 10-4 mol 
 How many moles of AgCl are formed from the reaction of 75.0 mL of a 0.078 M AgC2H3O2 solution with 55.0 mL of 0.109 M MgCl 2 solution? 2 AgC2H3O2 (aq) + MgCl 2 (aq) → 2 AgCl (s) + Mg(C2H3O2)2 (aq) a. 0.0120 moles AgCl b. 0.0117 moles AgCl c. 0.00585 moles AgCl d. 0.0600 moles AgCl
The iron content in ores can be determined by titrating a sample with a solution of potassium permanganate. The ore is first dissolved in hydrochloric acid, forming iron (II) ions, which react with permanganate ions according to the following net-ionic reaction: MnO4- (aq) + 5 Fe 2+ + 8H + (aq) → Mn 2+ (aq) + 5 Fe 3+ (aq) + 4 H 2O (l) A sample of ore of mass 0.202g was dissolved in hydrochloric acid, and the resulting solution needed 16.7 mL of 0.0108 M KMnO4(aq) to reach the stoichiometric point. What mass of iron (II) ions are present?         What is the mass percentage of iron in the sample of ore?
Consider the following balanced redox equation:  H2O  +  2 MnO4 –  +  3 SO32- →   2 MnO2  +  3 SO42-  +  2 OH – a)  How many moles of SO32- (MW:80.07 g/mol) are required to completely react with 20.3 mL of a 0.500 M MnO4– (MW: 118.90 g/mol) solution? a. 0.0152 moles SO32- b. 0.0067 moles SO32- c. 0.005075 moles SO32- d. 0.3045 moles SO32-     b) How many mL of a 1.25 M Na 2SO3 (MW: 126 g/mol) are required to completely react with 2.55 mL of a 3.50 M KMnO4 (MW: 158 g/mol) solution?            c) How many grams of MnO 2 (MW: 86.94 g/mol) are produced when 32.0 mL of 0.615 M MnO 4- (MW: 118.90 g/mol) reacts with excess water and sulfite?   
Blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with an acidic potassium dichromate, K2Cr2O7, solution. The balanced redox equation is given below: H+ (aq) + 2 Cr2O72- (aq) + C2H5OH (aq) → 4 Cr3+ (aq) + 2 CO 2 (g) + 11 H2O (l) If 45.12 mL of 0.04918 M Cr 2O72- solution is required to titrate 25.0 mL of C 2H5OH, what is the molar concentration of C2H5OH? a. 0.05450 M b. 0.01362 M c. 0.17752 M d. 0.04438 M
A 0.250 M solution of sulfuric acid (H2SO4) is to be reacted with a solution of sodium hydroxide via a double-displacement reaction to make sodium sulfate and water. 50.0 mL of the H2SO4 solution reacts with 25.0 mL of the NaOH solution. What is the molarity of the NaOH solution? (A) 0.0625 M (B) 0.125 M (C) 0.250 M (D) 0.500 M (E) 1.00 M
According to the following balanced reaction, how many moles of Fe(OH) 2 can form from 175.0 mL of 0.227 M LiOH solution?  Assume that there is excess FeCl2.              FeCl2(aq) + 2 LiOH(aq)  →  Fe(OH)2(s) + 2 LiCl(aq) A) 3.97 × 10−2 moles B) 2.52 × 10−2 moles C) 1.99 × 10−2 moles D) 5.03 × 10−2 moles E) 6.49 × 10−2 moles
Calculate the number of moles of iron(III)sulfide that forms when 62.0 mL of 0.135 M iron(III)chloride reacts with 45.0 mL of 0.285 M calcium sulfide. a) 8.56 x 10−3 mol b) 4.19 x 10−3 mol c) 1.25 x 10−2 mol d) 4.28 x 10−3 mol e) 8.38 x 10−3 mol
When 5.0 grams of Na2O (MM = 61.98 g/mol) are dissolved in 1.00 L of water, what is the concentration of the Na + ions? A. 0.040 M B. 0.080 M C. 0.16 M D. 6.2 M E. 12 M
Sulfuric acid cannot be stored in an aluminum container because sulfuric acid dissolves aluminum metal. The following equation shows the reaction: 2 Al (s) + 3 H2SO4 (aq) → Al2(SO4)3 (aq) + 3 H2 (g) Calculate the volume of sulfuric acid that would be required to completely dissolve a 4.643 g block of aluminum if you are given a 0.98 M H2SO4 solution. A. 175.60 mL B. 710.66 mL C. 284.48 mL D. 263.40 mL E. 242.33 mL  
In acidic solution, the dichromate ion, Cr2O72– (aq) will oxidize Fe2+ to Fe3+ and form Cr3+. This net ionic equation represents the reaction that takes place during the reaction.  Cr2O72- (aq) + 6 Fe2+ (aq) + 14H+(aq) → 2 Cr3+ (aq) +6Fe3+ (aq) + 7 H2O(l) What volume of 0.100 M Cr 2O7 2- (aq) is required to oxidize 60.0 mL of 0.250 M Fe 2+(aq)? a) 25.0 mL b) 42.0 mL c) 58.4 mL d) 175 mL
What volume (L) of a 2.50 M SrCl 2 will completely react with 0.150 L of a 1.75 M AgNO3 solution? SrCl2(aq) + 2AgNO3(aq) → 2AgCl(s) + Sr(NO3)2(aq) A. 0.0525 L B. 0.210 L C. 0.0686 L D. 0.429 L
What volume of 0.131 M BaCl 2 is required to react completely with 42.0 mL of 0.453 M Na2SO4? The following is the net ionic equation. Ba2+ (aq) + SO42- (aq) → BaSO4(s) A. 12.1 mL B. 72.6 mL C. 145 mL D. 290 mL
When 5.0 grams of Na 2O (MM = 61.98 g/mol) are dissolved in 1.00 L of water, what is the concentration of the Na+ ions? A.  0.040 M     B.  0.080 M     C.  0.16 M     D.  6.2 M     E.  12 M
The SO2 present in air is mainly responsible for the acid rain phenomenon. Its concentration can be determined by titrating against a standard permanganate solution as follows: 5 SO2 + 2 MnO4- + 2 H2O → 5 SO42- + 2 Mn2+ + 4 H+ Calculate the number of grams of SO 2 in a sample of air if 7.37 mL of 0.00800 M KMnO 4 solution are required for the titration.
A 55.0 mL sample of a 0.102 M potassium sulfate solution is mixed with 35.0 mL of a 0.114 M lead (II) acetate solution and this precipitation reaction occurs: K2SO4 (aq) + Pb(C2H3O2)2 (aq)      →       2 KC 2H3O2 (aq) + PbSO4 (s) The solid PbSO4 is collected , dried, and found to have a mass of 1.01 g. Determine the limiting reactant, the theoretical yield, and the percent yield. 
Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 23.65 mL of 0.3000 M NaOH solution to titrate both acidic protons in 55.00 mL of the tartaric acid solution. You may want to reference (Pages 149 - 153) Section 4.6 while completing this problem.Calculate the molarity of the tartaric acid solution.
If 23.9 mL of the strontium hydroxide solution was needed to neutralize a 31.5 mL aliquot of the nitric acid solution, what is the concentration (molarity) of the acid?
You may want to reference (Pages 149 - 153) Section 4.6 while completing this problem.If 45.6 mL of 0.112 M HCl solution is needed to neutralize a solution of KOH, how many grams of KOH must be present in the solution?
You may want to reference(Pages 148 - 153)Section 4.6 while completing this problem.If 56.2 mL of BaCl2 solution is needed to precipitate all the sulfate ion in a 752 mg sample of Na2SO4, what is the molarity of the solution?
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.What is the concentration of Ni2+ that remains in solution?
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.What is the concentration of SO42- that remains in solution?
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.What is the concentration of K+ that remains in solution?
A solution is made by mixing 15.0 g of Sr(OH)2 and 60.0 mL of 0.210 M HNO3. You may want to reference (Pages 149 - 153) Section 4.6 while completing this problem.Calculate the concentration of Sr2+ ion remaining in solution.
A solution is made by mixing 15.0 g of Sr(OH)2 and 60.0 mL of 0.210 M HNO3. You may want to reference (Pages 149 - 153) Section 4.6 while completing this problem.Calculate the concentration of NO3- ion remaining in solution.
Find the volume of 0.120 M hydrochloric acid necessary to react completely with 1.53 g Al(OH)3.
An acid solution is 0.120 M in HCl and 0.210 M in H2 SO4.You may want to reference (Pages 138 - 182) Chapter 4 while completing this problem.What volume of a 0.160 M solution of KOH must be added to 550.0 mL of the acidic solution to completely neutralize all of the acid?        
You want to analyze a silver nitrate solution.You could add HCl(aq) to the solution to precipitate out AgCl(s). What volume of a 0.160 M HCl(aq) solution is needed to precipitate the silver ions from 16.0 mL of a 0.210 M AgNO3 solution?
You may want to reference (Pages 149 - 153) Section 4.6 while completing this problem.What volume of 0.130 M HClO4 solution is needed to neutralize 51.00 mL of 8.75×10−2 M NaOH?
You may want to reference (Pages 149 - 153) Section 4.6 while completing this problem.What volume of 0.132 M HCl is needed to neutralize 2.76 g of Mg(OH)2?
You may want to reference(Pages 148 - 153)Section 4.6 while completing this problem.How many milliliters of 0.130  M  HCl are needed to completely neutralize 51.0 mL of 0.106  M  Ba(OH)2 solution?
You may want to reference(Pages 148 - 153)Section 4.6 while completing this problem.How many milliliters of 0.126  M  H2SO4 are needed to neutralize 0.210 g of NaOH?
A solution contains Cr3 + ion and Mg2 + ion. The addition of 1.00 L of 1.53 M NaF solution is required to cause the complete precipitation of these ions as CrF3 (s) and MgF2 (s). The total mass of the precipitate is 50.0 g .Find the mass of Cr3 + in the original solution.
How many moles of hydrogen gas would be produced for every mole of magnesium added into the HCl solution? Reaction of magnesium metal with hydrochloric acid. The metal is readily oxidized by the acid, producing hydrogen gas, H2(g), and MgCl2(aq).
A solution contains Ag + and Hg2+ ions. The addition of 0.100 L of 1.35 M NaI solution is just enough to precipitate all the ions as AgI and HgI2. The total mass of the precipitate is 31.2 g .Find the mass of AgI in the precipitate.
Lakes that have been acidified by acid rain (HNO3 and H2SO4) can be neutralized by a process called liming, in which limestone (CaCO3 ) is added to the acidified water.What mass of limestone (in kg) would be required to completely neutralize a 15.3 billion-liter lake that is 1.8×10−5 M in H2 SO4 and 8.8×10−6 M in HNO3 ?
Sodium carbonate is often added to laundry detergents to soften hard water and make the detergent more effective. Suppose that a particular detergent mixture is designed to soften hard water that is 3.6×10−3 M in Ca2 + and 1.2×10−3 M in Mg2 + and that the average capacity of a washing machine is 20.0 gallons of water.If the detergent requires using 0.66 kg detergent per load of laundry, determine what percentage (by mass) of the detergent should be sodium carbonate in order to completely precipitate all of the calcium and magnesium ions in an average load of laundry water.
You want to analyze a silver nitrate solution.You could add solid KCl to the solution to precipitate out AgCl(s). What mass of KCl is needed to precipitate the silver ions from 16.0 mL of 0.210 M AgNO3 solution?
A sample of 5.55 g of Mg(OH)2 is added to 25.2 mL of 0.180 M HNO3.Which is the limiting reactant in the reaction?
A sample of 5.55 g of Mg(OH)2 is added to 25.2 mL of 0.180 M HNO3.How many moles of Mg(OH)2 are present after the reaction is complete?
A sample of 5.55 g of Mg(OH)2 is added to 25.2 mL of 0.180 M HNO3.How many moles of HNO3 are present after the reaction is complete?
A sample of 5.55 g of Mg(OH)2 is added to 25.2 mL of 0.180 M HNO3.How many moles of Mg(NO3)2 are present after the reaction is complete?
You may want to reference (Pages 148 - 153)Section 4.6 while completing this problem.How many milligrams of sodium sulfide are needed to completely react with 25.00 mL of a 0.0100 M aqueous solution of cadmium nitrate, to form a precipitate of CdS (s)?
You may want to reference (Pages 149 - 153) Section 4.6 while completing this problem.What mass of NaOH is needed to precipitate the Cd2+ ions from 36.0 mL of 0.510 M Cd(NO3)2 solution?
You may want to reference(Pages 148 - 153)Section 4.6 while completing this problem.If 42.6 mL of 0.212  M  HCl solution is needed to neutralize a solution of Ca(OH)2, how many grams of Ca(OH)2 must be in the solution?
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.What is the limiting reactant?
A solution of 116 mL of 0.180 M KOH is mixed with a solution of 260 mL of 0.210 M NiSO4.How many grams of this precipitate form?
Hard water often contains dissolved Ca2 + and Mg2 + ions. One way to soften water is to add phosphates. The phosphate ion forms insoluble precipitates with calcium and magnesium ions, removing them from solution. A solution is 0.055 M in calcium chloride and 0.090 M in magnesium nitrate.What mass of sodium phosphate would you add to 2.0 L of this solution to completely eliminate the hard water ions? Assume complete reaction.
Consider two solutions, the first being 50.0 mL of 1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5 oC to 27.7 oC.Before mixing, how many grams of Cu are present in the solution of CuSO4?
Consider two solutions, the first being 50.0 mL of 1.00 M CuSO4 and the second 50.0 mL of 2.00 M KOH. When the two solutions are mixed in a constant-pressure calorimeter, a precipitate forms and the temperature of the mixture rises from 21.5 oC to 27.7 oC.Predict the identity of the precipitate in the reaction.
A 36.0 mL sample of 1.30 M KBr and a 61.0 mL sample of 0.610 M KBr are mixed. The solution is then heated to evaporate water until the total volume is 55.0 mL .How many grams of silver nitrate are required to precipitate out silver bromide in the final solution?
Hard water contains Ca2+, Mg2+, and Fe2+, which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with Na+. Keep in mind that charge balance must be maintained.If 1600. L of hard water contains 0.021 M Ca2+ and 0.0050 M Mg2+, how many moles of Na+ is needed to replace these ions?
Hard water contains Ca2+, Mg2+, and Fe2+, which interfere with the action of soap and leave an insoluble coating on the insides of containers and pipes when heated. Water softeners replace these ions with Na+. Keep in mind that charge balance must be maintained.If the sodium is added to the water softener in the form of NaCl, how many grams of sodium chloride are needed?
How many grams of barium phosphate (molar mass= 601.93 g ) are produced by mixing 209.28 mL of 0.182 M barium nitrate with 127.80 mL of 0.173 M sodium phosphate?  3Ba(NO3)2 + 2Na 3PO4 → Ba3(PO4)2 + 6NaNO3A) 7.64 gramsB) 13.3 gramsC) 6.65 gramsD) 4.44 gramsE) 22.9 grams
Calculate the amount, in mL, of 0.0168 M Ca(OH) 2 that would be required to completely react with 25.38 mL of 0.0784 M HClO3.A) 5.44 mLB) 59.22 mLC) 236.88 mLD) 2.72 mLE) 10.88 mL
Solid calcium bicarbonate (Ca(HCO3)2) reacts with aqueous hydrochloric acid (HCl) to form aqueous calcium chloride, liquid water, and carbon dioxide gas.What is the minimum amount of 0.2102 M hydrochloric acid (in milliliters) required to completely react with 8.362 g calcium bicarbonate?
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation.     2AgNO3(aq)+MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)a) What mass of silver chloride can be producd from 1.49L of a 0.254M solution of silver nitrate?b) The reaction described in Part A required 4.00L of magnesium chloride. What is the concentration of this magnesium chloride solution?
Zinc reacts with hydrochloric acid according to the reaction equation:Zn + 2HCl → ZnCl2 + H2How many milliliters of 5.50 M HCl(aq) are required to react with 3.65 g of an ore containing 33.0% Zn(s) by mass?
30.mL of 0.10 M Ca(NO3)2 and 15.0 mL of 0.20 M Na 3PO4 solutions are mixed. After the reaction is complete, which of these ions has the lowest concentration in the final solution?a) Na+b) NO3–c) Ca2+d) PO43–
ln an acid-base titration, a 20.0 mL HCI solution of unknown concentration requires 15.6 mL of a 0.250 M NaOH solution to reach the equivalence point. What is the concentration (M) of the unknown HCI solution? HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq)A. 12.1 MB. 72.6 MC. 320 MD. 0.195 M
Pb(NO3)2 (aq) + 2NH4I(aq) → PbI2(s) + 2NH4NO3(aq)a) What volume of a 0.110 M NH4I solution is required to react with 923 mL of a 0.480 M Pb(NO 3)2 solution?b) How many moles of PbI2 are formed from this reaction?
A sample of CO32- antacid is dissolved with 25.0mL of 0.0981M HCl. The hydrochloric acid that is not neutralized by the antacid is titrated to a bromophenol endpoint with 5.83mL of 0.104M NaOH. Calculate the number of moles of base in the antacid.
We use 625. mL of a sodium hydroxide, NaOH, solution to completely neutralize 4.50 grams of phosphoric acid.a. What is the molarity of the NaOH solution?    b. What are the name and the mass of the salt that forms?
What volume of 0.405 M KOH solution is needed to react completely with 2.15 g of copper (II) sulfate, CuSO4? The products of the chemical reaction are copper (II) hydroxide and potassium sulfate.
How many moles of Ca(OH)2 are needed to neutralize three moles of HCl?21.513
20.0 mL of a 0.10 M solution of a diprotic acid (H 2A) are titrated with 0.20 M NaOH. How many mL of this NaOH solution are required to completely neutralize this acid solution?a. 25.0b. 20.0c. 15.0d. 10.0e. 5.00
What mass of Na2CrO4 is required to precipitate all of the silver ions from 75.0 mL of a 0.100 M solution of AgNO3?
What volume of 0.100 M Na3PO4 is required to precipitate all the lead(II) ions from 150.0 mL of 0.250 M Pb(NO3)2?
What mass of solid aluminum hydroxide can be produced when 50.0 mL of 0.200 M Al(NO3)3 is added to 200.0 mL of 0.100 M KOH?
What mass of barium sulfate can be produced when 100.0 mL of a 0.100 M solution of barium chloride is mixed with 100.0 mL of a 0.100 M solution of iron(III) sulfate?
What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO 3 is added to 20.0 mL of 1.00 M NaBr?
What is the molar mass of a 0.350 g sample of a monoprotic acid if it requires 50.0 mL of 0.440 M Ca(OH)2 to completely neutralize it? 
What volume of 3.05 M HCl(aq) will react with 25.0 g Zn(s)? Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)a. 0.251 Lb. 4.01 Lc. 0.125 Ld. 0.0627 Le. 2.33 L  
Sodium hydrogen carbonate (NaHCO 3), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCl), which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction:HCl (aq) + NaHCO3 (aq) → NaCl (aq) + H 2O (I) + CO2 (g)The CO2 gas produced is what makes you burp after drinking the solution.Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 50 mL of a 0.034 M HCl solution. What mass of NaHCO3 would he need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.c. Calculate the percent sodium chloride in the original unknown mixture.
Vinegar is a solution of acetic acid, CH 3COOH, dissolved in water. A 5.54 g sample of vinegar was neutralized by 30.10 mL of 0.100 M NaOH. What is the percent by weight of acetic acid in the vinegar?a) 24.4 %b) 0.109 %c) 3.26 %d) 9.79 %
What is the molar mass of a 0.350 g sample of a monoprotic acid if it requires 50.0 mL of 0.440 M Ca(OH)2 to completely neutralize it? a) 5.30 g/molb) 7.95 g/molc) 31.8 g/mold) 47.7 g/mol
How much 0.5685 M nitric acid, HNO 3, solution would a student need to use to neutralize 0.8232 g of Al(OH)3?a. 37.12 mLb. 18.56 mLc. 32.92 mLd. 55.69 mLe.47.48 mL
According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.210 M Pb(NO3)2 solution?2 KCl(aq) + Pb(NO3)2 (aq) → PbCl2(s) + 2 KNO3(aq)A) 97.4 mLB) 116 mLC) 43.0 mLD) 86.1 mLE) 58.1 mL
If 340 mL of 0.0824 M aqueous Ba 2+ and 230 mL of 0.253 M aqueous H + are reacted, how many mol of liquid H2O is produced?Ba(OH)2(aq) + 2HClO4(aq) → Ba(ClO4)2(aq) + 2H2O(l)
What mass of KCl is needed to precipitate the silver ions from 15.0 mL of 0.200 M AgNO3 solution?
According to the following reaction, how many moles of Fe(OH) 2 can form from 175.0 mL of 0.227 M LiOH solution? Assume that there is excess FeCl2.FeCl2(aq) + 2 LiOH(aq) → Fe(OH) 2(s) + 2 LiCl(aq)A) 3.97 × 10-2 molesB) 2.52 × 10-2 molesC) 1.99 × 10-2 molesD) 5.03 × 10-2 molesE) 6.49 × 10-2 moles
It requires 23.56 mL of 0.105 M sodium hydroxide to neutralize 15.00 mL of a sulfuric acid (H2SO4) solution. Determine the concentration of the sulfuric acid (H2SO4) solution.       The titration of 25.0 mL of an H 2SO4 solution of unknown concentration requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H2SO4 solution?
What mass of NaOH is needed to precipitate the Cd  2+ ions from 35.0 mL of 0.500 M Cd(NO3)2 solution?
(a) How many milliliters of 0.120 M HCl are needed to completely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution?
(b) How many milliliters of 0.125 M H 2SO4 are needed to neutralize 0.200 g of NaOH?
A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?
What is the molarity of a NaOH solution if 23.6 mL are needed to titrate a 0.5116g sample of KHP?
What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?a. 0.100 M NaOH
What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?b. 0.0500 M Ba(OH)2
What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?b. 0.0500 M Sr(OH)2
What volume of each of the following bases will react completely with 25.00 mL of 0.200 M HCl?c. 0.250 M KOH
Given the precipitation of AgCl from a NaCl solution using silver nitrate:AgNO3 + NaCl(aq) →  AgCl(s) + NaNO3(aq)If a solution of AgNO3 of unknown molarity is added to a flask containing 132ml of NaCl solution also of unknown molarity. At the endpoint 42.15 ml of the AgNO3 solution have been added and 8.42 g of AgCl are recovered as a precipitate from the reaction:a) What is the molarity of the NaCl solution?  b) What is the molarity of AgNO3 solution? 
Determine the number of grams of H 2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 x 1023 atoms of Fe according to the following reaction.2 HCl(aq) + Fe(s) → H 2(g) + FeCl 2(aq)A) 0.374 gB) 1.33 gC) 1.14 gD) 0.187 gE) 1.51 g
Calculate the molarity of each of these solutions.c. A 0.1025-g sample of copper metal is dissolved in 35 mL of concentrated HNO 3 to form Cu2+ ions and then water is added to make a total volume of 200.0 mL. (Calculate the molarity of Cu2+.)
A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?
How many mL of 0.200 M H2SO4 (aq) must be added to 25.0 mL of 0.0888 M BaCl2 (aq) to precipitate all the barium as barium sulfate?a) 22.2 mLb) 25.0 mLc) 9.01 mLd) 5.55 mLe) 11.1 mL
A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.a. What is the molarity of the acetic acid?
Solid sodium hydroxide reacts with phosphoric acid according to the following equation: 3NaOH (s) + H3PO4 (aq) → Na 3PO4 (aq) + 3H 2O (l) What volume (in ml) of 0.0160 M phosphoric acid can be neutralized by 64.531 grams of sodium hydroxide? [molar masses: NaOH = 40.00 g/mole; H3PO4 = 98.00g/mole]
What volume of 0.0521 M Ba(OH) 2 is required to neutralize exactly 14.20 mL of 0.141 M H3PO4? Phosphoric acid contains three acidic hydrogens.
A 10.00-mL sample of sulfuric acid from an automobile battery requires 35.08 mL of 2.12 M sodium hydroxide solution for complete neutralization. What is the molarity of the sulfuric acid? Sulfuric acid contains two acidic hydrogens.
A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point.b. If the density of the vinegar is 1.006 g/cm 3, what is the mass percent of acetic acid in the vinegar?
A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of 0.213 M NaOH. After the reaction occurred, an excess of OH– ions remained in the solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. Sulfuric acid has two acidic hydrogens.
A 6.50-g sample of a diprotic acid requires 137.5 mL of a 0.750 M NaOH solution for complete reaction. Determine the molar mass of the acid.
Citric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?
How do you calculate the mass of KHC8H4O4 (molar mass=204.44 g/mol) that reacts with 15mL of 0.16 M NaOH solution ?
What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?
Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid-base titrations. If 19.15 mL of NaOH is required to neutralize 0.442 g of KHP, what is the concentration of NaOH?
A 30.0-mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M HNO3 solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.
Zinc reacts with hydrochloric acid according to the reaction equation:Zn(s) + 2HCl(aq) → ZnCl 2(aq) + H2(g)How many milliliters of 2.50 M HCl(aq) are required to react with 8.15 g of Zn(s)?
The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.
The following equation is unbalanced.HNO3 + Ba(OH)2 → Ba(NO3)2 + H2OIf 12.0 mL of 0.600M of HNO3 solution reacts with 30.0 mL of 0.700M Ba(OH)2 solution, what is the molarity of Ba(OH)2 after the reaction is completed?
2HNO3(aq) + Ba(OH)2(aq) → 2H2O(l) + Ba(NO3)2(aq)0.1155 L sample of an unknown HNO3 solution required 42.9 mL of .10 M of Ba(OH) 2 for complete neutralization. What was the concentration of the HNO3 solution?
Zinc reacts with hydrochloric acid according to the reaction equationZn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)How many milliliters of 6.00 M HCl(aq) are required to react with 5.65 g of Zn(s)?
A solution of hydrochloric acid is to be neutralized by using a 0.15 M solution of barium hydroxide. 25.0 mL of the HCl solution requires 33.3 mL of the Ba(OH)2 solution. What is the molarity of the HCl solution?A. 0.40 MB. 0.11 MC. 0.15 MD. 0.20 ME. 0.22 M
According to the following reaction, how many moles of Fe(OH) 2 can form from 175.0 mL of 0.2 M LiOH solution? Assume that there is excess FeCl2. FeCl2 (aq) + 2LiOH (aq) → Fe(OH) 2 (s) + 2LiCl (aq) a. 5.03 x 10- 2 moles b. 1.75 x 10 -2 moles c. 2.52 x 10 -2 moles d. 6.49 x 10 -2 moles e. 3.97 x 10 -2 moles
What volume of 0.305 M AgNO3 is required to react exactly with 155.0 mL of 0.274 M Na2SO4 solution? 
A 27.6-mL sample of a 1.62 M potassium chloride solution is mixed with 14.6 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs:2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)The solid PbCl2 is collected, dried, and found to have a mass of 2.56 g. Determine the limiting reactant, the theoretical yield, and the percent yield.Determine the limiting reactant.
A 27.6-mL sample of a 1.62 M potassium chloride solution is mixed with 14.6 mL of a 0.890 M lead(II) nitrate solution and this precipitation reaction occurs:2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)The solid PbCl2 is collected, dried, and found to have a mass of 2.56 g. Determine the limiting reactant, the theoretical yield, and the percent yield.Determine the percent yield.
You may want to reference (Pages 152 - 157)Section 4.4 while completing this problem.A 60.5 mL sample of a 0.114 M potassium sulfate solution is mixed with 37.5 mL of a 0.116 M lead(II) acetate solution and the following precipitation reaction occurs:K2SO4(aq) + Pb(C2H3O2)2(aq) → 2KC2H3O2(aq) + PbSO4(s)The solid PbSO4 is collected, dried, and found to have a mass of 1.00 g .Determine the limiting reactant, the theoretical yield, and the percent yield.
Mixtures of CaCl2 and NaCl are used to melt ice on roads. A dissolved 1.9348-g sample of such a mixture was analyzed by using excess Na2C2O4 to precipitate the Ca2+ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid, and the resulting H2C2O4 was titrated with 37.68 mL of 0.1019 M KMnO4 solution.Calculate the mass percent of CaCl2 in the original sample.
Concentrated sulfuric acid (18.3 M) has a density of 1.84 g/mL.What is the mass % of H2SO4 in the solution?
A person’s blood alcohol (C2H5OH) level can be determined by titrating a sample of blood plasma with a potassium dichromate solution. The balanced equation is16 H+  (aq) + 2 Cr2O7 2−(aq) + C2H5OH(aq) ⟶ 4 Cr3+(aq) + 2 CO2(g) + 11 H2O(l)If 35.46 mL of 0.05961 M Cr2O7 2− is required to titrate 28.00 g of plasma, what is the mass percent of alcohol in the blood?
When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2 formed can be determined by the reaction with hydrogen peroxide:H2O2 (aq) + SO 2 (g) → H2SO4 (aq)The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.302-g sample of coal is burned and the SO2 is collected in a solution of hydrogen peroxide. It took 28.44 mL of a 0.1000-M NaOH solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.
The mass percent of Cl− in a seawater sample is determined by titrating 25.00 mL of seawater with AgNO3 solution, causing a precipitation reaction. An indicator is used to detect the end point, which occurs when free Ag+ ion is present in solution after all the Cl− has reacted. If 53.63 mL of 0.2970 M AgNO3 is required to reach the end point, what is the mass percent of Cl− in the seawater (d of seawater = 1.024 g/mL)?
An unknown amount of acid can often be determined by adding an excess of base and then “back-titrating” the excess. A 0.3471-g sample of a mixture of oxalic acid, which has two ionizable protons, and benzoic acid, which has one, is treated with 100.0 mL of 0.1000 M NaOH. The excess NaOH is titrated with 20.00 mL of 0.2000 M HCl. Find the mass % of benzoic acid
A mixture of bases can sometimes be the active ingredient in antacid tablets. If 0.4826 g of a mixture of Al(OH)3 and Mg(OH)2 is neutralized with 17.30 mL of 1.000 M HNO3, what is the mass % of Al(OH)3 in the mixture?
A sample of impure magnesium was analyzed by allowing it to react with excess HCl solution. After 1.32 g of the impure metal was treated with 0.100 L of 0.750 M HCl, 0.0125 mol of HCl remained. Assuming the impurities do not react, what is the mass % of Mg in the sample?
What mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate with 100.0 mL of 0.15 M calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.
On a lab exam, you have to find the concentrations of the monoprotic (one proton per molecule) acids HA and HB. You are given 43.5 mL of HA solution in one flask. A second flask contains 37.2 mL of HA, and you add enough HB solution to it to reach a final volume of 50.0 mL. You titrate the first HA solution with 87.3 mL of 0.0906 M NaOH and the mixture of HA and HB in the second flask with 96.4 mL of the NaOH solution. Calculate the molarity of the HA and HB solutions.
A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass.What is the molarity of the solution?
A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. Calculate the concentration of each ion remaining in solution after precipitation is complete.
The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potassium hydroxide.Determine the concentrations (in M) of all ions left in solution after mixing and the mass of solid formed.
Two aqueous solutions contain the ions indicated below.What is the concentration of each ion in solution after reaction?
To study a marine organism, a biologist prepares a 1.00-kg sample to simulate the ion concentrations in seawater. She mixes 26.5 g of NaCl, 2.40 g of MgCl2, 3.35 g of MgSO4, 1.20 g of CaCl2, 1.05 g of KCl, 0.315 g of NaHCO3, and 0.098 g of NaBr in distilled water.If the density of the solution is 1.025 g/cm3 , what is the molarity of each ion?
To study a marine organism, a biologist prepares a 1.00-kg sample to simulate the ion concentrations in seawater. She mixes 26.5 g of NaCl, 2.40 g of MgCl2, 3.35 g of MgSO4, 1.20 g of CaCl2, 1.05 g of KCl, 0.315 g of NaHCO3, and 0.098 g of NaBr in distilled water.What is the total molarity of alkali metal ions?
To study a marine organism, a biologist prepares a 1.00-kg sample to simulate the ion concentrations in seawater. She mixes 26.5 g of NaCl, 2.40 g of MgCl2, 3.35 g of MgSO4, 1.20 g of CaCl2, 1.05 g of KCl, 0.315 g of NaHCO3, and 0.098 g of NaBr in distilled water.What is the total molarity of alkaline earth metal ions?
To study a marine organism, a biologist prepares a 1.00-kg sample to simulate the ion concentrations in seawater. She mixes 26.5 g of NaCl, 2.40 g of MgCl2, 3.35 g of MgSO4, 1.20 g of CaCl2, 1.05 g of KCl, 0.315 g of NaHCO3, and 0.098 g of NaBr in distilled water.What is the total molarity of anions?
A 25.00-mL sample of hydrochloric acid solution requires 24.16 mL of 0.106 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?
A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point. What is the molarity of the acetic acid?
The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of 204.22 g/mol. In the titration, 34.67 mL of the sodium hydroxide solution was required to react with 0.1082 g KHP. Calculate the molarity of the sodium hydroxide.
If 38.5 mL of lead(II) nitrate solution reacts completely with excess sodium iodide solution to yield 0.628 g of precipitate, what is the molarity of lead(II) ion in the original solution?
If 25.0 mL of silver nitrate solution reacts with excess potassium chloride solution to yield 0.842 g of precipitate, what is the molarity of silver ion in the original solution?
A 50.00-mL sample of aqueous Ca(OH) 2 requires 34.66 mL of a 0.944-M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide.
Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.0811 M NaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration of sulfuric acid in this sample of rain?
What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO3 requires 20.22 mL of the AgNO3 solution to reach the end point?AgNO3(aq) + NaCl(aq) ⟶ AgCl(s) + NaNO3(aq)
In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO3)2 solution.2Cl−(aq) + Hg(NO3)2(aq) ⟶ 2NO3−(aq) + HgCl2(s)What is the Cl− concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of 8.25 × 10−4 M Hg(NO3)2(aq) to reach the end point?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00 × 10−2 M HCl requires 36.6 mL of the acid to reach the end point.Ca(OH)2(aq) + 2HCl(aq) ⟶ CaCl2(aq) + 2H2O(l)What is the molarity?
Potassium acid phthalate, KNaC8H4O4, or KHP, is used in many laboratories, including general chemistry laboratories, to standardize solutions of base. KHP is one of only a few stable solid acids that can be dried by warming and weighed. A 0.3420-g sample of KNaC8H4O4 reacts with 35.73 mL of a NaOH solution in a titration. What is the molar concentration of the NaOH?KNaC8H4O4(aq) + NaOH(aq) ⟶ KNaC8H4O4(aq) + H2O(aq)
If 25.98 mL of 0.1180 M KOH solution reacts with 52.50 mL of CH3COOH solution, what is the molarity of the acid solution?
If 26.25 mL of 0.1850 M NaOH solution reacts with 25.00 mL of H2SO4, what is the molarity of the acid solution?
Sodium hydroxide is used extensively in acid-base titrations because it is a strong, inexpensive base. A sodium hydroxide solution was standardized by titrating 25.00 mL of 0.1528 M standard hydrochloric acid. The initial buret reading of the sodium hydroxide was 2.24 mL, and the final reading was 39.21 mL. What was the molarity of the base solution?
A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe2+ in acid and then titrating the Fe2+ with MnO4−. A 1.1081-g ore sample was dissolved in acid and then titrated with 39.32 mL of 0.03190 M KMnO4. The balanced equation is8 H+(aq) + 5 Fe2+(aq) + MnO4−(aq) ⟶ 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(l) Calculate the mass percent of iron in the ore.
What volume of 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid?NaCl(s) + H2SO4(l) ⟶ HCl(g) + NaHSO4(s)
What volume of a 0.2089 M KI solution contains enough KI to react exactly with the Cu(NO3)2 in 43.88 mL of a 0.3842 M solution of Cu(NO 3)2? 2Cu(NO3)2 + 4KI ⟶ 2CuI + I 2 + 4KNO3
Muriatic acid, an industrial grade of concentrated HCl, is used to clean masonry and cement. Its concentration is 11.7 M.How many milliliters of the muriatic acid solution contain 9.66 g of HCl?
Potassium iodide reacts with lead(II) nitrate in the following precipitation reaction:2 KI(aq) + Pb(NO3)2(aq) → 2 KNO3(aq) + PbI2(s)You may want to reference (Page 156) Section 4.4 while completing this problem.What minimum volume of 0.200 M potassium iodide solution is required to completely precipitate all of the lead in 155.0 mL of a 0.112 M lead(II) nitrate solution?
What volume of 0.100 M HCl will react completely with 50.00 mL of 0.200 M NaOH?
What volume of 0.150 M HNO 3 will react completely with 50.00 mL of 0.200 M NaOH?
What volume of 0.200 M HC 2H3O2 (1 acidic hydrogen) will react completely with 50.00 mL of 0.200 M NaOH?
What volume of 0.100 M NaOH will react completely with 25.00 mL of 0.200 M HCl?
What volume of 0.0500 M Sr(OH)2 will react completely with 25.00 mL of 0.200 M HCl?
What volume of 0.250 M KOH will react completely with 25.00 mL of 0.200 M HCl?
What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric acid?
When hydrochloric acid reacts with magnesium metal, hydrogen gas and aqueous magnesium chloride are produced. What volume of 5.0 M HCl is required to react completely with 3.00 g of magnesium?
What volume of 0.0105-M HBr solution is required to titrate 125 mL of a 0.0100-M Ca(OH)2 solution?Ca(OH)2(aq) + 2HBr(aq) ⟶ CaBr2(aq) + 2H2O(l)
You may want to reference (Pages 152 - 157) Section 4.4 while completing this problem.What volume (in mL) of a 0.175 M HNO3 solution is required to completely react with 35.1 mL of a 0.112 M Na2CO3 solution according to the following balanced chemical equation?Na2CO3(aq) + 2 HNO3(aq) → 2 NaNO3(aq) + CO2(g) + H2O(l)
Consider the following precipitation reaction: 2 Na3PO4(aq) + 3 CuCl2(aq) → Cu3(PO4)2(s) + 6 NaCl(aq) ;{ m{Cu}}_3 ({ m{PO}}_4 )_2 (s); + ;6;{ m{NaCl}}(aq)What volume of 0.176 M Na3PO4 solution is necessary to completely react with 90.5 mL of 0.113 M CuCl2?
Consider the following reaction: Li2S(aq) + Co(NO3)2(aq) → 2 LiNO3(aq) + CoS(s)What volume of 0.160 M Li2S solution is required to completely react with 130 mL of 0.160 M Co(NO3)2?
What is the minimum amount of 6.1 M H2SO4 necessary to produce 25.1 g of H2(g) according to the following reaction? 2 Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g)
Potatoes can be peeled commercially by soaking them in a 3-M to 6-M solution of sodium hydroxide, then removing the loosened skins by spraying them with water. Does a sodium hydroxide solution have a suitable concentration if titration of 12.00 mL of the solution requires 30.6 mL of 1.65 M HCI to reach the end point?
What volume of 0.600 M HCl is required to react completely with 2.50 g of sodium hydrogen carbonate?NaHCO3(aq) + HCl(aq) ⟶ NaCl(aq) + CO2(g) + H2O(l)
What volume of 0.08892 M HNO3 is required to react completely with 0.2352 g of potassium hydrogen phosphate?2HNO3(aq) + K2HPO4(aq) ⟶ H2PO4(aq) + 2KNO3(aq)
What volume of a 0.3300-M solution of sodium hydroxide would be required to titrate 15.00 mL of 0.1500 M oxalic acid?C2O4H2(aq) + 2NaOH(aq) ⟶ Na2C2O4(aq) + 2H2O(l)
What volume of a 0.00945-M solution of potassium hydroxide would be required to titrate 50.00 mL of a sample of acid rain with a H2SO4 concentration of 1.23 × 10−4 M.H2SO4(aq) + 2KOH(aq) ⟶ K2SO4(aq) + 2H2O(l)
How many milliliters of a 0.1500-M solution of KOH will be required to titrate 40.00 mL of a 0.0656-M solution of H3PO4?H3PO4(aq) + 2KOH(aq) ⟶ K2HPO4(aq) + 2H2O(l)
How many milliliters of 0.383 M HCl are needed to react with 16.2 g of CaCO3?2 HCl(aq) + CaCO3(s) ⟶ CaCl2(aq) + CO2(g) + H2O(l)
An auto mechanic spills 88 mL of 2.6 M H2SO4 solution from an auto battery. How many milliliters of 1.6 M NaHCO3 must be poured on the spill to react completely with the sulfuric acid?
One of the first steps in the enrichment of uranium for use in nuclear power plants involves a displacement reaction between UO2 and aqueous HF:UO2(s) + HF(aq)⟶ UF4(s) + H2O(l) [unbalanced]How many liters of 2.40 M HF will react with 2.15 kg of UO2?
A 1.42-g sample of a pure compound, with formula M 2SO4, was dissolved in water and treated with an excess of aqueous calcium chloride, resulting in the precipitation of all the sulfate ions as calcium sulfate. The precipitate was collected, dried, and found to weigh 1.36 g. Determine the atomic mass of M, and identify M.
You are given a 1.50-g mixture of sodium nitrate and sodium chloride. You dissolve this mixture into 100 mL of water and then add an excess of 0.500 M silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of 0.641 g.Calculate the percent sodium chloride in the original unknown mixture.
Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. The mass of the white precipitate formed is 0.641 g. Calculate the mass percent of magnesium chloride in the mixture.
Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. The mass of the white precipitate formed is 0.641 g. Determine the minimum volume of silver nitrate that must have been added to ensure complete formation of the precipitate.
A 1.00-g sample of an alkaline earth metal chloride is treated with excess silver nitrate. All of the chloride is recovered as 1.38 g of silver chloride. Identify the metal.
A mixture contains only NaCl and Al 2(SO4)3. A 1.45-g sample of the mixture is dissolved in water and an excess of NaOH is added, producing a precipitate of Al(OH)3. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.107 g. What is the mass percent of Al2(SO4)3 in the sample?
The thallium (present as Tl 2SO4) in a 9.486-g pesticide sample was precipitated as thallium(I) iodide. Calculate the mass percent of Tl 2SO4 in the sample if 0.1824 g of TlI was recovered.
A mixture contains only NaCl and Fe(NO 3)3. A 0.456-g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is filtered, dried, and weighed. Its mass is 0.107 g. Calculate the mass of iron in the sample.
A mixture contains only NaCl and Fe(NO 3)3. A 0.456-g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is filtered, dried, and weighed. Its mass is 0.107 g. Calculate the mass of Fe(NO3)3 in the sample.
A mixture contains only NaCl and Fe(NO 3)3. A 0.456-g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Fe(OH)3. The precipitate is filtered, dried, and weighed. Its mass is 0.107 g. Calculate the mass percent of Fe(NO3)3 in the sample.
A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then treated with an excess of aqueous chromium(III) nitrate, resulting in formation of 2.06 g of precipitate. Determine the concentration of the NaOH solution.
Chlorisondamine chloride (C14H20Cl6N2) is a drug used in the treatment of hypertension. A 1.28-g sample of a medication containing the drug was treated to destroy the organic material and to release all the chlorine as chloride ion. When the filtered solution containing chloride ion was treated with an excess of silver nitrate, 0.104 g silver chloride was recovered.  Calculate the mass percent of chlorisondamine chloride in the medication, assuming the drug is the only source of chloride.
Saccharin (C7H5NO3S) is sometimes dispensed in tablet form. Ten tablets with a total mass of 0.5894 g were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of BaSO4 obtained was 0.5032 g. What is the average mass of saccharin per tablet? What is the average mass percent of saccharin in the tablets?
Douglasite is a mineral with the formula 2 KCl • FeCl 2 • 2 H2O. Calculate the mass percent of douglasite in a 455.0-mg sample if it took 37.20 mL of a 0.1000-M AgNO3 solution to precipitate all the Cl2 as AgCl. Assume the douglasite is the only source of chloride ion.
What volume of 0.100 M NaOH is required to precipitate all of the nickel(II) ions from 150.0 mL of a 0.249-M solution of Ni(NO3)2?
A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?
A 450.0-mL sample of a 0.257-M solution of silver nitrate is mixed with 400.0 mL of 0.200 M calcium chloride. What is the concentration of Cl2 in solution after the reaction is complete?
H2 is produced by the reaction of 118.5 mL of a 0.8775-M solution of H 3PO4 according to the following equation: 2Cr + 2H3PO4 ⟶ 3H2 + 2CrPO4.(b) Perform the calculations outlined.
Gallium chloride is formed by the reaction of 2.6 L of a 1.44 M solution of HCl according to the following equation: 2Ga + 6HCl ⟶  2GaCl3 + 3H2.(a) Outline the steps necessary to determine the number of moles and mass of gallium chloride.
Gallium chloride is formed by the reaction of 2.6 L of a 1.44 M solution of HCl according to the following equation: 2Ga + 6HCl ⟶  2GaCl3 + 3H2.(b) Perform the calculations outlined.
What mass of barium sulfate can be produced when 100.0 mL of a 0.100-M solution of barium chloride is mixed with 100.0 mL of a 0.100-M solution of iron(III) sulfate?
The flask represents the products of the titration of 25 mL of sulfuric acid with 25 mL of sodium hydroxide.If each orange sphere represents 0.010 mol of sulfate ion, how many moles of acid and of base reacted?
What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO  3 is added to 20.0 mL of 1.00 M NaBr?
To find the mass percent of dolomite [CaMg(CO3)2] in a soil sample, a geochemist titrates 13.86 g of soil with 33.56 mL of 0.2516 M HCl. What is the mass percent of dolomite in the soil?
A sample of concentrated nitric acid has a density of 1.41 g/mL and contains 70.0% HNO3 by mass.What mass (g) of HNO3 is present per liter of solution?
A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. What mass of precipitate is produced?
Concentrated sulfuric acid (18.3 M) has a density of 1.84 g/mL.How many moles of H2SO4 are in each milliliter of solution?
Two aqueous solutions contain the ions indicated below.If each sphere represents 0.050 mol of ion, what mass (in g) of precipitate forms, assuming 100% yield?
A mordant is a substance that combines with a dye to produce a stable fixed color in a dyed fabric. Calcium acetate is used as a mordant. It is prepared by the reaction of acetic acid with calcium hydroxide.2CH3CO2 H + Ca(OH)2 ⟶ Ca(CH3CO2)2 + 2H2OWhat mass of Ca(OH)2 is required to react with the acetic acid in 25.0 mL of a solution having a density of 1.065 g/mL and containing 58.0% acetic acid by mass?
The amount of ascorbic acid (vitamin C; C6H8O6) in tablets is determined by reaction with bromine and then titration of the hydrobromic acid with standard base: C6H8O6(aq) + Br2(aq) ⟶ C6H6O6(aq) + 2 HBr(aq)HBr(aq) + NaOH(aq) ⟶ NaBr(aq) + H2O(l)A certain tablet is advertised as containing 500 mg of vitamin C. One tablet was dissolved in water and reacted with Br2. The solution was then titrated with 43.20 mL of 0.1350 M NaOH. Did the tablet contain the advertised quantity of vitamin C?
In the process of salting-in, protein solubility in a dilute salt solution is increased by adding more salt. Because the protein solubility depends on the total ion concentration as well as the ion charge, salts containing doubly charged ions are often more effective at increasing the protein solubility than those containing singly charged ions.How many grams of MgCl2 must dissolve to equal the ion concentration of 12.4 g of NaCl?
Water “softeners” remove metal ions such as Ca2+ and Fe3+ by replacing them with enough Na+ ions to maintain the same number of positive charges in the solution. If 1.0×103 L of “hard” water is 0.015 M Ca2+ and 0.0010 M Fe3+, how many moles of Na+ are needed to replace these ions?
The active agent in many hair bleaches is hydrogen peroxide. The amount of H2O2 in 14.8 g of hair bleach was determined by titration with a standard potassium permanganate solution:2 MnO4 −(aq) + 5 H2O2(aq) + 6 H+(aq) ⟶ 5 O2(g) + 2 Mn2+(aq) + 8 H2O(l) How many moles of MnO4−  were required for the titration if 43.2 mL of 0.105 M KMnO4 was needed to reach the end point?
A 10.00-mL sample of vinegar, an aqueous solution of acetic acid (HC 2H3O2), is titrated with 0.5062 M NaOH, and 16.58 mL is required to reach the equivalence point. If the density of the vinegar is 1.006 g/cm3, what is the mass percent of acetic acid in the vinegar?
Acetylsalicylic acid is the active ingredient in aspirin. It took 35.17 mL of 0.5065 M sodium hydroxide to react completely with 3.210 g of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?
A 30.0-mL sample of an unknown strong base is neutralized after the addition of 12.0 mL of a 0.150 M HNO3 solution. If the unknown base concentration is 0.0300 M, give some possible identities for the unknown base.
A 2.20-g sample of an unknown acid (empirical formula = C 3H4O3) is dissolved in 1.0 L of water. A titration required 25.0 mL of 0.500 M NaOH to react completely with all the acid present. Assuming the unknown acid has one acidic proton per molecule, what is the molecular formula of the unknown acid?
A student titrates an unknown amount of potassium hydrogen phthalate (KHC 8H4O4, often abbreviated KHP) with 20.46 mL of a 0.1000-M NaOH solution. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?
Carminic acid, a naturally occurring red pigment extracted from the cochineal insect, contains only carbon, hydrogen, and oxygen. It was commonly used as a dye in the first half of the nineteenth century. It is 53.66% C and 4.09% H by mass. A titration required 18.02 mL of 0.0406 M NaOH to neutralize 0.3602 g carminic acid. Assuming that there is only one acidic hydrogen per molecule, what is the molecular formula of carminic acid?
How many grams of barium sulfate form when 35.0 mL of 0.160 M barium chloride reacts with 58.0 mL of 0.065 M sodium sulfate?
How many grams of iron(III) sulfide form when 62.0 mL of 0.135 M iron(III) chloride reacts with 45.0 mL of 0.285 M calcium sulfide?
With ions shown as spheres and solvent molecules omitted for clarity, the circle illustrates the solid formed when a solution containing K+, Mg2+, Ag+, or Pb2+ (blue) is mixed with one containing ClO4 −, NO3 −, or SO4 2− (yellow).If each sphere represents 5.0×10−4 mol of ion, what mass of product forms?
The precipitation reaction between 25.0 mL of a solution containing a cation (purple) and 35.0 mL of a solution containing an anion (green) is depicted below (with ions shown as spheres and solvent molecules omitted for clarity).If each sphere represents 2.5×10−3 mol of ion, find the total number of ions present.
A 1.50-g sample of an unknown alkali-metal carbonate was dissolved in water, and 31.10 mL of 0.350 M CaCl2 was required to precipitate all the carbonate ions as CaCO3. Give the name and formula of the unknown compound.
A 0.750-g sample of a compound that might be iron(II) chloride, nickel(II) chloride, or zinc chloride is dissolved in water, and 22.40 mL of 0.515 M AgNO3 is required to completely precipitate all the chloride ion as AgCl. Name the compound, and write its formula.
Aluminum sulfate, known as cake alum, has a wide range of uses, from dyeing leather and cloth to purifying sewage. In aqueous solution, it reacts with base to form a white precipitate.What mass of precipitate forms when 185.5 mL of 0.533 M NaOH is added to 627 mL of a solution that contains 15.8 g of aluminum sulfate per liter?
The reaction of  WCl6 with Al at ~400 °C gives black crystals of a compound containing only tungsten and chlorine. A sample of this compound, when reduced with hydrogen, gives 0.2232 g of tungsten metal and hydrogen chloride, which is absorbed in water. Titration of the hydrochloric acid thus produced requires 46.2 mL of 0.1051 M NaOH to reach the end point. What is the empirical formula of the black tungsten chloride?
Consider the reaction:2A(aq) + B(aq) → C(aq)What is the limiting reactant if you mix equal volumes of a 6 M solution of A and a 6 M solution of B?
How many grams of NaH2PO4 are needed to react with 43.74 mL of 0.285 M NaOH?NaH2PO4(s) + 2 NaOH(aq)⟶ Na3PO4(aq) + 2 H2O(l)
H2 is produced by the reaction of 118.5 mL of a 0.8775-M solution of H3PO4 according to the following equation: 2Cr + 2H3PO4 ⟶ 3H2 + 2CrPO4.(a) Outline the steps necessary to determine the number of moles and mass of H2.
How many grams of PbCl2 are formed when 25.0 mL of 0.614 M KCl react with Pb(NO3)2? 2 KCl (aq) + Pb(NO3)2(aq) →2 KNO3 (aq) + PbCl2(s) •21.3 g•12.8 g•8.54 g•4.27 g•2.13 g
Lead(IIl) nitrate and ammonium iodide react to form lead(Il) iodide and ammonium nitrate according to the Pb(NO3)2 (aq) + 2NH4I (aq) → PbI2 (s) + 2NH4NO3 (aq) What volume of a 0.370 M NH4l solution is required to react with 429 mL of a 0.140 M Pb(NO3)2 solution? How many moles of Pbl are formed from this reaction?
Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to BaO2(s) + H2SO4(aq) → BaSO4(s) + H2O2(aq) How many milliliters of 3.00 M H2SO4(aq) are needed to react completely with 77.5 g of BaO2(s)?
Zinc reacts with hydrochloric add according to the reaction equation Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) How many milliliters of 3.00 M HCI (aq) are required to react with 7.65 g of Zn(s)?
Lead(ll) nitrate and ammonium iodide react to form lead(lI) iodide and ammonium nitrate according to the reaction What volume of a 0.270 M NH4I solution is required to react with 173 mL of a 0.460 M Pb(NO3)2 solution? How many moles of Pbl2 are formed from this reaction?
Zinc reacts with hydrochloric acid according to the reaction equation Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) How many milliliters of 5.00 M HCl(aq) are required to react with 4.65 g of an ore containing 44.0% Zn(s) by mass?
Find the volume of 0.120 M hydrochloric acid necessary to react completely with 1.54 g AI(OH)3.
For the remaining questions, assume that you start with 0.410 g of copper turnings: Calculate the initial number of moles of Cu. Calculate the minimum volume of 16.0 M HNO3 required to dissolve all of the copper (step 1). If, in practice, 5.0 mL of 16.0 M nitric acid were added to effect the dissolution of the copper (step 1), what would be the minimum volume of 4.00 M NaOH required to neutralize the remaining acid and convert all of the Cu2+(aq) to Cu(OH)2(s) (step 2)? Calculate the minimum volume of 1.00 M H2SO4 required to dissolve all of the CuO(s) (step 4). Calculate the minimum mass of zinc required to reduce all of the Cu 2+(aq) to Cu(s) (step 5). (Note that, in practice, a significant excess of zinc is used due to loss of H 2(g).)
Zinc metal and silver nitrate react as shown below. Assuming there is sufficient silver nitrate, how many mL of 0.75 M zinc nitrate solution could be produced from 2.33 g zinc? Zn (s) + AgNO3 (aq) → Zn(NO3)2 (aq) + Ag (s) (a) 27 mL (b) 21 mL (c) 24 mL (d) 96 mL (e) 48 mL
What is the minimum amount of 6.6 M H2SO4 to produce 26.8 g of H2 (g) according to the following reaction? 2Al (s) + 3H2SO4 (aq) → Al2(SO4)2 (aq) + 3H2 (s) Express your answer using two significance figures.
How many grams of Ag 2CO3 will precipitate when excess Na 2CO3 solution is added to 74.0 mL of 0.747 M AgNO3 solution? 2AgNO3 (aq) + Na 2CO3 (aq) → Ag 2CO3 (s) + 2NaNO3 (aq) 
Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric according to BaO2 (s) + H2SO4 (aq) → BaSO4 (s)+ H2O2 (aq) How many milliliters of 2.50 M H2SO4 (aq) are needed to react completely with 63.3 g of BaO2 (s)?
To determine the concentration of SO42- ion in a sample of groundwater, 100.0 mL of the sample is titrated with 0.0250 M Ba(NO3)2, forming insoluble BaSO4. If 4.79 mL of the Ba(NO3)2 solution is required to reach the end point of the titration, what is the (molar) concentration of SO42- in the sample?
Be sure to answer all parts.Calculate the following quantity: number of Mg 2+ ions in each milliliter of 0.472 M magnesium bromide. 
If 10.0 g of ethanol (CH3CH2OH) is added to 10.0 g of methanol (CH3OH), then which compound by convention would be classified as the solvent?a. Ethanolb. Methanolc. Bothd. Neither 
Write the batanced equation for the reaction of aqueous Pb(CIO3)2 with aqueous Nal. Pb(CIO3)2 + 2NaI → PbCl2 + 2NaClO3What mass of precipitate wil form if 1.50 L of highly concentrated Pb(CIO3)2 is mixed with 0.500 L of 0.270 M Nal? Assume the reaction goes to completion.
Chlorine can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid, HCl(aq), as described by the chemical equation MnO2(s) + 4HCl(aq) → MnCl2(aq) + 2H2O(l) + Cl2(g) How much MnO2 (s) should be added to excess HCI(aq) to obtain 235 ml of Cl2(g) at 25°C and 715 Torr?
The combustion of propane may be described by the chemical equation, C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(g) How many grams of O 2(g) are needed to completely burn 33.5 g of C 3H8(g)?
Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric add according to BaO2 (s) + H2SO4 (aq) → BaSO4 (s) + H2O2 (aq) How many milliliters of 5.00 M H2SO4 (aq) are needed to react completely with 22.9 g of BaO2 (s)?
NaOH (s) + H2SO4 (aq) → Na2SO4 (aq) + H2O Consider the unbalanced equation above. A 0.911 g sample of impure NaOH was dissolved in water and required 29.3 mL of 0.226 M H2SO4 solution to react with the NaOH in the sample. What was the mass percent of NaOH in the sample? 
Be sure to answer all parts.How many total moles of ions are released when the following sample dissolves completely in water? Enter your answer in scientific notation. 
Write the balanced chemical equation for the following acid and base reaction. (Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) HC2H3O2 (aq) + Al (OH)3 (aq) → Using the balanced reaction above, calculate the amount of 0.0024 M Al(OH) 3 that would neutralize 22 mL of 0.0026 M HC2H3O2.How many moles of salt are produced in the reaction? What is the molar concentration of the salt after the reaction is complete? 
Enter your answer in the provided box. A 3.00 x 103 mL sample of 2.75 M HCl solution is treated with 4.37 g of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged.
The dissolution reaction is KMnO4 (s) → K+ (aq) + MnO4- (aq) If a solution is made that is 0.15 M in KMnO4, what are the concentrations of the two ions? 
Rescue Breathing Devices Self-contained self-rescue breathing devices, like the one in the figure below, convert CO2 into O2 according to the following (balanced) reaction: 4KO2 (s) + 2CO2 (g) → 2K2CO3 (s) + 3O2 (g) How many grams of KO2 are needed to produce 985.0 L of O 2 at 20.5°C and 1.00 atm?
In the laboratory you dissolve 23.5 g of potassium fluoride in a volumetric flask and add water to a total volume of 500 mL. What is the molarity of the solution? What is the concentration of the potassium cation?What is the concentration of the fluoride anion?
What is the molarity of the acetic acid solution if 27.7 mL of a 0.245 M KOH solution is required to titrate 24.0 mL of a solution of HC2H3O2? HC2H3O2 (aq) + KOH (aq) → H2O (l) + KC2H3O2 (aq) Express your answer with the appropriate units.
The concentration of nitrate ion in a solution that contains 0.900 M aluminum nitrate is _______ M.(i) 2.70 (ii) 1.80 (iii) 0.450(iv) 0.900 (v) 0.300
Write the balance neutralization between H2SO4 and KOH in aquesous solution.H2SO4 + 2KOH → 2H2O0.350 L of 0.410 M H2SO4 is mixed with 0.300 L of 0.270 M KOH. What concentration of sulfuric acid remains after neutralization.
What mass of oxygen is needed to react with 3.69 gal of methanol according to the balanced equation below? (1.00 gal = 3.79 L, and the density of methanol is 0.793 g/mL.) 2CH3OH() + 3O2(g) → 2CO2(g) + 4H2O(g)If appropriate, express your answer in scientific notion. (Click on the answer box to show the pallet.) 
Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to BaO2 (s) + H2SO4 (aq) → BaSO4 (s) + H2O2 (aq) How many milliliters of 3.50 M H2SO4(aq) are needed to react completely with 39.5 g of BaO2 (s)? Use the periodic table to determine the molar mass of BaO2.
CaCO3 (s) + HCl (aq) → CaCl2 (aq) + CO2 (g) + H2O (l)Consider the unbalanced equation above. What is the concentration of the original hydrochloric acid solution if 91.5 mL of HCl reacts with 3.72 g of calcium carbonate?
Given the following equation, how many grams of PbCO3 will dissolve when 1.0 L of 1.00 M H+ is added to 3.00 g of PbCO3? PbCO3 (s) + 2H+ (aq) → Pb2+ (aq) + H2O (l) + CO2 (s)
What volume of 0.253 M H 2SO4 is needed to react with 59.2 mL of 0.103 M NaOH? The equation is H2SO4 (aq) + 2NaOH (aq) → Na 2SO4 (aq) + 2H2O (l)
Enter your answer in the provided box. A 1.50 x 103 mL sample of 2.50 M HCl solution is treated with 4.72 g of magnesium. Calculate the concentration of the acid solution after all the metal has reacted. Assume that the volume remains unchanged.
How many mL of 1.30 M HCI solution contains enough HCl to react completely with 0.300 g of zinc metal? The reaction is Zn(s) + 2HCl(aq) → ZnCl 2(aq) + H2(g) 
The chloride ion concentration in a solution may be determine by the precipitation of lead chloride.Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s) A student finds that 16.96 mL of 0.6170 M lead nitrate is needed to precipitate all of the chloride ion in a 50.00 mL sample of an unknown. What is the molarity of the chloride ion in the student's unknown? 
Green plants use light from the Sun to drive photosynthesis. Photosynthesis is a chemical reaction in which water (H2O) and carbon dioxide (CO2) chemically react to form the simple sugar glucose (C6H12O6) and oxygen gas (O2). What mass of oxygen gas is produced by the reaction of 8.91 g of water? Be sure your answer has the correct number of significant digits. 
An aqueous solution of hydroiodic acid is standardized by titration with a 0.126 M solution of barium hydroxide. If 27.4 mL of base are required to neutralize 29.7 mL of the acid, what is the molarity of the hydroiodic acid solution?
Zinc reacts with hydrochloric acid according to the reaction equation.Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)How many milliliters if 5.00 M HCl(aq) are required to react with 4.55 g of Zn(s)? http://www.chegg.com/homework-help/questions-and-answers/zinc-reacts-hydrochloric-add-according-reaction-equation-zn-s-2hcl-aq-rightarrow-zncl2-aq--q21864849
A student titrates 0.4054 grams of an unknown monoprotic acid to the equivalence point with 17.26 mL of 0.0989 M NaOH (aq). The molecular mass of the unknown acid is: (Enter only the numerical value for your answer) 
Enter your answer in the provided box.How many grams of KHP are needed to neutralize 97.98 mL of a 0.1087 M NaOH solution? (molar mass of KHP = 204.2 g/mol)
Calculate the molarity of the hydroxide ions in a solution that has been prepared by dissolving 88.7 g of barium hydroxide (Ba(OH)2) in water and diluting the solution to a final volume of 3.00 L. (M.W's: Ba = 137.3 g/mol, O = 16.0  g/mol, and H = 1.0 g/mol) 
Dietary iron forms a 1: 1 complex with hemoglobin (Hb), which is responsible for O 2 transport in the body based on the following equation: Hb + 4O2 → Hb (O2)4 How many moles of oxygen could be transported by the hemoglobin complex formed from 9 mg of dietary iron? [Anemia-A Limiting Reagent Problem? p. 172] Express your answer to two significant figures and include the appropriate units.
The amount of I3- (aq) in a solution can be determined by titration with a solution containing a known concentration of S2O32- (aq) (thiosulfate ion). The determination is based on the net ionic equation 2S2O32- (aq) + I3-(aq) → S4O62- (aq) + 3I-(aq) Given that it requires 30.4 mL of 0.470 M Na2S2O_3 (aq) to titrate a 25.0-mL sample of I_3^- (aq), calculate the molarity of I3- (aq) in the solution. 
When solutions of silver nitrate and magnesium chloride are mixed, silver chloride precipitates out of solution according to the equation 2AgNO3 (aq) + MgCl2 (aq) → 2AgCl (s) + Mg(NO3)2 (aq) Part AWhat mass of silver chloride can be produced from 1.94 L of a 0.115 M solution of silver nitrate?  Express your answer with the appropriate units. Part BThe reaction described in Part A required 3.88 L of magnesium chloride. What is the concentration of this magnesium chloride solution? Express your answer with the appropriate units.
Calculate the number of milliliters of 0.434 M KOH required to precipitate all of the Pb2+ ions in 142 mL of 0.438 M Pb(NO 3)2 solution as Pb(OH)2. The equation for the reaction is: Pb(NO3)2 (aq) + 2KOH (aq) → Pb(OH) 2 (s) + 2KNO3 (aq) 
You want to analyze a silver nitrate solution. Part A You could add HCl(aq) to the solution to precipitate out AgCI(s). What volume of a 0.180 M HCl(aq) solution is needed to precipitate the silver ions from 20.0 mL of a 0.240 M AgNO3 solution? Express your answer with the appropriate units. Part B You could add solid KCl to the solution to precipitate out AgCl(s). What mass of KCl is needed to precipitate the silver ions from 20.0 mL of 0.240 M AgNO3 solution? Express your answer with the appropriate units. 
The antacid tablet in the glass of water (Figure P4.112) contains 740.0 mg of magnesium oxide per tablet. What volume of 0.100 M stomach acid (HCI) could one tablet neutralize?
Calculate the H2C2O4(aq) molarity (M) if 10.00 ml of its solution reacts completely with 31.5 mL of a 0.0158M KMnO4(aq).
Calculate the mass of MgCO3 precipitated by mixing 10.0 mL of a 0.200 M Na2CO3 solution with 5.00 mL of a 0.0500 M Mg(NO3)2 solution.
How many grams of Cu(NO3)2 are required to prepare 18.00 mL of a 0.124 M Cu2+ solution? Please use the Periodic Table to calculate the molar mass using the figures in that specific table. 
How many milliliters of a 0.15 M potassium chloride solution should be added to 47.70 mL of a 0.31 M lead(II) nitrate solution to precipitate all of the lead(II) ion?
Potassium hydrogen phthalate (KHP) is often used as a primary standard in acid-base titration. If 20.65 mL of NaOH is required to neutralize 0.457 g of KHP, what is the concentration of the NaOH? 
When potassium chloride is dissolved in water, a. Potassium chloride is the solute. b. Potassium chloride is the solvent. c. Potassium chloride is the solution.
Enter your answer in the provided box. How many grams of solid barium sulfate form when 41.0 mL of 0.160 M barium chloride reacts with 70.0 mL of 0.065M sodium sulfate? Aqueous sodium chloride forms also.