Ch.4 - Chemical Quantities & Aqueous ReactionsWorksheetSee all chapters
All Chapters
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 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 massvolume 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+?

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. 
Calculate the mass percentage of Na2 SO4 in a solution containing 10.6 g Na2 SO4 in 485 g water.
A solution is made containing 14.6 g of CH3 OH in 185 g H2 O.Calculate the mass percent of CH3 OH.
When magnesium metal is burned in air, two products are produced. One is magnesium oxide, MgO. The other is the product of the reaction of Mg with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas.In an experiment a piece of magnesium ribbon is burned in air in a crucible. The mass of the mixture of MgO and magnesium nitride after burning is 0.470 g. Water is added to the crucible, further reaction occurs, and the crucible is heated to dryness until the final product is 0.486 g of MgO. What was the mass percentage of magnesium nitride in the mixture obtained after the initial burning?
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 148 - 153)Section 4.6 while completing this problem.What is the molarity of an HCl solution if 27.3 mL of it neutralizes 134.5 mL of 0.0165 M Ba(OH)2?
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?
Find the volume of 0.120 M hydrochloric acid necessary to react completely with 1.53 g Al(OH)3.
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?
Formic acid has the chemical formula HCOOH. It is a colorless liquid that has a density of 1.220 g/mL.How many milliliters of a 0.15 M solution of NaOH would it take to completely react with 0.755 mL of formic acid?
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.
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.
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?
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?
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
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?
What volume of 0.0200 M calcium hydroxide is required to neutralize 35.00 mL of 0.0500 M nitric 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.
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 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?
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?
If 25.98 mL of 0.1180 M KOH solution reacts with 52.50 mL of CH 3COOH solution, what is the molarity of the acid solution?
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 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.
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.
Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin. A solution containing 81.5 g of ascorbic acid dissolved in 220 g of water has a density of 1.22 g/mL at 55oC.Calculate the mass percentage of ascorbic acid in this 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?