Ch.4 - Chemical Quantities & Aqueous ReactionsSee 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. 
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.
How many moles of Ca(OH)2 are needed to neutralize three moles of HCl?21.513
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 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.a. If you had an extremely magnified view of the solution (to the atomic-molecular level), list the species you would see (include charges, if any).
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.b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges.
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.
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
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?
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?b. 0.0500 M Sr(OH)2
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+.)
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 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.
How do you calculate the mass of KHC8H4O4 (molar mass=204.44 g/mol) that reacts with 15mL of 0.16 M NaOH solution ?
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 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)?
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
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?
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
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)?
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.
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?
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.
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.
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.
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) 
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)
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) 
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.