68) Calculate the masses of potassium dichromate, K2Cr2O7, and water in 400 g of an 8.65% solution of potassium
dichromate.
69) What mass of an 8.65% solution of potassium dichromate contains 60.0 g of K2Cr2O7? What mass of water does
this amount of solution contain?
70) Calculate the mass of an 8.30% solution of ammonium chloride, NH4Cl, that contains 100 g of water. What mass
of NH4Cl does this amount of solution contain?
71) The density of an 18.0% solution of ammonium chloride, NH4Cl, solution is 1.05 g/mL. What mass of NH4Cl
does 350 mL of this solution contain?
72) The density of an 18.0% solution of ammonium sulfate (NH4)2SO4, is 1.10 g/mL. What mass of ammonium
sulfate would be required to prepare 350 mL of this solution?
73) What volume of the solution of NH4Cl described in in #4 contains 80.0 g of NH4Cl?
74) What volume of the solution of ammonium sulfate in #5 contains 80.0 g of (NH4)2SO4?
75) A reaction requires 37.8 g of NH4Cl. What volume of the solution described in #4 would you use if you wished
to use a 20.0% excess of ammonium chloride?
76) What is the molarity of a solution that contains 490 g of phosphoric acid, H3PO4, in 2.00L of solution?
77) What is the molarity of a solution that contains 1.37 g of sodium chloride in 25.0 mL of solution?
78) What is the molarity of a barium chloride solution prepared by dissolving 3.50 g of BaCl 2 • 2H20 in enough
water to make 500 mL of solution?
79) What mass of sodium sulfate, Na2SO4, is contained in 750 mL of a 2.00 molar solution?
80) What mass of zinc chloride, ZnCl2, is required to prepare 5.00L of a 0.450 molar solution?
81) What mass of potassium benzoate trihydrate, KC7H502 • 3H20, is needed to prepare one liter of a 1.025 molar
solution of potassium benzoate?
82) What volume of a 0.320 M Na2CO3 solution can be prepared from 16.4 g of Na2CO3?
83) What volume of 0.850 M CuSO4 solution can be prepared from 16.4 g of CuSO4∙5H2O ?
Solution Stoichiometry
84. What volume of 0.185 molar nitric acid, HN03, is required to react with 12.61 g of calcium hydroxide, Ca(OH)2,
according to the following equation?
2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H20
85. What volume of a 2.00 molar solution of sulfuric acid, H2SO4, is required to react with 250g of magnesium carbonate,
MgCO3, according to the following equation?
MgCO3 + H2SO4 → MgSO4 + CO2 + H2O
86. What volume of a 0.250 molar solution of silver nitrate, AgNO3 is required to react with 18.6 g of potassium
phosphate, KPO4, according to the following equation?
3AgNO3 + K3PO4 → Ag3PO4 + 3KNO3
87. The density of a 1.08 M CsCl solution is 1.138 g/mL at 20˚C. What is the percent by mass of CsCl in the solution?
88. A solution made by dissolving 18.0g of CaCl2 in 72.0g of water has a density of 1.180g/mL at 20˚C. (a) What is the
percent by mass of CaCl2 in the solution? (b) What is the molarity of CaCl2 in the solution?
89. Stock phosphoric acid solution is 85.0% H3PO4 and has a specific gravity of 1.17. What is the molarity of the
solution?
90. Stock Hydrofluoric acid solution is 49.0% HF and has a specific gravity of 1.17. What is the molarity of the solution?
91. What volume of 0.850 M (COOH)2 solution would be required to react with 30.0 mL of 0.180 M Na2CO3 solution?
Na2CO3 + (COOH)2 → Na2(COO)2 + H2CO3
92. What volume of 0.200 M FeSO4 solution would be required to react with 20.0 mL of 0.250 M KMnO4 (in sulfuric acid
solution) according to the following equation?
10FeSO4 + 2KMnO4 + 8H2SO4 → 5Fe2(SO4)3 + 2MnSO4 + K2SO4 + 8H2O
93. Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume of concentrated sulfuric
acid required to prepare 2.50 L of 0.150 M H2SO4 solution.
94. Commercial concentrated hydrochloric acid is 12.0 M HCl. What volume of concentrated hydrochloric acid is
required to prepare 3.50 L of 2.40 M HCl solution?
95. Calculate the volume of 2.00 M NaOH solution required to prepare 100 mL of a 0.500 M solution of NaOH.
96. Calculate the volume of 0.0500 M Ba(OH)2 solution that contains the same number of moles of Ba(OH)2 as 120 mL of
0.0800 M Ba(OH)2 solution.
97. Calculate the resulting molarity when 50.0 mL of 2.30 M NaCl solution is mixed with 80.0 mL of 1.40 M MaCl.
98. Calculate the resulting molarity when 125 mL of 6.00 M H2SO4 solution is mixed with 225 mL of 3.00 M H2SO4
89) Stock Phosphoric acid solution is 85.0% H3PO4 and has a specific gravity of 1.70. What is the molarity of the
solution?
Stoichiometry and Solutions
1. If it takes 36 ml of 0.5 molar sodium hydroxide solution to titrate to an endpoint of 15 ml of sulfuric
acid, what is the molarity of the sulfuric acid?
0.60
2. When 80 ml of 0.40 molar aluminum sulfate is allowed to react with excess barium nitrate, how many
grams of barium sulfate will be formed?
22
3. How many milliliters of 0.80 M phosphoric acid will it take to react with 120 ml of 0.70 molar calcium
hydroxide?
70
4. A 40% solution of sodium phosphate has a specific gravity of 1.6. What volume of the solution will
react completely with 80 ml of 0.60 M lead II nitrate?
8.2
5. When zinc reacts with hydrochloric acid, 85 ml of hydrogen gas are produced at 27 degrees Celsius and
740 torr. What volume of 1.5 molar hydrochloric acid is needed to produce this volume of hydrogen
gas?
6. If 40 ml of 0.80 molar sulfuric acid reacts with 30 ml of 1.2 molar sodium hydroxide solution, how
many milliliters of which reactant will be in excess? How many liters of liquid water will be produced?