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228 Chapter 4 Stoichiometry of Chemical Reactions 83. A sample of gallium bromide, GaBr2, weighing 0.165 g was dissolved in water and treated with silver nitrate, AgNO3, resulting in the precipitation of 0.299 g AgBr. Use these data to compute the %Ga (by mass) GaBr2. 84. The principal component of mothballs is naphthalene, a compound with a molecular mass of about 130 amu, containing only carbon and hydrogen. A 3.000-mg sample of naphthalene burns to give 10.3 mg of CO2. Determine its empirical and molecular formulas. 85. A 0.025-g sample of a compound composed of boron and hydrogen, with a molecular mass of ~28 amu, burns spontaneously when exposed to air, producing 0.063 g of B2O3. What are the empirical and molecular formulas of the compound. 86. Sodium bicarbonate (baking soda), NaHCO3, can be purified by dissolving it in hot water (60 °C), filtering to remove insoluble impurities, cooling to 0 °C to precipitate solid NaHCO3, and then filtering to remove the solid, leaving soluble impurities in solution. Any NaHCO3 that remains in solution is not recovered. The solubility of NaHCO3 in hot water of 60 °C is 164 g L. Its solubility in cold water of 0 °C is 69 g/L. What is the percent yield of NaHCO3 when it is purified by this method? 87. 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) + H2 O(l) 88. What volume of 0.08892 M HNO3 is required to react completely with 0.2352 g of potassium hydrogen phosphate? 2HNO3(aq) + K2 HPO4(aq) ⟶ H2 PO4(aq) + 2KNO3(aq) 89. 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? C2 O4 H2(aq) + 2NaOH(aq) ⟶ Na2 C2 O4(aq) + 2H2 O(l) 90. 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. H2 SO4(aq) + 2KOH(aq) ⟶ K2 SO4(aq) + 2H2 O(l) 91. 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) + 2H2 O(l) What is the molarity? 92. What mass of Ca(OH)2 will react with 25.0 g of propionic acid to form the preservative calcium propionate according to the equation? 93. 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? H3 PO4(aq) + 2KOH(aq) ⟶ K2 HPO4(aq) + 2H2 O(l) 94. Potassium acid phthalate, KHC6H4O4, 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 KHC6H4O4 reacts with 35.73 mL of a NaOH solution in a titration. What is the molar concentration of the NaOH? KHC6 H4 O4(aq) + NaOH(aq) ⟶ KNaC6 H4 O4(aq) + H2 O(aq) This content is available for free at http://cnx.org/content/col11760/1.9PDF Image | Stoichiometry of Chemical Reactions
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