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INTEGRATIVE EXERCISES

105 Suppose you have 5.00 g of powdered magnesium metal, 1.00 L of 2.00 M potassium nitrate solution, and 1.00 L of 2.00 M silver nitrate solution, (a) Which one of the solutions will react with the magnesium powder (b) What is the net ionic equation that describes this reaction (c) What volume of solution is needed to completely react with the magnesium (d) What is the molarity of the ions in the resulting solution  [Pg.156]

106 (a) By titration, 15.0 mL of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of an organic acid. What is the molar mass of the acid if it is monoprotic (b) An elemental analysis of the acid indicates that it is composed of 5.89% H, 70.6% C, and 23.5% O by mass. What is its molecular formula  [Pg.156]

107 A 3.455-g sample of a mixture was analyzed for barium ion by adding a small excess of sulfuric acid to an aqueous solution of the sample. The resultant reaction produced a precipitate of barium sulfate, which was collected by filtration, washed, dried, and weighed. If 0.2815 g of barium sulfate was obtained, what was the mass percentage of barium in the sample  [Pg.156]

108 A tanker truck carrying 5.0 X 10 kg of concentrated sulfuric acid solution tips over and spills its load. If the sulfuric acid is 95.0% H2SO4 by mass and has a density of 1.84 g/mL, how many kilograms of sodium carbonate must be added to neutralize the acid  [Pg.156]

109 A sample of 5.53 g of Mg(OH)2 is added to 25.0 mL of 0.200 M HNO3. (a) Write the chemical equation for the reaction that occurs, (b) Which is the limiting reactant in the reaction (c) How many moles of Mg(OH)2, HNO3, and Mg(N03)2 are present after the reaction is complete  [Pg.156]

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