1.
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What is the pH after 0.070 mol of solid NaNO2 is added to 250.0 mL of a solution that is 0.10 M HNO2? The Ka of HNO2 is 7.2 x 10-4. Assume no volume change.
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2.
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What is the pH of a buffer solution that is prepared by dissolving 40.0 g HC2H3O2 and 30.0 g NaC2H3O2 in enough water for 250.0 mL of solution? The Ka of HC2H3O2 is 1.8 x 10-5.
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3.
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What is the pH of a solution prepared by adding 5.00 g NH4Cl to 100.0 mL of 0.40 M NH3? The Kb of NH3 is 1.8 x 10-5.
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4.
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Consult Figure 18-8 on page 725 of your text. What is the approximate pH of a solution if we observe the following? 10 mL of the solution and a drop of bromphenol blue is blue.
10 mL of the solution and a drop of phenol red is yellow.
10 mL of the solution and a drop of bromthymol blue is yellow.
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5.
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What is the pH of a solution that is prepared by mixing 20.00 mL of 0.1000 M HCl with 12.00 mL of 0.1500 M NaOH?
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6.
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What is the pH of a solution that is prepared by mixing 20.00 mL of 0.1000 M HC2H3O2 with 6.00 mL of 0.1500 M NaOH? The Ka of HC2H3O2 is 1.8 x 10-5.
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7.
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What is the pH of 0.50 M Na2SO3? For HSO3-, Ka = 6.2 x 10-8.
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8.
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How many grams of NaOH must be added to a 250.0-mL sample of 0.30 M HC2H3O2 to give a solution with a pH of 5.00? Assume no volume change. The Ka of HC2H3O2 is 1.8 x 10-5.
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9.
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Why is it not practical to titrate ammonia with acetic acid?
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10.
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A 0.2500 M solution of HCl is used to titrate 40.0 mL of a 0.500 M solution of methylamine, CH3NH2 (Kb = 5.0 x 10-4). What are the pH's at 0, 10, 50, and 90% titrated?
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