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| 1. | Given the following balanced ionization reactions for the following weak acids and bases, write the Ka or Kb expressions for each. | |||||||||||||||||
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| 2. | Calculate [OH–] in a solution containing 100.0 g of potassium hydroxide in 2.50 L solution. Potassium hydroxide is a strong base. | |||||||||||||||||
| 3. | A solution is prepared in which 0.600 mole of hydrogen chloride is dissolved in enough water to make 5.80 L. Calculate the concentration of hydrogen ions in this solution. | |||||||||||||||||
| 4. | A solution is prepared the contains 0.0445 mole of sulfuric acid in a total solution volume of 12.1 L. Sulfuric acid typically undergoes complete ionization according to the equation: H2SO4 → 2H+ + SO42- Calculate [H+]. Sulfuric acid is a strong acid. |
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| 5. | Phosphoric acid is a weak acid that undergoes the following ionization reaction: H3PO4 (aq) → H+(aq) + H2PO4-(aq) If there are 1.32 × 10-2 mole of phosphoric acid present in 875 mL of solution, calculate the concentration of hydrogen ions, H+, in solution. Ka for phosphoric acid is 7.0 × 10-3. Begin by calculating [H3PO4]. Then use Ka to determine [H+]. |
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| 6. | Determine the pH of each of the following solutions, and tell whether the solution is acidic or basic. | |||||||||||||||||
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| 7. | Calculate both [H+] and [OH–] for the following solutions. All are either strong acids or strong bases. Be sure to clearly identify all answers. | |||||||||||||||||
| a. | 2.5 M NaOH | |||||||||||||||||
| b. | 0.045 M HCl | |||||||||||||||||
| 8. | Calculate the pH of a 0.1 M solution of sodium hydroxide, NaOH, a strong base. Hint: First find [OH–]. Use this to find [H+] which you then convert to pH |
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| 9. | a. | Determine the concentration of hydrogen ions, [H+] in a solution whose pH is 5.17. | ||||||||||||||||
| b. | Calculate the hydroxide ion concentration, [OH-], for this solution. | |||||||||||||||||
| 10. | Determine [H3O+] in a solution whose pH = 9.22. (Hint: [H3O+] = [H+]) | |||||||||||||||||
| 11. | A 2.67 g sample of hydrogen fluoride gas (HF) is dissolved in sufficient water to make 1.05 L of solution at 25°C to form an acidic solution. Hydrogen fluoride is a weak acid with Ka = 6.6 × 10-4 Calculate the pH of this solution. Hint: Begin by calculating [HF]. Then use Ka to determine [H+]. Finally convert [H+] to pH. |
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| 12. | The formula for ascorbic acid, better known as Vitamin C, is HC6H7O6. Ka for ascorbic acid is 8.00 × 10-5. Determine the pH of a solution prepared by dissolving a 500.0 mg vitamin C tablet in enough water to make 200.0 mL of solution. |
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