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| 1. | Calculate [H+] in a 2.00 L solution of hydrogen chloride in which 3.65 g of HCl is dissolved. Ka for HCl is very large. | |
| 2. | Calculate [H+] in a solution containing 3.20 g of HNO3 in 250 mL of solution. Nitric acid is a very strong acid. | |
| 3. | An acetic acid (HC2H3O2) solution is 0.25 M. Given that Ka for acetic acid is 1.8 × 10-5, find [H+]. | |
| 4. | A solution of acetic acid contains 12.0 g of HC2H3O2 in 500 mL of solution. Calculate [H+]. | |
| 5. | Calculate [H+] and [OH-] at 25 ° C in: | |
| a. | a 5.0 M NaOH solution. NaOH is a strong base. | |
| b. | a 0.025 M Ca(OH)2 solution. Ca(OH)2 is a strong base. | |
| c. | a 0.10 M HCl solution. HCl is a strong acid | |
| d. | a 0.01 M HC2H3O2 solution. HC2H3O2 is a weak acid with Ka = 1.8 × 10-5. | |
| 6. | A mass of 1.4 g of KOH is dissolved in water to form 500 mL of solution. What is the concentration of H+ ions in this solution if the temperature of the solution is 25° C? | |
| 7. | A mass of 4.0 g of NaOH is dissolved in water to form 500 mL of solution with a temperature of 25° C. Calculate the hydronium ion concentration in this solution. | |
| 8. | Calculate the pH of a solution of nitric acid that: | |
| a. | has a concentration of 1.0 × 10-4 M | |
| b. | consists of 6.3 g of solute dissolved in 1.00 L of solution? | |
| 9. | Calculate the pH of a solution that consists of 5.0 g of HCl in 250 mL of solution? | |
| 10. | What is the [H+] of a solution with a pH of 10.00 at 25° C? | |
| 11. | What is the pH of an aqueous solution containing 0.0020 M barium hydroxide, Ba(OH)2? | |
| 12. | Calculate the hydronium ion concentration of: | |
| a. | 100.0 mL of an aqueous solution containing 0.60 g of sodium hydroxide, NaOH. | |
| b. | a blood sample with a pH of 7.40 | |