Adapted by Nelson Nuñez-Rodriguez
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By David W. Ball
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| QUESTION | ANSWER |
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1. Differentiate between a strong acid and a weak acid. |
1. A strong acid is 100% ionized in aqueous solution, whereas a weak acid is not 100% ionized. |
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3. Identify each as a strong acid or a weak acid. Assume aqueous solutions.
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3.
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5. Write a chemical equation for the ionization of each acid and indicate whether it proceeds 100% to products or not.
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5.
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7. Write the balanced chemical equation for the reaction of each acid and base pair.
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7.
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9. Identify each salt as neutral, acidic, or basic.
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9.
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11. Identify each salt as neutral, acidic, or basic.
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11.
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13. Write the hydrolysis reaction that occurs, if any, when each salt dissolves in water.
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13.
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15. When NH4NO2 dissolves in H2O, both ions hydrolyze. Write chemical equations for both reactions. Can you tell if the solution will be acidic or basic overall? |
15. NH4+ + H2O → NH3 + H3O+; NO2− + H2O → HNO2 + OH−; it is not possible to determine whether the solution will be acidic or basic. |
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17. A lab technician mixes a solution of 0.015 M Mg(OH)2. Is the resulting OH− concentration greater than, equal to, or less than 0.015 M? Explain your answer. |
17. greater than 0.015 M because there are two OH− ions per formula unit of Mg(OH)2 |