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Laboratory Section:

1. Write the formula of the salt formed when the following acid and base react. Indicate the acid/base properties of a solution of the salt as either neutral, greater than 7, or less than 7.

2. For each of the following salts indicate the formula of the anion and the cation in the salt, the formula of the acid and base that had to react to form the salt. Indicate the acid/base properties of a solution of the salt as either neutral, greater than 7, or less than 7. For example:

KCN is a salt: the cation is K⁺ : the anion is CN^-. The acid and base that reacted to form the salt are HCN (a weak acid) and KOH (a strong base). Since K⁺ comes from a strong base, K⁺ will not effect the pH of the solution. The anion CN^- come from a weak acid, and therefore can effect the pH of the solution. Since CN^- is the conjugate base of HCN, it is basic and the pH of the solution will be greater than 7.

Complete the following table for the two salts.

3. Based on the acid base properties you assigned to KClO and CH₃NH₃NO₃ write the balanced chemical equation that describes the acid base character of the ion that controls the pH of the solution. For the example in 2 we had concluded that CN^- controls the pH of the solution, so we can write a chemical equation that describes how CN^- behaves as a base.

CN^- + H₂O HCN + OH^-

Write the chemical equation for each salt from Q2:

KClO

CH₃NH₃NO₃

4. Calculate the pH of a 0.100 M KClO solution. (NOTE: K_a (HClO) = 3.0 x 10^-8)

pH =

5. Calculate the pH of a 0.100 M CH₃NH₃NO₃ solution. (NOTE: Here is a table of equilibrium constants to help answer this question.)

pH =

6. Is there anything about the questions that you feel you do not understand? List your concerns/questions.

7. If there is one question you would like to have answered in lecture, what would that question be?