Last modified: Sat 10/26/2013 01:01:51 pm
ACA

Oklahoma State University

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Answer all of the questions below. If you do not know an answer enter CNA. However, it will help me the most if you answer each question with your best intuition/idea about what would be a reasonable answer.


First Name:

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Laboratory Section:

1. The following three substances are salts. For each identify the ions found in an aqueous solution.

NaC2H3O2

cation

anion

C2H5NH3Cl

cation

anion

KC6H5O

cation

anion

2. Predict whether the pH of 0.1 M solutions of each of the salts is greater, less or equal to 7.

Salt (0.1M)

pH (greater, equal or less than 7)

NaC2H3O2

C2H5NH3Cl


KC6H5O

3. In a 0.10 M NaC2H3O2 solution which ion effects the pH of the solution?

4. Write a Bronsted-Lowry equation which describes the acid/base character of the ion in Q3. (Hint: if you have indicated the salt has the properties of a base write a BL equation which supports that behavior.)

5. Calculate the pH of 0.10 M NaC2H3O2 solution.

pH =

6. Calculate the pH of a solution that is 0.10 M HC2H3O2 and 0.10 M NaC2H3O2. Hint: Write the chemical reaction for the weak acid dissociation for the ICE table. Just be careful when you enter the initial concentration of each species in the chemical equation.)

pH =

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

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