Question

Part A : A 14.0 mL sample of vinegar, which is an aqueous solution of acetic acid, CH3COOH, requires 24.5 mL of a 0.650 M solution of NaOH to reach the endpoint in a titration:

CH3COOH(aq)+NaOH(aq)?NaCH3COO(aq)+H2O(l)

What is the molarity of the acetic acid solution? (Express the concentration to three significant figures and include the appropriate units.)

Part B: Calculate the pH of each solution given the following [H3O+] or [OH?] values.

[H3O+] = 3.0×10^?4 M

[H3O+] = 1.0×10^?8 M

[OH?] = 5.0×10^?5 M

[OH?] = 2.0×10^?11 M

[H3O+] = 7.0×10^?8 M

[OH?] = 7.5×10^?4 M

Express your answer using two decimal places.

Part C: Solution X has a pH of 10.1, and solution Y has a pH of 7.6.

1. Which solution is more acidic?

A.solution Y OR B. solution X

2. What is the [H3O+] in solution X?

Express your answer to one significant figure and include the appropriate units.

3. What is the [H3O+] in solution Y?

Express your answer to one significant figure and include the appropriate units.

4. What is the [OH?] in solution X?

Express your answer to tone significant figure and include the appropriate units.

5. What is the [OH?] in solution Y?

Express your answer to one significant figure and include the appropriate units.