Question

1.00 liter solution contains 0.40 M acetic acid and 0.52 M potassium acetate. If 0.130 moles of calcium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of calcium hydroxide.)

A. The number of moles of CH3COOH will increase.
B. The number of moles of CH3COO- will decrease.
C. The equilibrium concentration of H3O will remain the same.
D. The pH will decrease.
E. The ratio of [CH3COOH] / [CH3COO-] will increase.

Answer 1

Answer:

Explanation:

Initial moles of Acetic acid=$M\times V=0.42\ M\times 1\ L=0.40\ mol.$

Initial moles of potassium acetate = $M\times V=0.52\ mol$

since, CaOH is a strong base. So, after its addition i react with acetic acid.

Moles of acetic acid left= $0.40-0.13=0.27\ mol$

Moles of potassium acetate=$0.52+0.13 = 0.65\ mol$

Now, we check all given options:

A. False ( because it gets consumed by KOH)

B. True

C. False ( it decrease because of addition of base)

D. False ( It increase because of addition of base)

E. False ( Because con of $CH_3COOH$ decrease and $CH_3COO-$ increase.