A 1.00 liter solution contains 0.40 moles acetic acid and 0.31 moles sodium acet

Question

A 1.00 liter solution contains 0.40 moles acetic acid and 0.31 moles sodium acetate . If 0.15 moles of hydroiodic acid 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 hydroiodic acid.)

A. The number of moles of CH3COOH will decrease.

B. The number of moles of CH3COO- will increase.

C. The equilibrium concentration of H3O+ will remain the same.

D. The pH will remain the same. E. The ratio of [CH3COOH] / [CH3COO-] will increase.

Explanation / Answer

(i) The statement A is false.

Reason: The added strong acid (HI) reacts with sodium acetate to form acetic acid, so the no. of moles of CH3COOH will increase.

(ii) The statement B is false.

Reason: The added strong acid (HI) reacts with sodium acetate to form acetic acid, so the no. of moles of CH3COO- will decrease.

(iii) The statement C is true.

(iv) The statement D is true.

(v) The statement E is true.

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