A 1.00 liter solution contains 0.42 M acetic acid and 0.54 M potassium acetate .

Question

A 1.00 liter solution contains 0.42 M acetic acid and 0.54 M potassium acetate.

If 0.140 moles of barium 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 barium hydroxide.)

_______TrueFalseA. The number of moles of CH3COOH will decrease.

_______TrueFalseB. The number of moles of CH3COO- will decrease.

_______TrueFalseC. The equilibrium concentration of H3O+ will increase.

_______TrueFalseD. The pH will increase.

_______TrueFalseE. The ratio of [CH3COOH] / [CH3COO-] will remain the same.

Explanation / Answer

A 1.00 liter solution contains 0.42 M acetic acid and 0.54 M potassium acetate. It is an acidic buffer.

By adding Ba(OH)2 to this solution, concentration of salt increases and concentration of acid decreases.

True A. The number of moles of CH3COOH will decrease.

False B. The number of moles of CH3COO- will decrease.

False C. The equilibrium concentration of H3O+ will increase.

True   D. The pH will increase.

False E. The ratio of [CH3COOH] / [CH3COO-] will remain the same.

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