Question

A 1.00 liter solution contains 0.23 M hypochlorous acid and 0.30 M potassium hypochlorite.

If 0.150 moles of potassium 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 potassium hydroxide.)

_______TrueFalseA. The number of moles of HClO will decrease.

_______TrueFalseB. The number of moles of ClO^- will increase.

_______TrueFalseC. The equilibrium concentration of H₃O⁺ will decrease.

_______TrueFalseD. The pH will remain the same.

_______TrueFalseE. The ratio of [HClO] / [ClO^-] will decrease.

Answer 1

Hypochlorous Acid (HClO) is a weak acid. Potassium Hypochlorite (KClO) is a salt.

KOH is a strong base.

The base will neutralize the salt when added to the solution.

1)  The number of moles of HClO will decrease. TRUE

HClO + KOH -----> KClO + H₂O

2) The number of moles of ClO^- will increase. TRUE

HClO + KOH -----> KClO + H₂O

3) The equilibrium concentration of H₃O⁺ will decrease. FALSE

Acid concentration decreases.

4) The pH will remain the same. FALSE

Since the H⁺ concentration changes, the pH will differ.

5) The ratio of [HClO] / [ClO^-] will decrease. TRUE

since HClO decreases and ClO^- increases.