At equilibrium, a 1.00 M OCl− solution has an [OH−] of 5.75 × 10−4 M. Which of the following is the correct pH of the solution?

Question

Angelina_Jolie [31]

3 years ago

5

At equilibrium, a 1.00 M OCl− solution has an [OH−] of 5.75 × 10−4 M. Which of the following is the correct pH of the solution?

3.24 3.3 × 10−7 14.00 10.76

Chemistry

2 answers:

sveta [45] · Answer 1 · 2022-02-28T12:56:50+03:00

sveta [45]3 years ago

6 0

Thank you for posting your question here at brainly. I hope the answer will help you. Feel free to ask more questions.

Below is the solution:

pOH = - log (5.75 × 10^−4) = 3.24
<span>pH = 14 - 3.24 = 10.76</span>

Degger [83] · Answer 2 · 2022-02-28T14:23:42+03:00

Degger [83]3 years ago

3 0

pOH = - log (5.75 × 10^−4) = 3.24

pH = 14 - 3.24 = 10.76