Answer to Question #343893 in Organic Chemistry for Charles Ankrah

Question

What is OH- of a solution whose pH is 4.732

Answer 1

Solution:

For any aqueous solution at 25^∘C:

pH + pOH = 14

pOH = 14 − pH = 14 − 4.732 = 9.268

pOH = 9.268

We can convert between pOH and [OH⁻] using the following equation:

pOH = −log[OH⁻]

[OH⁻] = 10^−pOH = 10^−9.268 = 5.395×10⁻¹⁰

[OH⁻] = 5.395×10⁻¹⁰ M

Answer: The hydroxide ion (OH⁻) concentration is 5.395×10⁻¹⁰ M