Answer to Question #343892 in Organic Chemistry for Charles Ankrah

Question

What is the OH+ of a solution whose POH =4.70

Answer 1

Solution:

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

pOH = −log[OH⁻]

[OH⁻] = 10^−pOH = 10^−4.70 = 2.00×10⁻⁵

[OH⁻] = 2.00×10⁻⁵ M

For any aqueous solution at 25^∘C:

pH + pOH = 14

pH = 14 − pOH = 14 − 4.7 = 9.3

pH = 9.3

We can convert between pH and [H⁺] using the following equation:

pH = −log[H⁺]

[H⁺] = 10^−pH = 10^−9.3 = 5.01×10⁻¹⁰

[H⁺] = 5.01×10⁻¹⁰ M

Answer:

The hydroxide ion (OH⁻) concentration is 2.00×10⁻⁵ M

The hydrogen ion (H⁺) concentration is 5.01×10⁻¹⁰ M