Question

What are the hydronium and hydroxide ion concentrations in a solution whose pH is 6.52?

a) [H₃O⁺] = 2.4 × 10⁻⁷ M, [OH⁻] = 4.2 × 10⁻⁸ M
b) [H₃O⁺] = 4.2 × 10⁻⁸ M, [OH⁻] = 2.4 × 10⁻⁷ M
c) [H₃O⁺] = 1.7 × 10⁻⁶ M, [OH⁻] = 5.9 × 10⁻⁸ M
d) [H₃O⁺] = 5.9 × 10⁻⁸ M, [OH⁻] = 1.7 × 10⁻⁶ M

Answer 1

In a solution with a pH of 6.52, the hydronium and hydroxide ion concentrations are both 2.5118864 * 10^(-7) M.

Step-by-step explanation:

In a solution with a pH of 6.52, the hydronium ion concentration can be calculated using the equation [H3O+] = 10^(-pH). Plugging in the pH value of 6.52, we get [H3O+] = 10^(-6.52).

Using a calculator, we find that [H3O+] = 2.5118864 * 10^(-7) M.

Since water is neutral with a pH of 7, the hydronium and hydroxide ion concentrations are equal in a neutral solution. Therefore, the hydroxide ion concentration is also 2.5118864 * 10^(-7) M.