Calculate the pH of a solution that contains 2.4 × 10^-5 M H₃O^⁺ at 25°C. A)2.40 B)9.38 C)4.62 D)11.60 E)4.17

Question

Quizplus · Accepted Answer

First we need to write the balanced equation for the dissociation of HSBO4+:

HSBO4+ ⇌ H+ + SBO4^2-

Kw = [H+][OH-] = 1.0 × 10^-14

Ka = [H+][SBO4^2-]/[HSBO4+] = 1.2 × 10^-7

[H+] = √(Ka[HSBO4+]) = √(1.2 × 10^-7 × 2.4 × 10^-5) = 9.38 × 10^-7

pH = -log[H+] = -log(9.38 × 10^-7) = 4.62

Calculate the PH of a Solution That Contains 2