Calculate the pH of a solution containing 0.105 M HA and 0.146 M A^-. The Ka for the weak acid is 1.8 *10^-⁵. A) 4.88 B) 9.11 C) 4.74 D) 7.00

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Quizplus · Accepted Answer

The correct answer is A because the pH of a solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]). In this case, the pKa is -log(1.8 x 10^-5) = 4.74, and the [A-]/[HA] ratio is 0.146/0.105 = 1.39. Plugging these values into the equation gives a pH of 4.88.

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