Which of the following is the correct hydroxide ion (OH^-)concentration of an aqueous solution with a pH of 2.77? (K_w = 1.01 × 10^-14) A) 5.9 × 10^-12 M B) 1.7 × 10^-3 M C) 5.2 × 10^-2 M D) 1.1 × 10¹ M E) 5.9 × 10² M

Question

Quizplus · Accepted Answer

The concentration of hydroxide ions ($[OH^-]$) in a solution can be found using the relationship $K_w = [H^+][OH^-]$, where $K_w$ is the ion product constant for water ($1.01 \times 10^{-14}$ at 25°C). Given a pH of 2.77, the concentration of hydrogen ions ($[H^+]$) is $10^{-2.77}$. To find $[OH^-]$, rearrange the equation to $[OH^-] = \frac{K_w}{[H^+]}$. Substituting the given values, $[OH^-] = \frac{1.01 \times 10^{-14}}{10^{-2.77}} = 5.9 \times 10^{-12}$ M.

Which of the Following Is the Correct Hydroxide Ion (OH-)concentration

Which of the Following Is the Correct Hydroxide Ion (OH^-)concentration