Question

If a solution of aspirin has a [OH-] = 4.4 x 10–12 M, what is the pH of the solution?

Answer 1

Answer on Question #71796 – Chemistry – Other

Task:

If a solution of aspirin has a $[\mathrm{OH}^{-}] = 4.4 \times 10^{-12} \mathrm{M}$, what is the pH of the solution?

Solution:

$$\begin{array}{l} pH + pOH = 14; \\ pOH = -\log[\mathrm{OH}^{-}] = -\log(4.4 \times 10^{-12}) = 11.3565 \approx 11.36; \\ pH = 14 - pOH = 14 - 11.36 = 2.64; \\ pH = 2.64 \\ \end{array}$$

Answer: pH=2.64

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