If the $\mathrm { p } K _ { w }$ of a neutral solution is 13.6, what is its pH?

Question

Quizplus · Accepted Answer

The $\mathrm { p } K _ { w }$ is the negative logarithm of the ionic product of water ($K_w$), and for a neutral solution, $pH = pOH$. Since $\mathrm { p } K _ { w } = pH + pOH$, for a neutral solution, $2 \times pH = \mathrm { p } K _ { w }$. Therefore, $pH = \frac{\mathrm { p } K _ { w }}{2} = \frac{13.6}{2} = 6.8$. The closest answer is 6.81.

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If The $\mathrm { p } K _ { w }$