# Chapter 15 - Acids and Bases - Questions & Problems - Page 710: 15.20

(a) $[H^+] = 6.31 \times 10^{-6}M$ (b) $[H^+] = 1.00 \times 10^{-16}M$ (c) $[H^+] = 2.7 \times 10^{-6}M$

#### Work Step by Step

We will use the equations: $[H^+] = 10^{-pH}$ $[H^+] * [OH^-] = 10^{-14}$ (a) $[H^+] = 10^{-5.20} = 6.31 \times 10^{-6}$ (b) $[H^+] = 10^{-16.00} = 1.00 \times 10^{-16}$ (c) $[H^+] * 3.7 \times 10^{-9} = 10^{-14}$ $[H^+] = \frac{10^{-14}}{3.7 \times 10^{-9}} = 2.7 \times 10^{-6}$

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