Chapter 16 Principles of Chemical Reactivity: The Chemistry of Acids and Bases - Study Questions - Page 629a: 10

$[H_3O^+] = 3.02 \times 10^{- 11}M$ $[OH^-] = 3.311 \times 10^{- 4}M$ - It is a basic solution.

1. Calculate the hydronium concentration: $[H_3O^+] = 10^{-pH}$ $[H_3O^+] = 10^{- 10.52}$ $[H_3O^+] = 3.02 \times 10^{- 11}M$ 2. Find the $[OH^-]$: $[H_3O^+] * [OH^-] = Kw = 10^{-14}$ $ 3.02 \times 10^{- 11} * [OH^-] = 10^{-14}$ $[OH^-] = \frac{10^{-14}}{ 3.02 \times 10^{- 11}}$ $[OH^-] = 3.311 \times 10^{- 4}M$ - Solutions with pH > 7 are basic.