## Chemistry: The Molecular Science (5th Edition)

$[H_3O^+] = 7.586 \times 10^{- 10}M$ $[OH^-] = 1.318 \times 10^{- 5}M$ This is a basic solution.
$[H_3O^+] = 10^{-pH}$ $[H_3O^+] = 10^{- 9.12}$ $[H_3O^+] = 7.586 \times 10^{- 10}M$ $[H_3O^+] * [OH^-] = Kw = 10^{-14}$ $7.586 \times 10^{- 10} * [OH^-] = 10^{-14}$ $[OH^-] = \frac{10^{-14}}{ 7.586 \times 10^{- 10}}$ $[OH^-] = 1.318 \times 10^{- 5}M$ $[OH^-] > [H_3O^+]$: Basic solution. Assuming $25^{\circ}C$: pH > 7 : Basic solution.