## Chemistry: Principles and Practice (3rd Edition)

$[H_3O^+] = 3.02 \times 10^{- 11}$ $[OH^-] = 3.311 \times 10^{- 4}$ - It is a basic solution.
1. Calculate the hydronium concentration: $[H_3O^+] = 10^{-pH}$ $[H_3O^+] = 10^{- 10.52}$ $[H_3O^+] = 3.02 \times 10^{- 11}$ 2. Use "Kw" to calculate the hydroxide concentration: $[H_3O^+] * [OH^-] = Kw = 10^{-14}$ $3.02 \times 10^{- 11} * [OH^-] = 10^{-14}$ $[OH^-] = \frac{10^{-14}}{ 3.02 \times 10^{- 11}}$ $[OH^-] = 3.311 \times 10^{- 4}$ - Since $[OH^-] > [H_3O^+]$, this solution is basic.