## General Chemistry (4th Edition)

$[K^+] = 0.25M$ $[OH^-] = 0.25M$ $[H_3O^+] = 4 \times 10^{-14}M$ This solution is basic.
$KOH$ is a strong base; therefore: The reaction: $1KOH(aq) -- \gt 1K^+(aq) + 1OH^-(aq)$ will completely occur, so: $Initial[KOH] = [K^+] = [OH^-] = 0.25M$ - Now, use the $K_w$ value to calculate the $[H_3O^+]:$ $[OH^-] * [H_3O^+] = Kw = 10^{-14}$ $0.25 * [H_3O^+] = 10^{-14}$ $[H_3O^+] = \frac{10^{-14}}{ 0.25}$ $[H_3O^+] = 4 \times 10^{- 14}M$ - $KOH$ is a base, so its solution should be basic. Other method: - $[OH^-] > [H_3O^+]$, so the solution is basic.