Answer
(a) $[OH^-] = 6.6 \times 10^{- 13}M$
(b) $[OH^-] = 1.9 \times 10^{- 1}M$
(c) $[OH^-] = 1.9 \times 10^{- 6}M$
(d) $[OH^-] = 2.1 \times 10^{- 12}M$
Work Step by Step
1. Calculate the hydroxide ion concentration:
pH + pOH = 14
1.82 + pOH = 14
pOH = 12.18
$[OH^-] = 10^{-pOH}$
$[OH^-] = 10^{- 12.18}$
$[OH^-] = 6.6 \times 10^{- 13}M$
2. Calculate the hydroxide ion concentration:
pH + pOH = 14
13.28 + pOH = 14
pOH = 0.72
$[OH^-] = 10^{-pOH}$
$[OH^-] = 10^{- 0.72}$
$[OH^-] = 1.9 \times 10^{- 1}$
3. Calculate the hydroxide ion concentration:
pH + pOH = 14
8.29 + pOH = 14
pOH = 5.71
$[OH^-] = 10^{-pOH}$
$[OH^-] = 10^{- 5.71}$
$[OH^-] = 1.9 \times 10^{- 6}M$
4. Calculate the hydroxide ion concentration:
pH + pOH = 14
2.32 + pOH = 14
pOH = 11.68
$[OH^-] = 10^{-pOH}$
$[OH^-] = 10^{- 11.68}$
$[OH^-] = 2.1 \times 10^{- 12}M$