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Saturated,Unsaturated and Supersaturated Solutions

When 0.1...

Question

When $0.100$ mole of ammonia, ${N H}_{3}$ , is dissolved in sufficient water to make $1.0 L$ of solution, the solution is found to have a hydroxide ion concentration of $1.34 \times 10^{- 3} M$ . Calculate $K_{b}$ for ammonia.

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Solution

$N H_{3} + H_{2} O ⇌ {N H}_{4}^{+} + O H^{-}$

$[N H_{3}] = (0.1 - 1.34 \times 10^{- 3}) M$
$[N H_{4}^{+}] = 1.34 \times 10^{- 3} M$
$[O H^{-}] = 1.34 \times 10^{- 3} M$

Now
$K_{b} = \frac{[{N H}_{4}^{+}] [O H^{-}]}{[{N H}_{3}]}$

$K_{b} = 1.82 \times 10^{- 5}$

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