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Q.

An aqueous solution contains 10% ammonia by mass and has a density of $0 .99 g / m^{ℓ}$ . The hydrogen ion concentration in this solution is if $k_{a}$ for ${NH}_{4}^{\oplus} is 5.0 \times 10^{- 10} M$

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a

$1.079 \times 10^{- 2} M$

b

$1 \times 10^{- 12} M$

c

$9.268 \times 10^{- 13} M$

d

$5.82 \times 10^{- 3} M$

answer is C.

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Detailed Solution

$\begin{array}{l} molarity = \frac{10}{17} \times \frac{1}{100 / 0 .99} \times 1000 = 5 .82 M \\ {NH}_{3} + H_{2} O \to {NH}_{4} OH ⇌ {NH}_{4}^{\oplus} + {OH}^{\oplus} \\ [{OH}^{-}] = \sqrt{k_{b} . C}; k_{a} \times k_{b} = 10^{- 14}, [H^{+}] = \frac{k_{w}}{[{OH}^{-}]} [H^{+}] = 9 .268 \times 10^{- 13} \end{array}$

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