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Arrhenius Acid

Which of the ...

Question

Which of the following concentrations of $N H_{4}^{+}$ will be sufficient to prevent the precipitation of $M g (O H)_{2}$ form a solution which is 0.01 M $M g C l_{2}$ and 0.1 M $N H_{3}$ (aq) .

Given that : $K_{S P}$ of $M g (O H)_{2} = 2.5 \times 10^{- 11}$ and $K_{b}$ for $N H_{3} (a q) = 2 \times 10^{- 5}$

A

0.01 M

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B

0.002 M

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C

0.001 M

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D

0.04 M

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Solution

The correct option is D 0.04 M
$K_{S P} = [M g^{+ 2}] [O H^{-}]^{2}$

$[O H^{-}] = \sqrt{\frac{2.5 \times 10^{- 11}}{0.01}} = 5 \times 10^{- 5}$

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

$S o, [N H_{4}^{+}] = 0.04 M$

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Similar questions

Q. Which of the following concentrations of

N H_{4}^{+}

will be sufficient to prevent the precipitation of

M g (O H)_{2}

from solution is 0.01 M

M g C l_{2}

0.1 M N H_{3} (a q)

K_{s p}

M g (O H)_{2} = 2.5 \times 10^{- 11}

K_{b}

N H_{2} (a q) = 2 \times 10^{- 5}

Q. Which of the following concentrations of

N H_{4}^{+}

will be sufficient to prevent the precipitation of

M g (O H)_{2}

from a solution which is

0.01 {M MgCl}_{2}

0.1 {M NH}_{3} (a q)

? Given that the

K_{s p}

M g (O H)_{2} = 2.5 \times 10^{- 11}

K_{b}

N H_{3} (a q) = 2 \times 10^{- 5}

.

Q. Which of the following concentrations of

N H_{4}^{+}

will be sufficient to prevent the precipitation of

M g (O H)_{2}

from a solution which is

0.01 {M MgCl}_{2}

0.1 {M NH}_{3} (a q)

? Given that the

K_{s p}

M g (O H)_{2} = 2.5 \times 10^{- 11}

K_{b}

N H_{3} (a q) = 2 \times 10^{- 5}

.

Q. Calculate pH at which

M g (O H)_{2}

begin to precipitate form a solution containing 0.1 M

M g^{2 +}

K_{s p}

M g (O H)_{2} = 1 \times 10^{- 11}

Q. A solution has

0.05 M M g^{2 +}

0.05 M N H_{3}

. Calculate the concentration of

N H_{4} C l

required to prevent the formation of

M g (O H)_{2}

in this solution.

K_{s p} of M g (O H)_{2} = 9.0 \times 10^{- 12}

and ionization constant of

N H_{3} = 1.8 \times 10^{- 5}

\sqrt{1.8} = 1.34

)

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