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Standard XII

Chemistry

Solubility Product

Find the conc...

Question

Find the concentration of $H^{+}$ ion that must be maintained in a saturated solution of $H_{2} S (0.1 M)$ so as to precipitate $C d S$ not $Z n S$
Given: $[C d^{2 +}] = [Z n^{2 +}] = (0.1 M)$ initially.
$K_{s p} (C d S) = 8 \times 10^{- 27} K_{s p} (Z n S) = 1 \times 10^{- 21} K_{s p} (H_{2} S) = 1.1 \times 10^{- 21}$

1.5 M

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0.5 M

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0.1 M

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0.95 M

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Solution

The correct option is C $0.1 M$
In order to prevent precipitation of $Z n S,$
$[Z n^{2 +}] [S^{2 -}] < K_{s p} (Z n S) o r 0.1 \times [S^{2 -}] < 1 \times 10^{- 21} [S^{2 -}] < 1 \times 10^{- 20}$

This is the maximum value of $[S^{2 -}]$ before $Z n S$ will precipitate.

$H_{2} S (s) ⇌ 2 H^{+} (a q) + S^{2 -} (a q) K_{a} = \frac{[H^{+}]^{2} [S^{2 -}]}{[H_{2} S]} = \frac{x^{2} \times 1 \times 10^{- 20}}{0.1} = 1.1 \times 10^{- 21} x = [H^{+}] = 0.1 M$
So, No $Z n S$ will precipitate if concentration of $H^{+}$ greater than 0.1 M.
So, this concentration of $H^{+}$ must be maintained.

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Similar questions

Q. Find the

[H^{+}]

that must be maintained in a saturated

H_{2} S (0.1 M)

to precipitate

C d S

not

Z n S

[C d^{2 +}] = [Z n^{2 +}] = (0.1 M)

initially.

K_{s p} (C d S) = 8 \times 10^{- 27} K_{s p} (Z n S) = 1 \times 10^{- 21} K_{s p} (H_{2} S) = 1.1 \times 10^{- 21}

Q. Find the concentration of

H^{+}

ion that must be maintained in a saturated solution of

H_{2} S (0.1 M)

so as to precipitate

C d S

not

Z n S

Given:

[C d^{2 +}] = [Z n^{2 +}] = (0.1 M)

initially.

K_{s p} (C d S) = 8 \times 10^{- 27} K_{s p} (Z n S) = 1 \times 10^{- 21} K_{s p} (H_{2} S) = 1.1 \times 10^{- 21}

K_{s p}

C d S = 8 \times 10^{- 27}

K_{s p}

Z n S = 1 \times 10^{- 21}

K_{a}

H_{2} S = 1 \times 10^{- 21}

.
What

[H^{+}]

must be maintained in saturated

H_{2} S (0.1 M)

to precipitate

C d S

but not

Z n S

, if

[C d^{2 +}] = [Z n^{2 +}] = 0.1 M

initially?

Q. Maximum

p H

that must be maintained in a saturated

H_{2} S

(0.1 M) to precipitate

C d S

but not

Z n S

x

and concentration of

C d^{2 +}

ion at that

p H

y \times 10^{- 7}

then

x + y =

Given

[C d^{2 +}] = [{Z n}^{2 +}] = 0.1 M

initially

K_{s p} (C d S) = 8 \times 10^{- 27}

K_{s p} (Z n S) = 1 \times 10^{- 21}

K_{a 1} (H_{2} S) = 1.0 \times 10^{- 8}

K_{a 2} (H_{2} S) = 1.0 \times 10^{- 13}

Q. Find the

[H^{+}]

that must be maintained in a saturated

H_{2} S (0.1 M)

to precipitate

C d S

not

Z n S

[C d^{2 +}] = [Z n^{2 +}] = (0.1 M)

initially.

K_{s p} (C d S) = 8 \times 10^{- 27} K_{s p} (Z n S) = 1 \times 10^{- 21} K_{s p} (H_{2} S) = 1.1 \times 10^{- 21}

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Solubility Product

Standard XII Chemistry

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Find the concentration of H+ ion that must be maintained in a saturated solution of H2S (0.1 M) so as to precipitate CdS not ZnS Given: [Cd2+]=[Zn2+]=(0.1 M) initially. Ksp(CdS)=8×10−27Ksp(ZnS)=1×10−21Ksp(H2S)=1.1×10−21