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Standard XII

Chemistry

Solubility Product

M 2 SO 4 M+...

Question

$M_{2} {S O}_{4}$ ( $M^{+}$ is a monovalent metal ion) has a $K_{s p}$ of $1.2 \times 10^{- 5}$ at $298 K$ . The maximum concentration of $M^{+}$ ion that could be attained in a saturated solution of this solid at $298 K$ is:

3.46 \times 10^{- 3} M

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2.89 \times 10^{- 2} M

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2.8 \times 10^{- 3} M

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7.0 \times 10^{- 3} M

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Solution

The correct option is B $2.89 \times 10^{- 2} M$
Solubility can be expressed as:

$M_{2} {S O}_{4} \to 2 M^{+} + {S O_{4}}^{- 2}$

At eq. $2 S S$

Using the relation $K_{s p} = [M^{+}]^{2} [{S O_{4}}^{- 2}]$

$[M^{+}] = 2 S$

$[{S O_{4}}^{- 2}] = S$

upon substitution we get-

$K_{s p} = (2 S)^{2} (S) = 1.2 \times 10^{- 5}$

$∴ 4 S^{3} = 1.2 \times 10^{- 5}$

$S^{3} = 3 \times 10^{- 6}$

$S = 1.44 \times 10^{- 2} M$

as $[M^{+}] = 2 S = 2.88 \times 10^{- 2} M$

Therefore option $B$ is correct.

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Similar questions

M_{2} S O_{4} (M^{+}

is a monovalent metal ion) has a

K_{s p}

1.2 \times 10^{- 5}

298 K

. The maximum concentration of

M^{+}

ion that could be attained in a saturated solution of this solid at

298 K

is:

Q. The electrochemical cell shown below is a concentration cell,

M | M^{2 +}

(Saturated solution of a sparingly soluble salt,

M X_{2}) | | M^{2 +} (0.001 m o l d m^{- 3}) M .

The emf of the cell depends on the difference in concentration of

M^{2 +}

ions at the two electrodes. The emf of the cell at 298K is 0.059

The solubility product

(K_{s p} : m o l^{3} d m^{- 9})

M X_{2}

at 298 K based on the information available the given concentration cell is (take

2.303 \times R \times 298 / F = 0.059 V)

K_{s p}

for

S r F_{2} = 2.8 \times 10^{- 9}

25^{o} C

. How much

N a F

should be added to

100 m L

of solution having

0.016 M

{S r}^{2 +}

ions to reduce its concentration to

2.5 \times 10^{- 3} M

Q. A solution is saturated with respect to

S r C O_{3}

and

S r F_{2}

. The

[C O_{3}^{2 -}]

was found to be

1.2 \times 10^{- 3} M

. The values of the solubility products of

S r C O_{3}

and

S r F_{2}

are

7.0 \times 10^{- 10}

and

7.9 \times 10^{- 10}

respectively. The concentration of

F^{-}

in the solution would be:

Q. Determine the

K_{s p}

value for

A g C l

, when enough amount of

A g C l (s)

is dissolved in water at

298 K

to produce a saturated solution of having a concentration of

A g^{+}

ions is

1.3 \times 10^{- 5} M

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M2SO4 (M+ is a monovalent metal ion) has a Ksp of 1.2×10−5 at 298K. The maximum concentration of M+ ion that could be attained in a saturated solution of this solid at 298K is:

$M_{2} {S O}_{4}$ ( $M^{+}$ is a monovalent metal ion) has a $K_{s p}$ of $1.2 \times 10^{- 5}$ at $298 K$ . The maximum concentration of $M^{+}$ ion that could be attained in a saturated solution of this solid at $298 K$ is: