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Standard XII

Chemistry

Solubility Product

The solubilit...

Question

The solubility product of $B a S O_{4}$ at $25^{o}$ C is $1.0 \times 10^{- 9}$ . What would be the minimum concentration of $H_{2} S O_{4}$ necessary to precipitate $B a S O_{4}$ from a solution of $0.01$ M $B a^{+ 2}$ ions?

10^{- 9}

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10^{- 8}

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10^{- 7}

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10^{- 6}

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Solution

The correct option is D $10^{- 7}$
$K s p = [B a^{2 +}] [S O_{4}^{2 -}]$

$10^{- 9} = 0.01 \times x$

$x = [S O_{4}^{2 -}] = 10^{- 7}$ M

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Similar questions

The solubility product of $B a S O_{4}$ at $25^{\circ} C$ is $1.0 \times 10^{- 9}$ . What would be

the concentration of $H_{2} S O_{4}$ necessary to precipitate $B a S O_{4}$ from a solution

of $0.01 M$ $B a^{2 +}$ ions ?

The solubility product of $B a S O_{4}$ is $1.5 \times 10^{- 9}$ . The precipitation in a $0.01 M$ $B a^{2 +}$ ions solution will start on adding $H_{2} S O_{4}$ of concentration -

Q. The solubility product of

B a S O_{4}

1.5 \times 10^{- 9}

. The precipitation in a

0.01 M

B a^{2 +}

solution will start on adding

H_{2} S O_{4}

of concentration:

Q. What is the minimum concentration of

B a^{+ 2}

ions required in order to initiate the precipitation of

B a S O_{4}

from a solution containing

0.002 m o l L^{- 1}

S O_{4}^{- 2}

ions?
(Given

K_{s p}

for

B a S O_{4} = 1.4 \times 10^{- 10}

)

Q. The solubility product of

{B a S O}_{4}

1.5 \times 10^{- 9}

. The precipitation in a

0.01 M {B a}^{2 +}

ions solution will start on adding

H_{2} {S O}_{4}

of concentration?

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The solubility product of BaSO4 at 25oC is 1.0×10−9. What would be the minimum concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01 M Ba+2 ions?

The correct option is D 10−7Ksp=[Ba2+][SO2−4]10−9=0.01×xx=[SO2−4]=10−7M

The solubility product of $B a S O_{4}$ at $25^{o}$ C is $1.0 \times 10^{- 9}$ . What would be the minimum concentration of $H_{2} S O_{4}$ necessary to precipitate $B a S O_{4}$ from a solution of $0.01$ M $B a^{+ 2}$ ions?

The correct option is D $10^{- 7}$
$K s p = [B a^{2 +}] [S O_{4}^{2 -}]$

$10^{- 9} = 0.01 \times x$

$x = [S O_{4}^{2 -}] = 10^{- 7}$ M