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Standard XII

Chemistry

Common Ion Effect

The solubilit...

Question

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:

10^{- 9} M

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10^{- 8} M

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10^{- 7} M

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10^{- 6} M

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Solution

The correct option is D $10^{- 6} M$
$K_{s p} = 1.5 \times 10^{- 9}$
$Q_{s p} = [0.01] [B^{-}]$
The precipitation will occur when $Q_{s p}$ is greater than $K_{s p}$ and it will possible when $[S O_{4}^{2 -}] = 10^{- 6}$ .

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Similar questions

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:

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. An aqueous solution contains an unknown concentration of

B a^{2 +}

. When 50 mL of 1 M solution of

N a_{2} S O_{4}

is added,

B a S O_{4}

just begins to precipitate. The final volume is 500 mL. The solubility product of

B a S O_{4}

1 \times 10^{- 10}

. What is the original concentration of

B a^{2 +}

Q. If the concentration of

A^{+}

ions in a solution of a sparingly soluble salt,

A B

10^{- 3} M .

Find the concentration of

B^{-}

ions at which the precipitation of

A B

starts.
Given : Solubility product of AB is

1.0 \times 10^{- 8}

Q. An aqueous solution contains an unknown concentration of

{B a}^{2 +}

. When

50 m l

of a

1 M

solution of

{N a}_{2} {S O}_{4}

is added,

{B a S O}_{4}

just begins to precipitate. The final volume is

500 m l

. The solubility product of

{B a S O}_{4}

1 \times 10^{- 10}

. What is the original concentration of

{B a}^{2 +}

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The solubility product of BaSO4 is 1.5×10−9. The precipitation in a 0.01M Ba2+ ions solution will start on adding H2SO4 of concentration:

The correct option is D 10−6MKsp=1.5×10−9Qsp=[0.01][B−]The precipitation will occur when Qsp is greater than Ksp and it will possible when [SO2−4]=10−6.

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:

The correct option is D $10^{- 6} M$
$K_{s p} = 1.5 \times 10^{- 9}$
$Q_{s p} = [0.01] [B^{-}]$
The precipitation will occur when $Q_{s p}$ is greater than $K_{s p}$ and it will possible when $[S O_{4}^{2 -}] = 10^{- 6}$ .