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Solubility Product

If 100 mL of ...

Question

If $100 m L$ of $0.002 M$ $A g N O_{3}$ solution is mixed with $100 m L$ of $0.05 M$ $K_{2} C r O_{4}$ solution. Then, select the correct option regarding the precipitation of $A g_{2} C r O_{4}$ .
Given : $K_{s p}$ of $A g_{2} C r O_{4} = 1.1 \times 10^{- 12} .$

Precipitation occurs

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Precipitation does not occur

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Can't be determined from given data

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None of these

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Solution

The correct option is A Precipitation occurs
Final volume of the solution $= 100 + 100 = 200 m L$

To calculate $[A g^{+}]$ using the formula:

$M_{1} V_{1} = M_{2} V_{2}$
$0.002 M \times (100 m L) = M_{2} \times (200 m L)$
$[A g^{+}] = 0.001 M$

Calculate $[C r O_{4}^{2 -}]$ using the formula:
$M_{1} V_{1} = M_{2} V_{2}$
$0.05 M \times (100 m L) = M_{2} \times (200 m L)$
$[C r O_{4}^{2 -}] = 0.025 M$

Ionic product for $A g_{2} C r O_{4}$ solution :
$A g_{2} C r O_{4} (s) ⇌ 2 A g^{+} (a q) + C r O_{4}^{2 -} (a q)$

Ionic product $= [A g^{+}]^{2} [C r O_{4}^{2 -}]$
$= (1.0 \times 10^{- 3})^{2} (2.25 \times 10^{2 -})$
$= 2.25 \times 10^{- 8}$

Ionic product $> K_{s p}$
$∴$ precipitation occurs.

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Similar questions

Q. 15 mL of 0.05 M

A g N O_{3}

is mixed with 45 mL of 0.03 M

K_{2} C r O_{4}

. Then, which of the following is correct regarding

A g_{2} C r O_{4}

K_{s p}

A g_{2} C r O_{4} = 1.9 \times 10^{- 12} .

Q. If

100 m L

0.002 M

A g N O_{3}

solution is mixed with

100 m L

0.05 M

K_{2} C r O_{4}

solution. Then, select the correct option regarding the precipitation of

A g_{2} C r O_{4}

.
Given :

K_{s p}

A g_{2} C r O_{4} = 1.1 \times 10^{- 12} .

Q. 100 mL of a clear saturated solution of

A g_{2} S O_{4}

is added to 250 mL of a clear saturated solution of

P b C r O_{4}

. What is the precipitate formed? Given,

K_{s p}

values for

A g_{2} S O_{4}, A g_{2} C r O_{4}, P b C r O_{4}

and

P b S O_{4}

are

1.4 \times 10^{- 5}, 2.4 \times 10^{- 12}, 2.8 \times 10^{- 13}

and

1.6 \times 10^{- 5}

respectively.

100 m L

of a saturated solution of

A g_{2} S O_{4}

is added to

250 m L

of a saturated solution of

P b C r O_{4}

. Will any precipitate form and if so what?

Given that :

K_{s p}

for

A g_{2} S O_{4}, A g_{2} C r O_{4}, P b C r O_{4}

and

P b S O_{4}

are

1.4 \times 10^{- 5},

2.4 \times 10^{- 12},

2.8 \times 10^{- 13}

and

1.6 \times 10^{- 8}

respectively.

50.0ml of $A g N O_{3}$ solution of 0.05 M is mixed with 50.0ml of 0.01M $K B r O_{3}$ solution. Will the precipitate of $A g B r O_{3}$ be formed?

Given : $K_{s p}$ of $A g B r O_{3}$ = $6.0 \times 10^{- 5}$

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Solubility Product

Standard XII Chemistry

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If 100 mL of 0.002 M AgNO3 solution is mixed with 100 mL of 0.05 M K2CrO4 solution. Then, select the correct option regarding the precipitation of Ag2CrO4 . Given : Ksp of Ag2CrO4=1.1×10−12.

If $100 m L$ of $0.002 M$ $A g N O_{3}$ solution is mixed with $100 m L$ of $0.05 M$ $K_{2} C r O_{4}$ solution. Then, select the correct option regarding the precipitation of $A g_{2} C r O_{4}$ .
Given : $K_{s p}$ of $A g_{2} C r O_{4} = 1.1 \times 10^{- 12} .$