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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

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Solubility Product

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