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Question

# If a 25 mL 5.0×10−4M Ca2+ solution and 25 mL 2.5×10−4M C2O2−4 solution are mixed, then which of the following option is correct ? Given: Ksp(CaC2O4)=2.3×10−9.

A
Precipitate is formed
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B
No precipitate is formed
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C
Can't be determined.
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D
None of the above
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Solution

## The correct option is A Precipitate is formedAfter mixing, Total volume= 25+25=50 ml. To calculate [Ca2+] using the formula: M1V1=M2V2 (5.0×10−4M)×(25 mL)=M2×(50mL) [Ca2+]=2.5×10−4 M Calculate [C2O2−4] using the formula: M1V1=M2V2 (2.5×10−4M)(25mL)=M2(50mL) [C2O2−4]=1.25×10−4 M Ionic Product=[Ca2+][C2O2−4]=[2.5×10−4][1.25×10−4]=3.125×10−8 Since Ionic Product>Ksp ⇒Precipitate is formed.

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