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The solubility of CuBr is 2xx10^(-4) mol...

The solubility of `CuBr` is `2xx10^(-4)` mol/litre at `25^(@)C`. The `K_(sp)` value for `CuBr` is

A

` 4 xx 10^(-8) "mol"^(2)L^(-2)`

B

` 4 xx 10^(-4) "mol"^(2)L^(-2)`

C

` 4 xx 10^(-11) "mol"^(2)L^(-2)`

D

` 4 xx 10^(-15) "mol"^(2)L^(-2)`

Text Solution

Verified by Experts

The correct Answer is:
A
`CuBr to Cu^(+)+Br^(-)`
Solubility of CuBr is ` 2 xx 10^(-4) ` mol `L^(-1)`
Therefore , solubility of `Cu^(+)= 2 xx 10^(-4) ` mol `L^(-1)`
`implies ` Solubility product `=2 xx 10^(-4) xx 2 xx 10^(-4)`
`= 4 xx 10^(-8) mol^(2)L^(-2)`
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