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The concentration of saturated solution ...

The concentration of saturated solution of `Mg(OH)_2` is `8.2 xx 10^(-4) g L^(-1)` at 298 K temp. Then calculate its solubility product.

Text Solution

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`1.121xx10^(-14) ("mol L"^(-1))^3`
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Knowledge Check

  • The solubility of BaSO_4 in water is 2.42 xx 10^(-3) gL^(-1) at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO_4 = 233 g "mol"^(-1) )

    A
    `1.08 xx 10^(-8) "mol"^2 L^(-2)`
    B
    `1.08 xx 10^(-10) "mol"^2 L^(-2)`
    C
    `1.08 xx 10^(-14) "mol"^2 L^(-2)`
    D
    `1.08 xx 10^(-12) "mol"^2 L^(-2)`

  • If pH of a saturated solution of Ba(OH)_2 is 12, the value of its K_((Sp)) is :

    A
    `4.0xx10^(-6) M^3`
    B
    `4.0xx10^(-7)M^3`
    C
    `5.0xx10^(-6) M^3`
    D
    `5.0xx10^(-7) M^3`

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