The solubility of BaSO4 in water is 2.4...

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

A

`1.08 xx10^(-14)mol^2L^-2`

B

`1.08 xx10^(-12)mol^2L^-2`

C

`1.08 xx10^(-10)mol^2L^-2`

D

`1.08 xx10^(-8)mol^2L^-2`

Verified by Experts

The correct Answer is:

C

Similar Questions

Explore conceptually related problems

The solubility of Sb_(2)S_(3) in water is 1.0 xx 10^(-5) mol/letre at 298K. What will be its solubility product ?

The solubility of Sb_(2)S_(3) in water is 1.0 xx 10^(-8) mol/litre at 298 K. What will be its solubility product:

The solubility of a springly soluble salt AB_(2) in water is 1.0xx10^(-5) mol L^(-1) . Its solubility product is:

The solubility of CaF_2 in water at 298 K is 1.7 xx 10 ^(-3) grams per 100 cm ^(3) .Calculate the solubility product of CaF_2 at 298 K.

Solubility of CaF_(2) is 0.5xx10^(-4)" mol L"^(-1) . The value of K_(sp) for the salt is

The solubility of AgCl in water at 298 K is 1.06xx10^(-5) mole per litre. Calculate its solubility product at this temperature.

The solubility of AgCl in water at 298 K is 1.06xx10^(-5) mle per litre. Calculate its solubility product at this temperature.

The solubility in water of a sparingly soluble salt AB_2 is 1.0 xx 10 ^(-5) " mol " L^(-1) . Its solubility product number will be

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

The solubility of AgCl at 298 K is 1.3 xx 10 ^(-5) " mol " L^(-1) Calculate the value of K_(sp) at this temperature.