Calculate the molar solubility of BaSO4 in 2M Na2SO4 (Ksp = 1.1 x 10-10)2.2 x 10-10M5.5 x 10-11M2M1M

To calculate the molar solubility of BaSO4 in 2M Na2SO4, we need to set up the solubility product expression for the reaction.

The balanced chemical equation for the dissolution of BaSO4 is:

BaSO4(s) ⇌ Ba2+(aq) + SO42-(aq)

The solubility product expression is:

Ksp = [Ba2+][SO42-]

Given that the Ksp of BaSO4 is 1.1 x 10^-10, we can set up the following equation:

1.1 x 10^-10 = [Ba2+][SO42-]

Since BaSO4 is in a solution of Na2SO4, the concentration of SO42- ions is already 2M due to the Na2SO4. Therefore, we can simplify the equation to solve for [Ba2+], which represents the molar solubility of BaSO4:

1.1 x 10^-10 = Ba2+

Divide both sides by 2 to solve for [Ba2+]:

[Ba2+] = 1.1 x 10^-10 / 2 = 5.5 x 10^-11 M

Therefore, the molar solubility of BaSO4 in 2M Na2SO4 is 5.5 x 10^-11 M.