Calculate the molar solubility of BaSO4. (Ksp = 1.1 x 10-10)1.05 x 10-5M2.69 x 10-4M2.14 x 10-4M1.33 x 10-6M

The molar solubility of BaSO4 can be calculated using the Ksp (solubility product constant). The dissolution of BaSO4 in water can be represented by the following equation:

BaSO4(s) ⇌ Ba2+(aq) + SO42-(aq)

From this equation, we can see that for every mole of BaSO4 that dissolves, one mole of Ba2+ and one mole of SO42- are produced. Therefore, if we let x represent the molar solubility of BaSO4, then the concentrations of Ba2+ and SO42- in the solution at equilibrium are both x.

The Ksp expression for this reaction is:

Ksp = [Ba2+][SO42-] = x * x = x^2

We can solve this equation for x (the molar solubility of BaSO4) by taking the square root of both sides:

x = sqrt(Ksp) = sqrt(1.1 x 10^-10) = 1.05 x 10^-5 M

So, the molar solubility of BaSO4 is 1.05 x 10^-5 M.