Calculate the solubility of calcium sulfate 0.010 mol/L calcium nitrate at SATP

CaSO4 ==> Ca^+2 + SO4^=

Ca(NO2)2 ==> Ca^+2 + 2NO3^- = 0.01 M
Ksp CaSO4 = (Ca^+2)(SO4^=) = ??. Look up Ksp for CaSO4.

Subsitute 0.01 for Ca^+2 and x for SO4^= and solve for solubility CaSO4. Post your work if you get stuck.

To calculate the solubility of calcium sulfate in a solution of 0.010 mol/L calcium nitrate at SATP (Standard Ambient Temperature and Pressure), you need to know the solubility product constant (Ksp) of calcium sulfate. The expression for the solubility product constant of calcium sulfate is:

CaSO4 (s) ⇌ Ca2+ (aq) + SO4^2- (aq)

The Ksp value for calcium sulfate is approximately 4.93 x 10^-5 at SATP.

To calculate the solubility of calcium sulfate in the given solution, we need to consider the reaction between calcium nitrate and calcium sulfate:

Ca(NO3)2 (aq) + CaSO4 (s) ⇌ 2Ca^2+ (aq) + SO4^2- (aq) + 2NO3^- (aq)

Since we know the molar concentration of calcium nitrate is 0.010 mol/L, we can use the stoichiometry of the balanced equation to determine the molar concentration of calcium sulfate.

The molar concentration of calcium sulfate can be calculated using the formula:

[S = (x) / (V - x)]

Where:
S = solubility of calcium sulfate
x = molar concentration of calcium sulfate
V = total volume of the solution

In this case, since we are given the molar concentration of calcium nitrate and assuming the volume of the solution is known, we can substitute these values into the formula to calculate the solubility of calcium sulfate.