Question

Which of the following salts has the lowest molar solubility? Show work.

A.) SrCO3 (Ksp = 9.3 x 10^-10)

B.) MnS (Ksp = 2.5 x 10^-10)

C.) BaF2 (Ksp = 1 x 10^-6)

D.) BaSO4 (Ksp = 1.1 x 10^-10)

E.) AgCl (Ksp = 1.8 x 10^-10)

Answer 1

a)

SrCO₃ ==== Sr + CO₃

......................x.............x

ksp = x * x = x² = 9.3 x 10^-10

^{solve for x}

x = 3.05 x 10^-5 M

B )

MnS === Mn + S

................x.........x

ksp = x² = 2.5 x 10^-10 M

solve for x

x = 1.58 x 10^-5 M

c) BaF₂ ==== Ba + 2F

......................x..........2x

ksp = (2x)² * x = 1 x 10^-6 M = 4x³

solve for x

x = 0.006 M

D)

BaSO₄ ==== Ba + SO₄

ksp = x² = 1.1 x 10^-10

x = 1.048 x 10^-5 M

E)

AgCl

ksp = 1.8 x 10^-10

x= 1.34 x 10^-5 M

the lowest value and the lowest solubility is for BaSO₄

*hope it helps =)