Answer to Question #237101 in General Chemistry for Nana

Question

Determine the solubility of BaF₂ in g/L if K_sp of BaF₂ = 1 × 10^-6. (Please give your answer with 2 significant figures.)

Answer 1

when we have this compound in water then there is no common ion and both the ions comes from the compound. if the molar solubility of BaF2 is s then Ba2+ will be s and F- will be 2s.

The Ksp expresion would be,,,

Ksp = [Ba2+] [F-]2

Ksp for BaF2 is 1.0 x 10-6. So,....

1.0 x 10-6 = (s) (2s)2 = 4s3

s = cube root of [(1.0 x 10-6)/4]

s = 0.00630 mol/L

molar mass of BaF2 is 175.34 g/mol

so, the solubility of BaF2 in g/L would be...

0.00630mol/L x 175.34 g/mol = 1.10 g/L