# Answer to Question #40175 in Inorganic Chemistry for Farhan Mutlib

Question #40175

A saturated solution of BaF2 has 0.0200 g dissolved in 15.0 mL .

M(BaF2) = 175.34 g mol–1

Calculate the solubility of BaF2 in mol L–1.

s(BaF2) = 7.60427 × 10–3 mol L–1

Calculate the ion concentrations from the molar solubility.

[Ba2+] = 7.60427 × 10–3

[F–] = 1.520854 × 10–2

Calculate Ks(BaF2).

Ks(BaF2) = × 10–6 (3 sf)

How do i work out Ks?

M(BaF2) = 175.34 g mol–1

Calculate the solubility of BaF2 in mol L–1.

s(BaF2) = 7.60427 × 10–3 mol L–1

Calculate the ion concentrations from the molar solubility.

[Ba2+] = 7.60427 × 10–3

[F–] = 1.520854 × 10–2

Calculate Ks(BaF2).

Ks(BaF2) = × 10–6 (3 sf)

How do i work out Ks?

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