On the basis of the Ksp values below, what is the order of the solubility from least soluble to most soluble for these compounds?

AgBr: Ksp = 5.4 x 10-13

Ag2CO3: Ksp = 8.0 x 10-12

AgCl: Ksp = 1.8 x 10-10

Ag2CO3 < AgBr < AgCl

AgBr < Ag2CO3 < AgCl

AgBr < AgCl < Ag2CO3

AgCl < Ag2CO3 < AgBr

The order of solubility is AgBr < Ag₂CO₃ < AgCl

Explanation:

The solubility constant give us the molar solubilty of ionic compounds. In general for a compound AB the ksp will be given by:

Ksp = (A) (B) where A and B are the molar solubilities = s² (for compounds with 1:1 ratio).

It follows then that the higher the value of Ksp the greater solubilty of the compound if we are comparing compounds with the same ionic ratios:

Comparing AgBr: Ksp = 5.4 x 10⁻¹³ with AgCl: Ksp = 1.8 x 10⁻¹⁰, AgCl will be more soluble.

Comparing Ag2CO3: Ksp = 8.0 x 10⁻¹² with AgCl Ksp = AgCl: Ksp = 1.8 x 10⁻¹⁰ we have the complication of the ratio of ions 2:1 in Ag2CO3, so the answer is not obvious. But since we know that

Ag2CO3 ⇄ 2 Ag⁺ + CO₃²₋

Ksp Ag2CO3 = 2s x s = 2 s² = 8.0 x 10-12

s = 4 x 10⁻12 ∴ s = 2 x 10⁻⁶

And for AgCl

AgCl ⇄ Ag⁺ + Cl⁻

Ksp = s² = 1.8 x 10⁻¹⁰ ∴ s = √ 1.8 x 10⁻¹⁰ = 1.3 x 10⁻⁵

Therefore, AgCl is more soluble than Ag₂CO₃

The order of solubility is AgBr < Ag₂CO₃ < AgCl

5.4 x 10^-13

Explanation:

Edmentum says it is correct