Two compounds with general formulas a2x and ax3 have ksp=1.5×10−5m. part a which of the compounds has the higher molar solubility? which of the compounds has the higher molar solubility? a2x ax3

A₃X

Explanation:

In order to find the molar solubility (S) of a compound, we will use an ICE Chart.

A₂X

Let's consider the solution of A₂X.

     A₂X(s) ⇄ 2 A⁺(aq) + X²⁻(aq)

I                         0           0

C                     +2S        +S

E                       2S          S

The solubility product (Kps) is:

Kps = 1.5 × 10⁻⁵ = [A⁺]².[X²⁻] = (2S)².S = 4S³

S = 0.016 M

A₃X

Let's consider the solution of A₃X.

     A₃X ⇄ 3 A⁺(aq) + X³⁻(aq)

I                    0             0

C                 +3S         +S

E                   3S           S

The solubility product (Kps) is:

Kps = 1.5 × 10⁻⁵ = [A⁺]³.[X³⁻] = (3S)³.S = 27 S⁴

S = 0.027 M

A₃X has a higher molar solubility than A₂X.

we can conclude that the melting point of table salt is above room temperature (it's actually 801 deg c). the melting point of mercury must be below room temperature (- 39 deg c).