Consider the compounds with the generic formula listed and their corresponding molar solubilities in pure water. Which compound has the smallest value of Ksp?

a. AC; molar solubility = 1.35 x 10^-4 M
b. AX2; molar solubility = 2.25 x 10^-4 M
c. A2X; molar solubility= 1.75 x 10^-4 M

Is it a?

To determine which compound has the smallest value of Ksp, we need to compare the molar solubilities and their corresponding formulas.

The formula for the compound with the smallest value of Ksp will have the lowest molar solubility.

Comparing the molar solubilities:

a. AC; molar solubility = 1.35 x 10^-4 M
b. AX2; molar solubility = 2.25 x 10^-4 M
c. A2X; molar solubility= 1.75 x 10^-4 M

Based on the given molar solubilities, compound AC has the smallest molar solubility. Therefore, compound AC has the smallest value of Ksp.

To determine which compound has the smallest value of Ksp, we need to compare the molar solubilities of the compounds. The Ksp is the solubility product constant, and it is a measure of how much of a compound will dissolve in water.

The solubility product constant (Ksp) can be calculated by multiplying the concentrations of the constituent ions raised to their stoichiometric coefficients. In this case, the generic formula is AaXb, so the Ksp for each compound will be [A]a[X]b.

Let's calculate Ksp for each compound using the given molar solubilities:

a. AC: molar solubility = 1.35 x 10^-4 M
Ksp = [A]^1[C]^1

b. AX2: molar solubility = 2.25 x 10^-4 M
Ksp = [A]^1[X]^2

c. A2X: molar solubility = 1.75 x 10^-4 M
Ksp = [A]^2[X]^1

To compare the compounds, we need to calculate the Ksp values. However, we don't know the exact concentrations of the ions A and X, as their stoichiometry is not provided. Therefore, we cannot determine the order of Ksp values and identify the compound with the smallest Ksp based on the given information.

Hence, we cannot definitively say that compound "a" has the smallest value of Ksp without additional information.

Why not simply calculate the solubililty of each.