Question

A friend tells you: “The constant ${\mathbf{K}}_{\mathbf{sp}}$of a salt is called the solubility product constant and is calculated from the concentrations of ions in the solution. Thus, if salt A dissolves a greater extent than salt B, salt A must have a higher ${\mathbf{K}}_{\mathbf{sp}}$ than salt B.” Do you agree with your friend? Explain.

Short answer

Agreed with the friend, the Solubility product is referred to as ${\text{K}}_{\text{sp}}$and that is proportional to the concentration of ions forming in the solution. More soluble salts are dissolving more in the solutions. Therefore, there can be a higher${\text{K}}_{\text{sp}}$ for salt A, if it dissolves to a greater extent than salt B.

Step-by-step solution

Definition of solubility

Solubility is the property of molecules of the solute and solvent forming a new bond.

Explanations

Solubility product is the equilibrium constant of molar concentrations of the individual ions of a compound, raised to the power of their respective stoichiometric coefficient and that constant is a constant at a given temperature.

$\begin{array}{l}{\text{A}}_{\text{m}}{\text{B}}_{\text{n}}\text{(s)}\rightleftharpoons {\text{mA}}^{\text{n+}}\text{(aq)}+{\text{nB}}^{\text{m-}}\text{(aq)}\\ {\text{K}}_{\text{sp}}={\left[{\text{A}}^{\text{n+}}\right]}^{\text{m}}{\left[{\text{B}}^{\text{m-}}\right]}^{\text{n}}\end{array}$

There can be a higher ${\mathbf{K}}_{\mathbf{sp}}$ for salt A, if it dissolves to a greater extent than salt B.