Question

Express Ksp in terms of molar solubility, x , for the salts with the given formulas. ab(s) Ksp= ab2(s) Ksp= ab3(s) Ksp= a3b2(s) Ksp=

Answer 1

The molar solubility product (Ksp) of the salts is as follows:

• $\mathbf{Ksp = x^2}$
• $\mathbf{Ksp = 4x^3}$
• $\mathbf{Ksp = 27x^4}$
• $\mathbf{Ksp = 108x^5}$

What is Molar Solubility?

The solubility product (Ksp) is the equilibrium constant for the dissolution of a substance. The solubility product (Ksp) of a chemical substance is the fraction of concentrations at equilibrium

Given that:

• The molar solubility of the salt  = x

For the salt AB(s), we have:

$\mathbf{AB_{(s) } \leftrightharpoons A^+_{(aq)} + B^-_{(aq)} }$

$\mathbf{[ A^+] = [B^-] = x}$

$\mathbf{Ksp = [ A^+] [B^-] = x^2}$

For the salt AB²(s), we have:

$\mathbf{AB^2_{(s) } \leftrightharpoons A^+_{(aq)} + 2B^-_{(aq)} }$

$\mathbf{Ksp = [ A^+] [2B^-]^2}$

$\mathbf{Ksp = [ x] [2x]^2} \\ \\ \mathbf{Ksp =4x^3}$

For the salt AB³(s), we have:

$\mathbf{AB^3_{(s)} \leftrightharpoons A^+(aq) + 3B^-_{(aq)}}$

$\mathbf{Ksp = [ A^+] [3B^-]^3 } \\ \\ \mathbf{ Ksp = [ x] [3x]^3 } \\ \\ \mathbf{Ksp= 27x^4}$

For the salt A³B²(s), we have:

$\mathbf{A^3B^2_{(s)} \leftrightharpoons 3A^+(aq) + 2B^-(aq)}$

$\mathbf{Ksp = [ 3A^+] [2B^-]^3} \\ \\ \mathbf{Ksp = [ 3x]^3 [2x]^2} \\ \\ \mathbf{Ksp = 108x^5}$

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