Question

Express $K_{sp}$ in terms of molar solubility, x, for a salt with a formula of AB(s) $K_{sp}$ = AB$_2$(s) $K_{sp}$ = x[2x] AB$_3$(s) $K_{sp}$ = [x][3x] A$_3$B$_2$(s) $K_{sp}$ = [3x][2x] Incorrect. For AB, the solubility of AB(s) $\rightleftharpoons$ A(aq) + B(aq) excess -x 0 +x 0 +x So at equilibrium, [A] = x, [B] = x,

          Express $K_{sp}$ in terms of molar solubility, x, for a salt with a formula of
AB(s)  $K_{sp}$ = 
AB$_2$(s)  $K_{sp}$ = x[2x]
AB$_3$(s)  $K_{sp}$ = [x][3x]
A$_3$B$_2$(s)  $K_{sp}$ = [3x][2x]
Incorrect. For AB, the solubility of
AB(s)  $\rightleftharpoons$ A(aq) + B(aq)
excess
-x
0
+x
0
+x
So at equilibrium, [A] = x, [B] = x,

Express Ksp in terms of molar solubility, x, for a salt with a formula of
AB(s) Ksp =
AB2(s) Ksp = x[2x]
AB3(s) Ksp = [x][3x]
A3B2(s) Ksp = [3x][2x]
Incorrect. For AB, the solubility of
AB(s) ⇌ A(aq) + B(aq)
excess
-x
0
+x
0
+x
So at equilibrium, [A] = x, [B] = x,

Added by Vicente G.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ashley Brady

Step 1

The molar solubility of the salt is represented by x, which means that at equilibrium, the concentration of A⁺ is x and the concentration of B⁻ is also x. The solubility product constant, K_sp, is given by the product of the concentrations of the ions at Show more…

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Express Ksp in terms of molar solubility, x, for a salt with a formula of AB. The solubility equation for AB is AB(s) â‡Œ A+(aq) + B-(aq). Ksp = [A+][B-] So at equilibrium, [A+] = x and [B-] = x. Ksp = (x)(x) = x^2