Question

Write a balanced net ionic equation to show why the solubility of mg(oh)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. use the pull-down boxes to specify states such as (aq) or (s). + + k =

Answer 1

Net ionic equation

Mg(OH)2(s) + 2H+(aq) → Mg^2+(aq) + 2H20(l)

Kc = [MgCl2](aq) / [HCl]²(aq)

Step-by-step explanation:

Step 1: Data given

Suppose the strong acid = HCl

Step 2: The balanced equation

Mg(OH)2(s) + HCl(aq) → ...

Mg(OH)2(s) + 2H+(aq) + 2Cl-(aq) → MgCl2(aq) + 2H2O(l)

Net ionic equation

Mg(OH)2(s) + 2H+(aq) + 2Cl-(aq) → MgCl2(aq) + 2H2O(l)

Mg(OH)2(s) + 2H+(aq) + 2Cl-(aq) → Mg^2+(aq) + 2Cl-(aq) + 2H20(l)

Mg(OH)2(s) + 2H+(aq) → Mg^2+(aq) + 2H20(l)

MgCl2 is more soluble than Mg(OH)2 so the solubility increases.

Is the question asking for the equilibrium constant for Pb(OH)2 or for PbCl2?

Equilibrium constant

Mg(OH)2(s) + 2HCl aq) → MgCl2(aq) + 2H2O(l)

Kc = [MgCl2](aq) / [HCl]²(aq)