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 =

Net ionic equation

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

Kc = [MgCl2](aq) / [HCl]²(aq)

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)

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.