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. Be sure to specify states such as (aq) or (s). K = + ? +
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Data given
Suppose the strong acid = HCl
• The balanced equation is :-
When Mg(OH)2 reacts with HCl then,
Mg(OH)2 (s) + 2HCl (aq) ---> MgCl2(aq) + 2H2O(l) .
Net ionic equation is :-
• Mg(OH)2(s) + 2H+(aq) + 2Cl-(aq)---> MgCl2(aq) + 2H2O(l)
• Mg(OH)2(s) + 2H +(aq) + 2Cl-(aq)---> Mg2+(aq) + 2Cl- (aq) + 2H2O(l)
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