ionic equations: solved examples

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Problem strategy: You will need to convert the molecular equation to complete ionic equation , then cancel spectator ions to obtain the net ionic equation.For the complete ionic equation,represent all of the strong electrolytes by their separate ions in solution,addding (aq0 after formula of each.Retain the formulas of the other compounds.A compound should have (aq) after its formula if it is soluble or (s) if it is insoluble


(a)  Ca(OH)2 and Ca(ClO4)2 (aq) are souble ionice compounds, so are strong electrolytes.HClO4 is also strong electrolyte.You write each strong electrolyte in the form of seperate ions.Water H2O is a nonelectrolyte so you retain its molecular formula.The complete ionic equation is


2H+ (aq) + 2ClO4-(aq) + Ca2+ + 2H+ (aq) ----------> Ca2+ (aq)  + 2ClO4-2H+ (aq)+ 2H2O (l)


after cancelling spectator ions and dividing by 2,you get the following net ionic equation;


H+ (aq) + H+ (aq) ----------> H2O (l)


(b) NaOH and NaC2H3O2 are soluble ionic compounds so are strong electrolytes.The problem statement notes that HC2H3O2 is a weak electrolyte,which you write be its molecular formula.Water H2O is a  nonelectrolyte,so you retain its molecular formula also.The complete ionic equation is


HC2H3O2 (aq) + Na+(aq) + OH-(aq)  ----------> Na+(aq) + C2H3O2-(aq)+ H2O (l) 


and the net ionic equation is


HC2H3O2 (aq)  + OH-(aq) ----------> C2H3O2-(aq)+ H2O (l)

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