Question

Prove the following relations using the principles of electroneutrality and mass balance

            a.) [NO₂^-] = [H⁺] - [OH^-]                                    for a 0.2 M HNO₂ solution

            b.) [CH₃COOH] = 0.2 - [H⁺] + [OH^-]                  for a 0.2 M [CH₃COOH] solution

            c.) [H₂C₂O₄] = 0.1- [H⁺] + [OH^-] – [C₂O₄^2-]        for a 0.1 M H₂C₂O₄ solution

            d.) [HNC] = [OH^-] - [H⁺]                                    for a 0.1 M KCN solution

           

e.) [H₂PO₄^-]= ( [OH^-] - [H⁺] – [HPO₄^2-] – 3[H₃PO₄] ) / 2   

                                                                        for a 0.1 M Na₃PO₄

               

f.) [HSO^4-] = 0.2 – [H⁺] – [OH^-]                         for a 0.1 M H₂SO₄ solution

                                                           

(assume that the dissociation of H₂SO₄ to H⁺ and HSO^4- is quantitive).

Answer 1