1 in the determination of an equilibrium constant of a weak, Ask an Expert

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1. In the determination of an equilibrium constant of a weak acid, why isn't it necessary to know the concentration of the weak acid?

2. 41.89 mL of NaOH were required to completely titrate 25.00mL of a weak monoprotic acid. After 11.90 mL of NaOH had been added to the solution, the pH of the solution was 6.81. Calculate Ka and pKa for this weak acid.

3. A .45 M solution of NH4Cl has an acidic pH.

a) Write a net ionic equation accounting for this.

b) For the reaction in part a, write the equilibrium constant expression and calculate the equilibrium constant from a consideration of Kb and Kw.

c) Calculate the [H3O+] for a .45 M NH4Cl solution.

d) Calculate the degree (percent) of hydrolysis of .45 M NH4Cl.

e) For each of the salts listed below, indicate whether its water solution would be acidic, basic, or neutral.

NaBr, Na2CO3, KHSO4, KCN, NH4CH3COO, BaF2

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Category:- Chemistry
Reference No.:- M9865598

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