Answer to Question #63474 in General Chemistry for Jack

Question

4-Boric acid (H3BO3), Ka = 5.4 × 10−10, is frequently used as an eyewash. Determine the percent hydrolysis of 0.11 M boric acid solution.


5- By coincidence, the Kb of (C2H5)3N and the Ka of HNO2 are both 5.6 × 10-4 . Write appropriate acid-base equilibrium reactions and use them to determine whether each of solutions would be acidic, basic, or neutral. Don’t forget to indicate the phase of reactants and products.


a) HNO2


b) (C2H5)3N


c)(C2H5)3NHCl


d)NaNO2


e)(C2H5)3NHNO2






6-For each of the following, complete the reaction. Include charge (if any) and phase. Also, indicate whether the equilibrium will favor the reactants or products. Briefly justify your answer.


a) C2H5NH2(aq) + HSO4 - (aq)


b) NH4 + (aq) + PO4 3- (aq)


c) C5H5N (aq) + HCN (aq)




7-Determine the concentrations of the ionic species present in a 0.0156 M solution of the Cs2HPO3. (pKa1=1.30, pKa2=6.70 for H3PO3).