Question

Assume you dissolve 0.103 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.0x10^2 mL of solution and then titrate the solution with 0.113 M NaOH. (Ka for benzoic acid = 6.3x10^-5)

C6H5CO2H(aq) + OH^- (aq) = C6H5CO2 ^ - (aq) + H2O (l) * = means arrows both ways

a) What was the pH of the original benzoic acid solution? ______

b) What are the concentrations of all of the following ions at the equivalence points :

Na+ _____ M

H3O+ ______ M

OH- _______ M

C6H5CO2- _____ M

c) What is the pH of the solution at the equivalence points?

Please answer!!