Question

Assume you dissolve 0.303 g of the weak acid benzoic acid C6H5CO2H, , in enough water to make 1.00 x10^2 mL of solution and then titrate the solution with 0.178 M NaOH. ( Ka for benzoic acid = 6.3x 10^-5 .)

C6H5CO2H + OH- < ------> C6H5CO2- + H2O

A. What was the ph of the original benzoic acid solution?

pH = _____

B. What are the concentrations of all of the following ions at the equivalence point Na+, H3O+, OH-, and C6H5CO2-

[Na+] = _______M

[H3O+] = _____M

[OH-] = _______M

[C6H5CO2-] = ________ M

What is the pH of the solution at the equivalence point?

Ph= ______

****PLEASE ONLY ATTEMPT IF YOU KNOW THE ANSWER AS I'M DOWN TO MY LAST ATTEMPT*** THANKS!