Assume you dissolve 0.120 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 x 10^2 mL of solution and then....?

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Assume you dissolve 0.120 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 x 10^2 mL of solution and then....?

Assume you dissolve 0.120 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 x 10^2 mL of solution and then titrate the solution with 0.195 M NaOH. (Ka for benzoic acid = 6.3 x10^-5)

C6H5CO2H + OH- = C6H5CO2- + H2O

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 point: Na+ , H3O+, OH- and C6H5CO2-?
* I really do not know how to solve for the Na+ concentration :/

c) what is the pH of the solution at the equivalence point?

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Assume you dissolve 0.120 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 x 10^2 mL of solution and then....?

Assume you dissolve 0.120 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 x 10^2 mL of solution and then....?

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