Assume you dissolve 0.235 g of the weak acid benzoic acid,C6H5CO2H, in enough water to make 9.00 102 mL of solution and thentitrate the solution with 0.128 M NaOH.

C6H5CO2H(aq) + OH-(aq) -> C6H5CO2-(aq) + H2O(l lookingthink)

What are the concentrations of the following ions at theequivalence point?
Na+, H3O+, OH-
C6H5CO2-

_ M Na+
_ M H3O+
_ M OH-
_ M C6H5CO2-

What is the pH of the solution? ___

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Collen VonLv2

28 Sep 2019

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24. Assume you dissolve .235g of the weak acid benzoic acid,C6H5CO2H, in enough water to make 1.00 x 10^2 mL of solution andthen titrate the solution with .108M of NaOH
Chemical Reaction: C6H5CO2H + OH (double arows) C6H5CO2-- +H20
A) What was the pH of the original benzoic acid solution?
B) What are the concentrations fo all of the following ions at theequivalence point: Na+, H30+, OH-, and C6H5CO2--?
C) What is the pH of the solution at he equivalence point?
This problem confused everyone in my class, mostly because wedidn't learn about equivalence point problems yet, I really needsome guidance in the procedure of this problem. Thankyou

Benzoic acid C6H5COOH is a weak acid with Ka=6.3 X 10^-5
C6H5CO2H(aq) + H2O(l)<---> H3O^+(aq) + C6H5CO2^-(aq)

a) Calculate the pH of a 0.150 M benzoic acid solution. Show allcalulations.

b) Suppose 1.44g of sodium benzoate, Na^+C6H5COO-, is added to100.0 mL of the 0.150 M benzioic acid solution. Calculate the pH ofthe resulting buffer solution assuming the volume of the solutiondoes not change on addition of the solid.