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Assume you dissolve 0.253 g of the weak acid, benzoic acid (C6H5COOH) (HOBz), in enough water to make 100. mL, and then titrate the solution with 0.124 M NaOH(a) What was the original pH of the benzoic acid solution? (b) At the equivalence point what are the concentrations of [Na+] M ..... [OH-] M ..... [H+] ..... [BzO-] M(c) What is the pH at the equivalence point?

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Jean KeelingLv2
28 Sep 2019
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Related questions


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!!

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!

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