Question

You titrate 50.0 mL of 0.100 M benzoic acid (C6H5COOH) with 0.250 M KOH. What is the concentration of C6H5COO- at the equivalence point? The answer is: [C6H5COO-] = 7.14 x 10-2 M., but I'm not sure why?

What is the pH of the final solution at the equivalence point? Ka of C6H5COOH = 6.3 x 10-5.

Answer #1

Consider the titration of a 45.0 mL sample of 0.100 M HN3 with
0.250 M KOH. (Ka of HN3 = 2.5 x 10-5) Calculate each of the
following: (a) How many mL are required to reach the equivalence
point?
(b) What is the initial pH of the acid solution?
(c) What is the pH after the addition of 5.00 mL of KOH?
(d) What is the pH after the addition of 9.00 mL of KOH? (e)
What is the pH...

Starting with 0.250L of a buffer solution containing 0.250 M
benzoic acid (C6H5COOH) and 0.20 M sodium benzoate (C6H5COONa),
what will the pH of the solution be after the addition of 25.0 mL
of 0.100M HCl? (Ka (C6H5COOH) = 6.5 x 10-5)
Please solve in detail

The acid-dissociation constant for benzoic acid (C6H5COOH) is
6.3×10−5.
Part A Calculate the equilibrium concentration of H3O+ in the
solution if the initial concentration of C6H5COOH is 6.3×10−2 M .
Express your answer using two significant figures.
Part B Calculate the equilibrium concentration of C6H5COO− in
the solution if the initial concentration of C6H5COOH is 6.3×10−2 M
.
Part C Calculate the equilibrium concentration of C6H5COOH in
the solution if the initial concentration of C6H5COOH is 6.3×10−2 M
. Express...

The acid-dissociation constant for benzoic acid (C6H5COOH) is
6.3×10−5. Part A Calculate the equilibrium concentration of H3O+ in
the solution if the initial concentration of C6H5COOH is 6.3×10−2 M
. Express your answer using two significant figures. Part B
Calculate the equilibrium concentration of C6H5COO− in the solution
if the initial concentration of C6H5COOH is 6.3×10−2 M . Part C
Calculate the equilibrium concentration of C6H5COOH in the solution
if the initial concentration of C6H5COOH is 6.3×10−2 M . Express...

Determine the pH during the titration of 74.5
mL of 0.345 M benzoic acid
(Ka = 6.3×10-5) by
0.345 M KOH at the following
points.
(a) Before the addition of any KOH
(b) After the addition of 17.0 mL of
KOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 112 mL of
KOH

You titrated 100.00 mL of a 0.025 M solution of benzoic acid
(HBz) with 0.100 M NaOH to the equivalence point. Ka = 6.2x10-5

You are given a 30.0mL sample of 0.20M C6H5COOH(aq) (benzoic
acid). Ka for benzoic acid is 6.5x10-5.
b) what is the pH after the addition of 15.0mL of 0.30M
KOH(aq)?
c)if you start with a new 30.0mL sample of 0.20M C6H5COOH(aq),
what volume of 0.20M NaOH(aq) is required to reach the halfway to
the equivalence point?

An 80.9 mL sample of a 0.100 M solution of a diprotic acid, H2A,
is titrated with 0.100 M KOH. For H2A, Ka1 = 8.09 x 10^-5 and Ka2 =
8.09 x 10^-10. A) Calculate the concentration of A2- prior to the
addition of any KOH. B) What is the pH of the initial solution? C)
What is the pH exactly halfway to the first equivalence point? D)
What is the pH exactly halfway between the first and second
equivalence...

Suppose 25.00 mL of 0.250 M benzoic acid are titrated with 0.200
M NaOH. What is the pH at the equivalence point?

Consider a mixture of 50.0 mL of 0.100 M HCl and 50.0 mL of
0.100 M acetic acid. Acetic acid has a Ka of 1.8 x 10-5.
a. Calculate the pH of both solutions before mixing.
b. Construct an ICE table representative of this mixture.
c. Determine the approximate pH of the solution.
d. Determine the percent ionization of the acetic acid in this
mixture

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