Question

Calculate the **percent ionization** of a
**0.484** M solution of **benzoic
acid****,
C _{6}H_{5}COOH**.

Answer #1

C6H5COOH <=> C6H5COO- + H+

start

0.484
0
0

change

-x .. . . . . . . .. . .. . . +x. . . . ..+x

at equilibrium

0.210-x. . . . . . .. . . .x .. . . . . . x

Ka = [C6H5COO-][H+]/ [C6H5COOH]= (x^2/
0.484-x
5.3 x 10^-5
=x^2/0.484
(if x is small 0.484-x= 0.484)

x = 0.0056 M

% ionization = 0.0056 x 100/ 0.484=1.04 %

The acid ionization constant Ka of benzoic acid (C6H5COOH; HA)
is 6.5 ⨯ 10-5.
(1) Calculate the pH of 2.0L of 0.20 M benzoic acid solution.
(2) After adding 8.0 g of NaOH (molar mass: 40 g/mol) to 2.0 L of a
0.20 M benzoic acid solution,
Calculate the pH.
(3) The solution (2) made above is a buffer solution. 2.0 L of 0.1
M NaOH aqueous solution was added to this solution.
After adding more, calculate the pH of...

４０．2.20 L of a buffer solution that is 0.190 M in benzoic acid,
C6H5COOH, and 0.340 M in sodium benzoate, C6H5CONa, are diluted to
4.40 L with distilled water. What is the pH of the buffer? Ka of
C6H5COOH = 6.4 ✕ 10-5.

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...

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 pKa of benzoic acid (C6H5COOH) is 4.19. This means that
A. in a solution at pH = 7.0, benzoic acid would be nearly or
completely protonated.
B. in a solution at pH = 7.0, benzoic acid would be nearly or
completely deprotonated.
C. in a solution at pH = 4.19, benzoic acid would be 1/2
deprotonated (1/2 benzoic acid and 1/2 benzoate).
A and C
B and C

1. Calculate the percent ionization of propionic acid (C2H5COOH)
in solutions of each of the following concentrations.
Part A 2.06×10−2 M .
2. Calculate the pH at the equivalence point in titrating 0.100
M solutions of each of the following with 8.0×10−2 MNaOH.
Part A hydrobromic acid (HBr)
Part B chlorous acid (HClO2)
Part C benzoic acid (C6H5COOH)

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 6.6×10−2 M
.
Express your answer using two significant figures.
[H3O+] =
M
SubmitRequest Answer
Part B
Calculate the equilibrium concentration of C6H5COO− in the
solution if the initial concentration of C6H5COOH is
6.6×10−2 M .
Express your answer using two significant figures.
[C6H5COO−] =
M
SubmitRequest Answer
Part C
Calculate the equilibrium...

A buffer solution is prepared by mixing 20.0mL of 0.032M benzoic
acid C6H5COOH soultion with 25.0mL of 0.022 M NaC6H5COO. what is
the pH of the buffer produced? (Ka of benzoic acid = 6.2*10^-5)

(a) Calculate the percent ionization of 0.00250 M acetic acid
(Ka = 1.8e-05).
% ionization = %
(b) Calculate the percent ionization of 0.00250 M acetic acid in
a solution containing 0.0110 M sodium acetate.
% ionization = %

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