Question

Find the H3O+ concentration of a 0.210 M hypochlorous acid solution (whose acid dissociation constant is Ka=2.9×10−8).

Answer #1

hypochlorous acid dissociated as

HClO + H_{2}O
H_{3}O^{+} + OCl^{-}

it is monoprotic acid therefore [ H_{3}O^{+} ] =
[OCl^{-}]

Ka = [ H_{3}O^{+} ] [OCl^{-}] /
[HClO]

consider [ H_{3}O^{+} ] = [OCl^{-}] =
X

then above equation become

Ka = X^{2} / [HClO]

substitute value

2.9 10^{-8}
= X^{2} / 0.210

X^{2} = 2.9
10^{-8} 0.210

X^{2} = 6.09
10^{-9}

X = 7.8 10^{-5}
= [ H_{3}O^{+} ] = [OCl^{-}]

concentration of H_{3}O^{+} = 7.8
10^{-5}
M

Find the H3O+H3O+ concentration of a 0.220
MM hypochlorous acid solution (whose acid dissociation
constant is Ka=2.9×10−8Ka=2.9×10−8).
Express the concentration to two significant figures.

The acid-dissociation constant for hypochlorous acid (HClO) is
3.0×10−8.
Part A
Calculate the concentration of H3O+ at equilibrium if the
initial concentration of HClO is 8.6×10−3 M .
Express your answer using two significant figures.
[H3O+] =
M
SubmitMy AnswersGive
Up
Part B
Calculate the concentration of ClO− at equilibrium if the
initial concentration of HClO is 8.6×10−3 M .
Express your answer using two significant figures.
[ClO−] =
M
SubmitMy AnswersGive
Up
Part C
Calculate the concentration of HClO...

Find the dissociation constant (ka) of a 0.04 M weak
acid HX whose pH is 4.8

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...

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...

What is the equilibrium pH of an initially 4.4 M solution of
hypochlorous acid, HOCl, at 25°C (Ka = )? What is Ka for a weak
monoprotic acid if a 0.020 M solution of the acid has a pH of 3.28
at 25°C? 15.0 mL of 0.50 M HCl is added to a 100.0-mL sample of
0.484 M HNO2 (Ka for HNO2 = 4.0 × 10–4). What is the equilibrium
concentration of NO2– ions?

A solution of a weak acid HA has initial concentration c and
acid ionization constant Ka. To what concentration should the acid
be diluted to make [H3O+] half of what it was? Answer in terms of c
and Ka.

a) If acetic acid is the only acid that vinegar contains
(Ka=1.8×10−5), calculate the concentration of
acetic acid in the vinegar. A particular sample of vinegar has a pH
of 2.95.
b) The acid-dissociation constant for benzoic acid (C6H5COOH) is
6.3×10−5. Calculate the equilibrium concentration of H3O+ in the
solution if the initial concentration of C6H5COOH is
6.2×10−2 M .
c) Calculate the equilibrium concentration of C6H5COO− in the
solution if the initial concentration of C6H5COOH is
6.2×10−2 M ....

To a 1.00 L buffer solution made of 1.95 M hypochlorous acid
(HClO) and 1.03 M potassium hypochlorite (KClO) was added 0.509
moles of NaOH (assume no volume change to the solution).
What is the final pH of this buffer assuming Ka
hypochlorous acid = 2.90e-8?

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 11 minutes ago

asked 12 minutes ago

asked 21 minutes ago

asked 24 minutes ago

asked 30 minutes ago

asked 36 minutes ago

asked 42 minutes ago

asked 46 minutes ago

asked 46 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago