Question

Trichloroacetic acid, CCl_{3}COOH, has an acid
dissociation constant of 2.0 × 10^{-1} at 25 °C. Calculate
the pH of a 0.0420 M trichloroacetic acid solution.

pH = _____

Answer #1

A weak acid has a dissociation constant of 3.0 x 10-5. Calculate
the pH of a 2.90 M solution of this acid.
Q 13

The acid-dissociation constant of hydrocyanic acid (HCN) at
25.0°C is 4.9 × 10-10. What is the pH of an aqueous
solution of 0.030 M sodium cyanide (NaCN)?

Trichloroacetic acid is sometimes used in the treatment of
warts. Calculate the pH of a 3.0 M solution of trichloroacetic
acid. (ka = 2.0 x 10^-1)

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...

Hydrofluoric acid, HF, is a weak acid with an acid-dissociation
constant (Ka) of 6.3 ✕ 10−4. If
0.023 L of 0.17 M HF is titrated with 0.16 M
NaOH, a strong base, determine the pH at the equivalence point.
(The ion-product constant of water isKw = 1.01
✕ 10−14 at 25°C.)

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...

A diprotic acid, H2A, has acid dissociation constants of Ka1 =
3.48× 10–4 and Ka2 = 3.21× 10–12. Calculate the pH and molar
concentrations of H2A, HA–, and A2– at equilibrium for each of the
solutions below.(a) a 0.153 M solution of H2A.(b) a 0.153 M
solution of NaHA.(c) a 0.153 M solution of Na2A

The acid-dissociation constant for benzoic acid ( C 6 H 5 COOH)
is 6.3× 10 −5 .
Part A Calculate the equilibrium concentration of H3O+ in the
solution if the initial concentration of C6H5COOH is 5.7×10−2 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 5.7×10−2 M
. Express your answer using two significant figures.
Part C Calculate the equilibrium concentration of...

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...

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