Question

A. If the pH of a solution is 1.2, find [OH-]

B. Find the pH of a 0.058M solution of acetic acid (Ka= 1.8x10^-5)

C. Find the pH of a 0.02M solution of HF (Ka= 6.2x10^-4)

Answer #1

a. The hydroxide ion concentration of an aqueous solution of
0.538 M acetic acid is
[OH-] = ______ M.
b. Calculate the pH of a 0.538 M aqueous
solution of hydrofluoric acid
(HF, Ka =
7.2×10-4).

A.) Find the pH of a 0.338 M NaF solution. (The Ka of
hydrofluoric acid, HF, is 3.5×10?4.)
B.) Determine the [OH?] of a 0.30 M solution of NaHCO3. and
Determine the pH of this solution.
C.)Find the [OH?] of a 0.46 M methylamine
(CH3NH2) solution. (The value of Kb for methylamine
(CH3NH2) is 4.4×10?4.) include units
D.) Find the pH of a 0.46? M methylamine
(CH3NH2) solution.

A). Calculate [H3O+], [OH-], pH
and pOH for 0.035M solution of Ca(OH)2
B). Calculate the pH of a 0.028M solution of benzoic acid
Ka= 6.5 x 10-5

Calculate the pH of a solution that is 0.125M acetic acid and
0.150M sodium acetate. Calculate the pH if a 50.0mL of 0.150M
nitric acid is added to 275mL of the solution of acetic acid and
sodium acetate.
Ka=1.8x10-5

A.) Find the percent ionization of a 0.120 M solution of a weak
monoprotic acid having Ka= 1.2×10−3.
B.)Find the pH of a 0.120 M solution of a weak monoprotic acid
having Ka= 0.10.
C.) Find the percent ionization of a 0.120 M solution of a weak
monoprotic acid having Ka= 0.10.
D.) Find the pH of a 0.013 M solution of HF. (The value
of Ka for HF is 3.5×10−4.)

A.) What is the pH of a 500mL sample of 0.450M acetic acid
solution, given a Ka=1.8x10^-5?
B.) What is the pH after 20.000ml of 0.8M NaOH are added?
C.) What is the pH after 140.625mL of 0.8M NaOH are added?

5 acetic acid solutions, 0.10M, 0.50M,1.00M, 3.00M, 6.00M.
(PL5) Calculate pH for a solution which has [H+] = 0.765M.
(PL6) Calculate [H+] for a solution with pH=3.65
A1) Calculate percent dissociation of 5 solutions. Show your
work clearly for 0.10M solution.
(A2) Draw a graph of percent dissociation vs. concentration.
Label everything.
(Q1) What is the theoretical pH of 1.00M acetic acid (Ka =
1.8x10^-5)
(Q2) What is the theoretical percent dissociation for Q1?
(Q3) What is the theoretical pH...

-What concentration of ammonia is required to have a solution
with a pH of 11.36? Kb = 1.8x10-5
-What is the pH of a 0.014M solution of NaF? Ka for
HF = 6.8 x 10-4
-What is the other product of the aqueous base dissociation
reaction of ethyl amine?
C2H5NH2(aq) + H2O(l)
⇌ ________ + OH-(aq)

calculate the ph of a solution containing 0.15m acetic acid and
.25M sodium acetate for acetic acid ka=1.8x10^-5 if .0010 mol HCL
is added to 1.0 L buffer as in part a calculate the final ph of the
buffer. show work with ICE

1.Calculate the pH of an 0.0452 M Ba(OH)2 solution at 298 K
2. calculate the pH of an 0.229 M HNO2 solution at 298 K. Assume
ka for HNO2 is 4.5x10^-4
3.Calculate the pH of an 0.292 M NH3 solution at 298 K. assume
the Kb for NH3 is 1.8x10^-5

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