Question

a. Find the *p**H* of a 0.100 M solution of a weak
monoprotic acid having *K*a= 1.1×10^{−5}.

b.Find the percent dissociation of this solution.

c. Find the *p**H* of a 0.100 M solution of a weak
monoprotic acid having *K*a= 1.8×10^{−3}

^{d.} Find the percent
dissociation of this solution.

e.Find the
*p**H* of a 0.100 M solution of a weak monoprotic
acid having *K*a= 0.16.

f.Find the percent dissociation of this solution.

Answer #1

a )

C = 0.100 , Ka = 1.1 x 10^-5

[H+] = sqrt (Ka x C) = sqrt (1.1 x 10^-5 x 0.1) = 1.05 x 10^-3 M

pH = -log [H+] = -log (1.05 x 10^-3)

**pH = 2.98**

b) percent dissociation = [H+] x 100 / C = 1.05 x 10^-3 x 100 / 0.1

**percent dissociation** **= 1.05
%**

c)

HA ---------------------> H+ + A-

0.1-x x x ---------------> equilibrium

Ka = x^2 / 0.1-x

1.8 x 10^-3 = x^2 / 0.1-x

x^2 + 1.8 x 10^-3 x - 1.8 x 10^-4 = 0

x = 0.0125

[H+] = 0.0125 M

**pH = 1.90**

d)

percent dissocitation= ( x / C ) x 100

= (0.0125 / 0.1) x 100

= 12.5 %

**percent
dissocitation = 12.5 %**

e)

HA ---------------------> H+ + A-

0.1-x x x ---------------> equilibrium

Ka = x^2 / 0.1-x

0.16 = x^2 / 0.1-x

x^2 + 0.16 x - 0.016 = 0

x = 0.0697

[H+] = 0.0697M

**pH = 1.16**

f )

percent dissocitation= ( x / C ) x 100

= (0.0697 / 0.1) x 100

= 69.7 %

**percent dissocitation = 69.7 %**

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.)

Find the pH of a 0.140 M solution of a weak
monoprotic acid having Ka= 1.0×10−3.
Express your answer to two decimal places.
pH =
1.95
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Significant Figures Feedback: Your answer
1.93 was either rounded differently or used a different
number of significant figures than required for this part.
Part D
Find the percent dissociation of this solution.
Express your answer using two significant figures.
%
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Not...

1. The Ka of a monoprotic weak acid is 5.90 × 10-3. What is the
percent ionization of a 0.148 M solution of this acid?
2. If the Kb of a weak base is 4.5 × 10-6, what is the pH of a
0.26 M solution of this base?
3. Assuming complete dissociation, what is the pH of a 3.00 mg/L
Ba(OH)2 solution?

A 0.100 M solution of a monoprotic weak acid has a pH of 3.00.
Calculate the pKa

1.) If the Ka of a monoprotic
weak acid is 4.5 x 10^-6, what is the pH of a 0.30M solution of
this acid?
2.) The Ka of a monoprotic weak
acid is 7.93 x 10^-3. What is the percent ionization of a 0.170 M
solution of this acid?
3.) Enolugh of a monoprotic acid
is dissolved in water to produce a 0.0141 M solution. The pH of the
resulting solution is 2.50. Calculate the Ka for the
acid.

What is the percent ionization of a monoprotic weak acid
solution that is 0.186 M? The acid-dissociation (or ionization)
constant, Ka, of this acid is 2.43 × 10-12.

If the Ka of a monoprotic weak acid is 7.5 × 10-6, what is the
pH of a 0.12 M solution of this acid?

If the Ka of a monoprotic weak acid is 3.3 × 10-6, what is the
pH of a 0.30 M solution of this acid?

If the Ka of a monoprotic weak acid is 5.7 × 10-6, what is the
pH of a 0.14 M solution of this acid?

If the Ka of a monoprotic weak acid is 1.6 × 10-6, what is the
pH of a 0.12 M solution of this acid?

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