WorksheetsAP Chemistry PH and Buffers
Total questions: 10
Worksheet time: 8mins
Name
Class
Date
1.
Buffer is defined as
a)
ability to resist pH change
b)
ability to prevent pH from decreasing
c)
ability to resist a pH increase
d)
ability to resist pH change when small amount of acid added
2.
Acidic buffer is made up of
a)
weak acid and weak base
b)
weak acid and its conjugate salt
c)
weak acid and its conjugate base
d)
strong acid and its conjugate base
3.
Which solution A and B of equal volume and concentration mixed together to form a buffer?
a)
Nitric acid and potassium hydroxide
b)
Nitric acid and potassium nitrate
c)
Propanoic acid and potassium hydroxide
d)
Propanoic acid and potassium propanoate
4.
Which combination will form a buffer solution?
a)
100ml of 0.1M HCI with 50ml of 0.1M NaOH
b)
100ml of 0.1M CH3COOH with 50ml of 0.1M NaOH
c)
50ml of 0.1M HCI with 100ml of 0.1M NaOH
d)
50ml of 0.1M CH3COOH with 100ml of 0.1M NaOH
5.
When making a buffer of pH = 5, acids with the following Ka values are available. Which would be the best acid to use?
a)
1.8 x 10-5
b)
1.8 x 10-8
c)
4.9 x 10-10
d)
3.0 x 10-8
6.
Which pair is the most effective buffer?
Ka of HIO is 1.7 x 10-11
Ka of HF is 3.5 x 10-4
Ka of HIO is 1.7 x 10-11
Ka of HF is 3.5 x 10-4
a)
0.5 M HIO and 0.5 M NaIO
b)
0.1 M HF and 0.1 M NaF
c)
0.9 M HIO and 0.1 M NaIO
d)
0.1 M HF and 0.7 M NaF
7.
A buffer has a pH of 4.85 and contains formic acid and potassium formate. What can you conclude about the concentrations of the components of the buffer? The Ka of formic acid is 1.8 x 10-4.
a)
Formic acid > Potassium formate
b)
Formic acid < Potassium formate
c)
Formic acid = Potassium formate
d)
More information is needed to determine the relative concentrations
8.
What is the pH of a buffer that is 0.08 M NaA and 0.1 HA. The Ka of HA = 1.0 x 10-4.
a)
2.16
b)
3.91
c)
4.00
d)
4.10
9.
Suppose you have a solution of 0.3 M HBrO and 0.3 M BrO. You add a small amount of NaOH to this buffer solution. What is the reaction that takes place?
a)
H+ + BrO- --> HBrO
b)
OH- + H+ --> H2O
c)
OH- + HBrO --> H2O + BrO-
d)
OH- + BrO- --> O-2 + HBrO
10.
Suppose you have a solution of the strong acid HNO3 and the weak acid HNO2. As you add NaOH, the concentration of which of the following species increases?
a)
NO3-
b)
NO2-
c)
HNO2
d)
H+
100 %
