Problems B
347
4. Calculate the pOH for each of the solutions in Problem 1.
5. Calculate the pH of a solution made by dissolving 1.00 g of KOH in 250 ml of
distilled water.
6. Calculate the pH of a solution made by diluting 25.0 ml of commercial concentrated HBr solution (48.0% by weight, and density = 1.49 g/ml) to 2.00 liters.
7. A student pipets 50.0 ml of 0.1000 M HC1 into a flask and then adds increments
of 0.1000 M NaOH solution from a buret. Calculate the pH after the addition
of each of the following volumes of NaOH solution.
(a) 0.00 ml
^
(f) 49.9 ml
(b) 10.0 ml
'
(g) 50.0 ml
(c) 25.0 ml
(h) 50.1 ml
(d) 45.0 ml
(i) 51.0 ml
(e) 49.0 ml
G) 55.0 ml
Plot the results, showing pH on they axis and volume of NaOH added on the AT
axis. This graph is called a titration curve.
PROBLEMS B
8. Calculate the pH of solutions with the following H
+ concentrations (in moles/
liter).
(a) 1C3
(f) 7.6 x 10~»
(b) 10~
5
(g) 4.3 x 10B
(c) 109
(h) 8.3 x 10-"
(d) 0.0056
(i) 5.6
(e) 10
G) 0.35
9. Calculate the pH of solutions with the following OH~ concentrations (in
moles/liter).
(a) 102
(f) 8.5 x 1Q3
(b) 10-"
(g) 1.67 x 10-"
(c) 10-'°
(h) 4.73 x 10-'°
(d) 10
(i) 7.65
(e) 0.077
G) 0.22
10. Calculate the H
+ concentration for each of the solutions with the following
values for pH.
(a) 6.35
(f) 7.32
(b) 2.78
(g) 15.21
(c) 12.91
(h) 0.76
(d) 0.55
(i) 0
(e) 10.47
0) -0.36
11. Calculate the pOH for each of the solutions in Problem 8.
12. Calculate the pH of a solution made by dissolving 20.0 g of sulfamic acid,
H(NH 2 )SO 3 , and diluting to 200 ml with water. (Sulfamic acid is a strong acid,
like HC1.)