Dougherty Valley HS Chemistry
pH and pOH
Name:
Date:
Period:
1. What is pH a measure of? ______________________________________________
2. What is the equation used for finding pH? __________________________________
3. What is the equation that relates to pH and pOH? ____________________________
4. Complete the following table: (first one is done as an example)
a.
[H+] M
[OH-] M
pH
pOH
1.0 x 10-3
1.0 x 10-11
3
11
1.0 x 10-5
b.
c.
10.00
d.
e.
6.00
0.010
f.
0.0000010
g.
4.00
h.
i.
7.00
3.2 x 10-3
1.8 x 10-14
j.
k.
10.23
l.
m.
Acidic, base,
neutral
Acidic
6.78
0.0050
n.
0.000011
o.
10.97
p.
7.01
5. What would be the pH of each of the following?
a) 0.0010 M HCl ____
b) 0.0010 M HNO3 ____
c) 0.010 M NaOH ____
d) 0.0035 M HCl ____
g) 0.024 M HCl ____
h) 0.075 M KOH ____
i) 0.000034 M HCl ____
j) 0.000000000001M HCl ____
6. Classify each of the following as acidic, neutral, or basic:
a) Tomatoes-4.2 ______________
c) Eggs-7.8 ______________
b) soil-5.5 ______________
d) milk-6.4 ____________
e) ammonia-11.0 _______
Dougherty Valley HS Chemistry
pH Calculations
Find the pH of the following acidic solutions: Show work to receive full credit. Put a box around your final answer. Round
ALL final numerical answers to 2 decimal places
1)
A 0.001 M solution of HCl (hydrochloric acid). 3.00
2)
A 0.09 M solution of HBr (hydrobromic acid). 1.05
3)
A 1.34 x 10-4 M solution of hydrochloric acid. 3.87
4)
A 2.234 x 10-6 M solution of HI (hydroiodic acid). 5.65
5)
A 7.98 x 10-2 M solution of HNO3 (nitric acid). 1.10
6)
A solution containing 1 mole of hydrochloric acid in 12 L of water. 1.08
7)
A solution containing 0.34 moles of nitric acid in 735 L of water. 3.33
8)
A solution containing 8.543 moles of hydrobromic acid in 1098 L of water. 2.11
9)
A solution containing .0074 moles of hydrochloric acid in 660 L of water. 4.95
10)
A solution containing 0.005 grams of hydrochloric acid in 120 mL of water. 2.94
11)
A solution containing 5.0 x 10-4 grams of hydrobromic acid in 1.2 liters of water. 5.28
12)
A solution containing 4.5 grams of nitric acid in 2.3 liters of water. 1.51
13)
A solution containing 0.344 grams of hydrochloric acid in 792 mL of water. 1.92
14)
A solution containing 1.00 grams of nitric acid in 100 mL of water. 0.80
15)
A solution containing 1.1 grams of nitric acid in 8.7 liters of water. 2.70
16)
A solution containing 5.6 grams of hydroiodic acid in 1.5 liters of water. 1.53
17)
A solution containing 0.01 grams of hydrochloric acid in 10.7 liters of water. 4.59
18)
A solution containing 6.7 grams of nitric acid and 4.5 grams of hydrochloric acid in 8,000 mL of water.
1.54
19)
A solution containing 45 grams of nitric acid and 998 grams of hydrobromic acid in 150,000 L of water.
4.06
20)
A solution containing 0.09 grams of HCl, 0.9 grams of HBr, 9.0 grams of HI, and 90.0 grams of HNO3 in
fifty liters of water. 1.52
Dougherty Valley HS Chemistry
pH practice
Answer the following question regarding pH. Must show all work to receive full credit. Put a box
around your final answer. Round all answers to two decimal places.
1)
What is the pH and pOH of a 1.2 x 10-3 HBr solution? pH: 2.9
2)
What is the pH and pOH of a 2.34 x 10-5 NaOH solution? pOH: 4.6
3)
What is the pH and pOH of a solution made by adding water to 15 grams of hydroiodic acid
until the volume of the solution is 2500 mL? pH: 1.6
pOH: 12.4
4)
What is the pH and pOH of a solution that was made by adding 400 mL of water to 350 mL of
5.0 x 10-3 M NaOH solution? pOH: 2.7
pH: 11.3
5)
What is the pH and pOH of a solution with a volume of 5.4 L that contains 15 grams of
hydrochloric acid and 25 grams of nitric acid? pH: 0.82
pOH: 13.18
6)
A swimming pool has a volume of one million liters. How many grams of HCl would need to be
added to that swimming pool to bring the pH down from 7 to 4? (Assume the volume of the
HCl is negligible) 3545 grams (100.0 moles)
pOH: 11.1
pH: 9.4
Dougherty Valley HS Chemistry
pH Review Problems
Show work to receive full credit. Put a box around your final answer. Round ALL numerical answers
to 2 decimal places
1)
What is the molarity of a solution that has 450 grams of sodium chloride in 800 mL of water?
9.61 M
2)
What is the molarity of a solution that contains 100 grams of iron (II) nitrate in 2.4 liters of
water? 0.23 M
3)
What is the pH of a solution that contains 2.4 x 10-5 moles of hydrobromic acid in 0.5 L of
water? 4.32
4)
What is the pH of a solution that contains 25 moles of nitric acid dissolved in 5000 liters of
water? 2.30
5)
What is the pH of a solution that contains 0.009 grams of hydrochloric acid in 100 mL of water?
2.61
6)
What is an acid/base indicator used for?
7)
Define “titration”:
8)
In a few steps, describe how you would titrate a base of unknown concentration with an acid
with concentration 1 M.
9)
I did a titration where it took 50 mL of 0.10 M hydrochloric acid to neutralize 500 mL of a base
with unknown concentration. Using this titration information, what was the concentration of the
base? 0.01 M
10)
I did a titration where it took 25.0 mL of 5 M NaOH to neutralize 1000 mL of an acid with
unknown concentration. Using this information, what was the concentration of the acid? 0.125
M