Homework 1:
1.
Name three properties of acids and three properties of bases.
Acids: dissolve metals to make H
+
, taste sour, conduct electricity.
Bases: taste salty, conduct, feel slippery
2.
What is an acid, according to the Arrhenius definition? Produces H
+
when dissolved in water.
3.
If a solution has more OH- than H+, is it acidic or basic? Basic Which pH might it have—2 or 12? 12
4.
What is an electrolyte? A substance that produces ions when it dissolves in water.
If pure water is not a good conductor of electricity, why are you supposed to get out of the water during an electrical storm?
Water lowers the resistance to electrical flow through human skin. Water does not significantly conduct electricity.
5.
What does it mean to say that water dissociates? That it produces ions: H
2
O H
6.
What is the hydronium ion? H
3
O
+
+
+ OH
-
What is it the same as? Chemically it is equivalent to H
+
7.
What is pH a measure of? H
+
ion concentration.
What is the formula for pH?
8.
How does a solution with a pH of 12 compare to a solution with a pH of 8 in terms of [H
3
O
+
+
]?
9.
Find the pH of the following solutions:
[H
3
O
+ b) [H
3
O
+ c) [H
3
O
+
] = 1.6 x 10
] = 3.7 x 10
] = 9.2 x 10
-6
-4
M
M
-13
M
10.
Find the [H
3
O
+
] of the following solutions: a) pH = 1.6 b) pH = 7.2 c) pH = 8.8
Homework 2:
5.81
3.43
12.03
.025
6.31x10
1.58x10
-8
-9
1. Find the pOH of the following solutions: a) [OH b) [OH
-
-
] = 9.4 x 10
-12
]= 4.1 x 10
-1
M
M
2. Find the [OH-] of the following solutions:
11.02
0.38
a) pOH = 1.4 b) pOH = 10.1
3. What is the [H
3
O
+
4. What is the [H
3
O
+
.039
7.94x10
-11
] of a solution with a pOH of 6? 1x10
-8
] of a solution with an [OH
-
] = 3.4 x 10
-9
M? 1.01x10
-11
5. What is the pH of a solution with an [OH
-
] = 9.1 x 10
-4
M? 10.96
6 What is the pOH of a solution with a pH of 4?
7. What is the pOH of a solution with a [H
3
O
+
] = 9.0 x 10
-2
?
10
12.95
8. How does the Bronsted-Lowry definition of a base differ from the Arrhenius definition? B-L bases accept
H
+
ions from acids; Arrhenius bases produce OH
-
when dissolved in water.
9. What is the conjugate base for each of the following? a) H b) H
2
2
SO
CO c) NH
3
4
3
HSO
HCO
NH
2
-
-
4
3
-
(or SO
(or CO
2d) HF F
-
4
3
-2
)
)
10. For each of the following reactions, indicate the acid, base, conjugate acid, and conjugate base. a) NH
3
+ H
3
O
+
NH b) CH
3
OH + NH
2
-
4
+
+ H
2
O
CH
3
O
-
+ NH
3 c) OH
-
+ H
3 d) NH
2
-
+ H
O
+
2
H
2
O NH
O + H
3
2
O
+ OH
-
B/A
A/B
B/A
B/A
A/B
B/A
A/B
A/B
Homework 3:
1. What is the difference between a strong acid and a weak acid? Strong acids completely dissociate; weak acids don’t.
2. Strong acids have ( high , low) K a
values.
3. Name two strong acids. Name two weak acids. Strong: HI, HBr, HCl, H
2
SO
4
, HClO
4
, HNO
3
. Weak: HF,
CH
3
COOH, any other carbon containing acid.

4. For each of the following acids, indicate if it is monoprotic or polyprotic. a) HCOO H monoprotic (the bold one is the acid proton) b) H
2
SeO
3 c) CH
3
COO H d) H
3
BO
3 e) H
2
CO
3 f) H Br polyprotic monoprotic polyprotic monoprotic monoprotic
5. What volume of 0.196 M LiOH is required to neutralize 25.0 ml of 0.413 M HBr? (0.196)(V
B
V
B
= 52.7 mL
) = (25.0)(0.413);
6. What is the concentration of a solution of NaOH if 21.2 ml of a 0.0800 M solution of HCl are needed to neutralize 25.0 ml of the base? (21.2 mL)(M
B
) = (25.0 mL)(0.0800 M); M
B
= .0943 M
7. If 86.2 ml of 0.765 M sodium hydroxide neutralizes 50.0 ml of hydrochloric acid, what is the concentration of the acid? (0.765 M)(86.2 mL) = (50.0 mL)(M
A
); M
A
= 1.32 M
8. Calculate the [OH-] for lemon juice, pH = 2.3, and baking soda solution, pH = 8.5.
Lemon Juice: 2.00x10
-12
M
Baking soda: 3.16x10
-6
M