CHEM 1412 – Home-work 4
1.
2.
3.
In the reaction H2CO3 + H2O
A.
H2CO3 and H2O.
B.
HCO3- and H2CO3.
C.
H2O and H3O+.
D.
H3O+ and H2CO3.
E.
H2O and HCO3-.
In the reaction HSO4-(aq) + OH-(aq)
A.
Row 1
B.
Row 2
C.
Row 3
D.
Row 4
E.
Row 5
HCO3- + H3O+, the Brønsted acids are
SO42-(aq) + H2O(l), the conjugate acid-base pairs are
The OH- concentration in a 7.5  10-3 M Ca(OH)2 solution is
A.
7.5  10-3 M.
B.
1.5  10-2 M.
C.
1.3  10-12 M.
D.
1.0  10-7 M.
E.
1.0  10-14 M.
4.
5.
6.
7.
8.
What is the H+ ion concentration in a 4.8  10-2 M KOH solution?
A.
4.8  10-2 M
B.
1.0  10-7 M
C.
4.8  10-11 M
D.
4.8  10-12 M
E.
2.1  10-13 M
Calculate the H+ ion concentration in a 8.8  10-4 M Ca(OH)2 solution.
A.
8.8  10-4 M
B.
1.8  10-3 M
C.
2.2  10-11 M
D.
1.1  10-11 M
E.
5.7  10-12 M
A 0.14 M HNO2 solution is 5.7% ionized. Calculate the H+ ion concentration.
A.
8.0  10-3 M
B.
0.057 M
C.
0.13 M
D.
0.14 M
E.
0.80 M
Calculate the pH of a beer in which the hydrogen ion concentration is 6.3  10-5 M.
A.
4.2
B.
4.8
C.
5.63
D.
9.8
E.
14.0
Calculate the H+ ion concentration in lemon juice having a pH of 2.4.
A.
4.0  10-2 M
9.
10.
11.
12.
B.
250 M
C.
0.38 M
D.
4.0  10-3 M
E.
12 M
Calculate the pH of 2.6  10-2 M KOH.
A.
12.41
B.
15.59
C.
2.06
D.
7.00
E.
1.59
Diet cola drinks have a pH of about 3.0, while milk has a pH of about 7.0. How many times greater
is the H3O+ concentration in diet cola than in milk?
A.
2.3 times higher in diet cola than in milk
B.
400 times higher in diet cola than in milk
C.
0.43 times higher in diet cola than in milk
D.
1,000 times higher in diet cola than in milk
E.
10,000 times higher in diet cola than in milk
Acid strength decreases in the series HI > HSO4- > HF > HCN. Which of these anions is the weakest
base?
A.
I-
B.
SO42-
C.
F-
D.
CN-
Arrange the acids HOCl, HClO3, and HClO2 in order of increasing acid strength.
A.
HOCl < HClO3 < HClO2
B.
HOCl < HClO2 < HClO3
C.
HClO2 < HOCl < HClO3
13.
14.
15.
D.
HClO3 < HOCl < HClO2
E.
HClO3 < HClO2 < HOCl
Arrange the acids HBr, H2Se, and H3As in order of increasing acid strength.
A.
HBr < H2Se < H3As
B.
HBr < H3As < H2Se
C.
H2Se < H3As < HBr
D.
H3As< H2Se < HBr
E.
H3As< HBr < H2Se
Arrange the acids H2Se, H2Te, and H2S in order of increasing acid strength.
A.
H2S < H2Se < H2Te
B.
H2S < H2Te < H2Se
C.
H2Te < H2S < H2Se
D.
H2Se< H2S < H2Te
E.
H2Se< H2Te < H2S
Predict the direction in which the equilibrium will lie for the reaction
H2SO3(aq) + HCO3- (aq)
HSO3-(aq) + H2CO3(aq).
Ka1(H2SO3) = 1  10-2; Ka1(H2CO3) = 4.2  10-7
16.
A.
to the right
B.
to the left
C.
in the middle
P4O10 is classified as an acidic oxide because it
A.
reacts with acids to produce a salt.
B.
is insoluble in water.
C.
reacts with water to produce OH-.
D.
gives a solution of phosphoric acid, H3PO4, on dissolving in water.
E.
can act as a Lewis base by donating electron pairs.
17.
18.
20.
An aqueous solution of KCl would be
A.
neutral.
B.
basic.
C.
acidic.
Which one of these salts will form a basic solution upon dissolving in water?
A.
NaCl
B.
NaNO2
C.
NH4NO3
D.
KBr
E.
AlCl3
Identify the conjugate acid-base pairs in the reaction
HSO4- + HF ↔ H2SO4 + F-
One conjugate acid-base pair is _______________; the other acid-base pair is ______________.