Chem 051 - Fundamentals of Chemistry » Winter 2021 » Homework GOB Week 4
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Question #1
The mass percent concentration refers to
A.
grams of solute in 1 kg of solution.
B.
grams of solute in 100 g of solvent.
C.
grams of solute in 1 kg of solvent.
D.
grams of solvent in 100 g of solution.
E.
grams of solute in 100 g of solution.
Question #2
In a solution, the solvent
A.
can be a solid, liquid, or gas.
B.
is a liquid.
C.
is the substance present in the smallest concentration.
D.
can be a liquid or gas.
E.
is never a solid.
Question #3
The molarity (M) of a solution refers to
A.
moles of solute/L of solution.
B.
moles of solute/ L of solvent.
C.
grams of solute/100 mL of solution.
D.
grams of solute/L of solution.
E.
moles of solute/100 mL of solution.
Question #4
What is the molarity of a solution which contains 58.5 g of sodium chloride dissolved in 0.500 L of solution?
A.
1.50 M
B.
2.00 M
C.
4.00 M
D.
1.00 M
E.
0.500 M
Question #5
What volume of 0.10 M NaOH can be prepared from 250. mL of 0.30 M NaOH?
A.
0.75 L
B.
0.075 L
C.
750 L
D.
0.25 L
E.
0.083 L
Question #6
What mass of KCl is in 350 mL of 0.24 M KCl?
A.
84 g
B.
18 g
C.
6.3 g
D.
1.1.g
E.
0.84 g
Question #7
In water, a substance that ionizes completely in solution is called a
A.
strong electrolyte.
B.
nonelectrolyte.
C.
nonconductor.
D.
semiconductor.
E.
weak electrolyte.
Question #8
For Kw, the product of [H3O+] and [OH-] is
A.
1.0 X 10-14
B.
1.0 X 10-1
C.
1.0 X 10-7
D.
1.0
E.
1.0 X 1014
Question #9
What is the [H3O+] in a solution with [OH-] = 1 x 10-12 M?
A.
1 x 10-8 M
B.
1 x 102 M
C.
1 x 10-2 M
D.
1 x 10-7 M
E.
1 x 10-12 M
Question #10
What is the [OH-] in a solution that has a [H3O+] = 1 x 10-6 M?
A.
1 x 10-10 M
B.
1 x 10-8 M
C.
1 x 10-2 M
D.
1 x 10-12 M
E.
1 x 10-6 M
Question #11
What is the pH of a solution with [OH-] = 1 x 10-4 M?
A.
1.0 x 10-10
B.
-10.0
C.
4.0
D.
10.0
E.
-4.0
Question #12
The [H3O+] of a solution with pH = 2.0 is
A.
-10 M.
B.
1 x 10-2 M.
C.
1 x 10-12 M.
D.
1 x 102 M.
E.
10 M.
Question #13
The [H3O+] of a solution with pH = 8.7 is
A.
8.7 M.
B.
5.3 M.
C.
8.7 x 10-1 M.
D.
5 x 10-6 M.
E.
2 x 10-9 M.
Question #14
Which of the following is the strongest acid?
A.
NH4+
B.
H2CO3
C.
HCl
D.
NaOH
E.
H3PO4
Question #15
The name given to an aqueous solution of HBr is
A.
bromic acid.
B.
hydrogen bromide.
C.
hydrobromic acid.
D.
hypobromous acid.
E.
bromous acid.
Question #16
A solution with [ OH-] of 5 x 10-3 has a pH of ________.
A.
2.3
B.
7.0
C.
-2.3
D.
11.7
E.
5.0
Question #17
Ammonium hydroxide is a weak base because
A.
is a poor acceptor of protons.
B.
it is only slightly soluble in water.
C.
it dissociates only slightly in water.
D.
it is a dilute solution.
E.
it is completely ionized in aqueous solution.
Question #18
An acid and base react to form a salt and water in a(n) ________ reaction.
A.
reduction
B.
neutralization
C.
oxidation
D.
ionization
E.
dissociation
Question #19
In a neutralization reaction
A.
an acid and a salt react to form water and a base.
B.
two acids react to form water.
C.
water and a salt react to form an acid and a base.
D.
a base and a salt react to form water and an acid.
E.
an acid and a base react to form a salt and water.
Question #20
Which of the following is the correctly balanced equation for the complete neutralization of H3PO4 by Ca(OH)2?
A.
2H3PO4 + 3Ca(OH)2 → Ca3(PO4)2 + 6H2O
B.
4H3PO4 + 6Ca(OH)2 → 2Ca3(PO4)2 + 12H2O
C.
H3PO4 + Ca(OH)2 → Ca3(PO4)2 + H2O
D.
H3PO4 + Ca(OH)2 → CaHPO4 + 2H2O
E.
3H3PO4 + Ca(OH)2 → Ca3(PO4)2 + 5H2O
Question #21
The neutralization reaction between Al(OH)3 and HNO3 produces the salt with the formula
A.
H2O.
B.
NO3OH.
C.
Al(NO3)3.
D.
AlNO3.
Question #22
Which of the following is a neutralization reaction?
A.
HNO3 + KOH → H2O + KNO3
B.
KCl + NaNO3 → KNO3 + NaCl
C.
H2O + SO3 → H2SO4
D.
2NO2 → 2NO + O2
Question #23
25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is
A.
0.137 M.
B.
0.212 M.
C.
0.500 M.
D.
0.390 M.
E.
0.115 M.
Question #24
According to the Bronsted-Lowry definition,
A.
an acid acts as the solvent.
B.
a base produces H+ ions in aqueous solutions.
C.
a base is a proton acceptor.
D.
an acid is a proton acceptor.
E.
a base is a proton donor.
Question #25
If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in the condition termed acidosis.
A.
FALSE
B.
TRUE
Question #26
An acidic solution has a pH less than 7.0.
A.
FALSE
B.
TRUE
Question #27
A solution with a pH greater than 7 is basic.
A.
TRUE
B.
FALSE
Question #28
In any water solution, [H3O+] [OH-] = 1.0 x 10-7.
A.
TRUE
B.
FALSE
Question #29
An aqueous solution with [OH-] = 1.0 x 10-12 has a pH of 12.0.
A.
TRUE
B.
FALSE
Question #30
For many reactions of acids with bases, the resulting products are a salt and water.
A.
TRUE
B.
FALSE
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