A 20.0-g sample of HF is dissolved in water to give 2.0 ´ 102 mL of solution. The concentration of the solution is:
A.
1.0 M
B.
3.0 M
C.
0.10 M
D.
5.0 M
E.
10.0 M
2.
How many grams of NaCl are contained in 350. mL of a 0.250 M solution of sodium chloride?
A.
41.7 g
B.
5.11 g
C.
14.6 g
D.
87.5 g
E.
none of these
3.
Which of the following aqueous solutions contains the greatest number of ions?
A.
400.0 mL of 0.10 M NaCl
B.
300.0 mL of 0.10 M CaCl2
C.
200.0 mL of 0.10 M FeCl3
D.
200.0 mL of 0.10 M KBr
E.
800.0 mL of 0.10 M sucrose
4.
What mass of solute is contained in 256 mL of a 0.895 M ammonium chloride solution?
A.
12.3 g
B.
13.7 g
C.
47.9 g
D.
53.5 g
E.
none of these
5.
A 51.24-g sample of Ba(OH)2 is dissolved in enough water to make 1.20 liters of solution. How many mL of this solution must be diluted with water in order to make 1.00 liter of 0.100 molar Ba(OH)2?
A.
400. mL
B.
333 mL
C.
278 mL
D.
1.20 ´ 103 mL
E.
none of these
6.
What volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H2SO4?
A.
168 mL
B.
0.336 L
C.
92.3 mL
D.
226 mL
E.
none of these
7.
The net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species?
A.
3Al3+(aq)
B.
OH–(aq)
C.
3OH–(aq)
D.
2Al3+(aq)
E.
2Al(OH)3(s)
8.
The net ionic equation for the reaction of calcium bromide and sodium phosphate contains which of the following species?
A.
Ca2+(aq)
B.
PO43–(aq)
C.
2Ca3(PO4)2(s)
D.
6NaBr(aq)
E.
3Ca2+(aq)
9.
Which of the following is not a strong base?
A.
Ca(OH)2
B.
KOH
C.
NH3
D.
LiOH
E.
Sr(OH)2
10.
Which of the following is paired incorrectly?
A.
HI – strong acid
B.
HNO3 – weak acid
C.
Ba(OH)2 – strong base
D.
HBr – strong acid
E.
NH3 – weak acid
11.
You have 2 solutions of chemical A. To determine which has the highest concentration of A in molarity, what is the minimum number of the following you must know? I. the mass in grams of A in each solution II. the molar mass of A III. the volume of water added to each solution IV. the total volume of the solution
A.
0
B.
1
C.
2
D.
3
E.
You must know all of them.
12.
In writing the total ionic equation for the reaction (if any) that occurs when aqueous solutions of KOH and Mg(NO3)2 are mixed, which of the following would not be written as ionic species?
A.
KOH
B.
Mg(NO3)2
C.
Mg(OH)2
D.
KNO3
E.
All of these would be written as ionic species.
13.
The following reactions 2K(s) + Br2(l) ® 2KBr(s) AgNO3(aq) + NaCl(aq) ® AgCl(s) + NaNO3(aq) HCl(aq) + KOH(aq) ® H2O(l) + KCl(aq) are examples of
A.
precipitation reactions.
B.
redox, precipitation, and acid-base, respectively.
C.
precipitation (two) and acid-base reactions, respectively.
D.
redox reactions.
E.
none of these
14.
Which of the following salts is insoluble in water?
A.
Na2S
B.
K3PO4
C.
Pb(NO3)2
D.
CaCl2
E.
All of these are soluble in water.
15.
Which of the following ions is most likely to form an insoluble sulfate?
A.
K+
B.
Li+
C.
Ca2+
D.
S2–
E.
Cl–
16.
Which of the following compounds is soluble in water?
A.
Ni(OH)2
B.
K3PO4
C.
BaSO4
D.
CoCO3
E.
PbCl2
17.
A solution contains the ions Ag+, Pb2+, and Ni2+. Dilute solutions of NaCl, Na2SO4, and Na2S are available to separate the positive ions from each other. In order to effect separation, the solutions should be added in which order?
A.
Na2SO4, NaCl, Na2S
B.
Na2SO4, Na2S, NaCl
C.
Na2S, NaCl, Na2SO4
D.
NaCl, Na2S, Na2SO4
E.
NaCl, Na2SO4, Na2S
18.
Which of the following do you need to know to be able to calculate the molarity of a salt solution? I. the mass of salt added II. the molar mass of the salt III. the volume of water added IV. the total volume of the solution
A.
I, III
B.
I, II, III
C.
II, III
D.
I, II, IV
E.
You need all of the information.
19.
You mix 60.0 mL of 1.0 M silver nitrate with 25.0 mL of 0.80 M sodium chloride. What mass of silver chloride should you form?
A.
2.9 g
B.
5.8 g
C.
8.7 g
D.
9.6 g
E.
none of these
20.
You have separate solutions of HCl and H2SO4 with the same concentrations in terms of molarity. You wish to neutralize a solution of NaOH. Which acid solution would require more volume (in mL) to neutralize the base?
A.
the HCl solution
B.
the H2SO4 solution
C.
You need to know the acid concentrations to answer this question.
D.
You need to know the volume and concentration of the NaOH solution to answer this question.
E.
You need to know the acid concentrations and the volume and concentration of the NaOH solution to answer this question.
21.
A mixture contained no fluorine compound except methyl fluoroacetate, FCH2COOCH3 (molar mass = 92.1 g/mol. When chemically treated, all the fluorine was converted to CaF2 (molar mass = 78.1 g/mol). The mass of CaF2 obtained was 12.1 g. Find the mass of methyl fluoroacetate in the original mixture.
A.
92.0 g
B.
28.5 g
C.
24.2 g
D.
14.3 g
E.
12.1 g
22.
A 1.000-g sample of a metal chloride, MCl2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chloride that formed weighed 1.286 g. Calculate the atomic mass of M.
A.
222.8 g
B.
76.00 g
C.
152.0 g
D.
304.0 g
E.
none of these
23.
A 0.307-g sample of an unknown triprotic acid is titrated to the third equivalence point using 35.2 mL of 0.106 M NaOH. Calculate the molar mass of the acid.
A.
247 g/mol
B.
171 g/mol
C.
165 g/mol
D.
151 g/mol
E.
82.7 g/mol
24.
A student weighs out 0.568 g of KHP (molar mass = 204 g/mol) and titrates to the equivalence point with 36.78 mL of a stock NaOH solution. What is the concentration of the stock NaOH solution? KHP is an acid with one acidic proton.
A.
0.100 M
B.
3.15 M
C.
0.943 M
D.
0.0757 M
E.
none of these
25.
In the reaction 2Ca(s) + O2(g) ® 2CaO(s), which species is oxidized?
A.
O2
B.
O2–
C.
Ca
D.
Ca2+
E.
none of these
26.
In the reaction P4(s) + 10Cl2(g) ® 4PCl5(s), the reducing agent is
A.
chlorine.
B.
PCl5.
C.
phosphorus.
D.
Cl–.
E.
none of these
27.
Given the following reaction in acidic media: Fe2+ + Cr2O72– ® Fe3+ + Cr3+ answer the following question: The coefficient for water in the balanced reaction is
A.
1.
B.
3.
C.
5.
D.
7.
E.
none of these
28.
The following unbalanced equation represents a reaction that occurs in basic solution: MnO42– + C2O42– ® MnO2 + CO32– How many moles of MnO42– are required to produce 1 mole of CO32–?
A.
4
B.
3
C.
2
D.
1
E.
none of these
29.
The following equation describes the oxidation of ethanol to acetic acid by potassium permanganate: 3C2H5OH + 4KMnO4 ® 3HC2H3O2 + 4MnO2 + 4KOH + H2O 5.0 g of ethanol and an excess of aqueous KMnO4 are reacted, and 5.9 g HC2H3O2 result. What is the percent yield?
A.
100%
B.
91%
C.
67%
D.
30.%
E.
5.9 g HC2H3O2 is impossible since it represents more than a 100% yield.
30.
Balance the following equation(s).
MnO4– + Br– ® MnO2 + BrO3– (base)
Answer:
31.
Balance the following equation(s).
Bi(OH)3 + SnO22– ® Bi + SnO32– (base)
Answer:
32.
Balance the following equation(s).
KI + HNO3 ® KNO3 + NO + I2 + H2O
Answer:
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