Upload
dominic-hunt
View
219
Download
1
Embed Size (px)
Citation preview
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
1
QUESTIONAn unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? 1) Neither polar nor nonpolar 2) Polar 3) Either polar or nonpolar 4) Nonpolar 5) none of these
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
2
ANSWER2) Polar Section 4.1 Water, the Common Solvent (p. 134) The solubility rule for molecular compounds is “like dissolves like”, that is, polar molecules dissolve in polar solvents and nonpolar molecules dissolve in nonpolar solvents.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
3
QUESTIONHow many grams of NaCl are contained in 350. mL of a 0.250 M solution of sodium chloride? 1) 41.7 g 2) 5.11 g 3) 14.6 g 4) 87.5 g 5) None of these
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
4
ANSWER2) 5.11 g Section 4.3 The Composition of Solutions (p. 140) Volume (L) times concentration (mol/L) gives moles. Moles are then converted to grams.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
5
QUESTIONWhat volume of 18.0 M sulfuric acid must be used to prepare 15.5 L of 0.195 M H2SO4? 1) 168 mL 2) 0.336 L 3) 92.3 mL 4) 226 mL 5) None of these
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
6
ANSWER1) 168 mL Section 4.3 The Composition of Solutions (p. 140) Use the dilution formula, M1
V1 = M2 V2, M is
in mol/L and V is in L.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
7
QUESTIONThe net ionic equation for the reaction of aluminum sulfate and sodium hydroxide contains which of the following species? 1) 3Al
3+(aq)
2) OH–(aq)
3) 3OH–(aq)
4) 2Al3+
(aq) 5) 2Al(OH)3(s)
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
8
ANSWER
3) 3OH–(aq)
Section 4.6 Describing Reactions in Solution (p. 154) The net ionic equation is found by canceling the spectator ions from the total ionic equation.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
9
QUESTIONWhich of the following is a strong acid? 1) HF 2) KOH 3) HClO4 4) HClO 5) HBrO
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
10
ANSWER3) HClO4 Section 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes (p. 136) Memorization of the list of strong acids will allow one to determine the difference between strong acids and weak acids.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
11
QUESTIONAll of the following are weak acids except: 1) HCNO. 2) HBr. 3) HF. 4) HNO2. 5) HCN.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
12
ANSWER2) HBr. Section 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes (p. 136) Knowing the list of strong acids will allow one to determine which acids are strong and which are weak.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
13
QUESTIONWhich of the following is not a strong base? 1) Ca(OH)2 2) KOH 3) NH3 4) LiOH 5) Sr(OH)2
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
14
ANSWER3) NH3 Section 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes (p. 136) Knowing the list of strong bases will allow one to determine which bases are strong and which are weak.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
15
QUESTIONThe interaction between solute particles and water molecules, which tends to cause a salt to fall apart in water, is called: 1) hydration. 2) polarization. 3) dispersion. 4) coagulation. 5) conductivity.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
16
ANSWER1) hydration. Section 4.1 Water, the Common Solvent (p. 134) Hydration is the process of water molecules surrounding and stabilizing ions so that they can be pulled into solution.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
17
QUESTION
The concentration of a salt water solution that sits in an open beaker decreases over time.
1) True 2) False
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
18
ANSWER2) False Section 4.3 The Composition of Solutions (p. 140) The amount of water decreases over time so the concentration (mol NaCl/volume of water) increases over time.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
19
QUESTIONThe following reactions: Pb
2+ + 2I
– PbI2
2Ce4+ + 2I
– I2 + 2Ce
3+
HOAc + NH3 NH4
+ + OAc
–
are examples of
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
20
QUESTION (continued)
1) acid-base reactions. 2) unbalanced reactions. 3) precipitation, acid-base, and redox
reactions, respectively. 4) redox, acid-base, and precipitation
reactions, respectively. 5) precipitation, redox, and acid-base
reactions, respectively.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
21
ANSWER5) precipitation, redox, and acid-base
reactions, respectively. Section 4.5 Precipitation Reactions (p. 151) PbI2 is insoluble, Ce
4+ changes to Ce
3+ and
HOAc is an acid while NH3 is a base.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
22
QUESTIONWhich of the following salts is insoluble in water? 1) Na2S 2) K3PO4 3) Pb(NO3)2 4) CaCl2 5) All of these are soluble in water.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
23
ANSWER5) All of these are soluble in water. Section 4.5 Precipitation Reactions (p. 153) According to the solubility rules for ionic compounds, compounds containing Group IA ions or nitrate ions will always be soluble. Compounds containing halides are generally soluble, aside from silver, lead and mercury(I) halides.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
24
QUESTION
When NH3(aq) is added to Cu2+
(aq), a precipitate initially forms. Its formula is: 1) Cu(NH3)4
2+
2) Cu(NO3)2 3) Cu(OH)2 4) Cu(NH3)4
2+
5) CuO
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
25
ANSWER3) Cu(OH)2 Section 4.4 Types of Chemical Reactions (p. 148) Ammonia produces hydroxide ion in water: NH3 + H2O NH4
+ + OH
–
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
26
QUESTIONIn the balanced molecular equation for the neutralization of sodium hydroxide with sulfuric acid, the products are: 1) NaSO4 + H2O 2) NaSO3 + 2H2O 3) 2NaSO4 + H2O 4) Na2S + 2H2O 5) Na2SO4 + 2H2O
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
27
ANSWER5) Na2SO4 + 2H2O Section 4.8 Acid-Base Reactions (p. 158) The salt is made from the anion of the acid and the cation of the base.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
28
QUESTIONWhat mass of NaOH is required to react exactly with 25.0 mL of 1.2 M H2SO4? 1) 1.2 g 2) 1.8 g 3) 2.4 g 4) 3.5 g 5) None of these
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
29
ANSWER3) 2.4 g Section 4.8 Acid-Base Reactions (p. 158) Remember that the reaction is 2NaOH + H2SO4 Na2SO4 + 2H2O, so there are two moles of NaOH used per one mole of H2SO4.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
30
QUESTIONIn which of the following does nitrogen have an oxidation state of +4? 1) HNO3 2) NO2 3) N2O 4) NH4Cl 5) NaNO2
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
31
ANSWER2) NO2 Section 4.9 Oxidation-Reduction Reactions (p. 164) Oxygen almost always has an oxidation state of –2 when part of a compound. The exception is when it is part of a peroxide. For example, hydrogen peroxide H2O2. Then it has an oxidation state of –1.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
32
QUESTION
In the reaction 2Cs(s) + Cl2(g) 2CsCl(s), Cl2 is 1) the reducing agent. 2) the oxidizing agent. 3) oxidized. 4) the electron donor. 5) two of these
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
33
ANSWER2) the oxidizing agent. Section 4.9 Oxidation-Reduction Reactions (p. 164) Metals lose electrons, so they are oxidized, making the other reactant an oxidizing agent.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
34
QUESTIONWhich of the following statements is(are) true? Oxidation and reduction: 1) cannot occur independently of each other. 2) accompany all chemical changes. 3) describe the loss and gain of electron(s),
respectively. 4) result in a change in the oxidation states of
the species involved. 5) 1, 3, and 4 are true
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
35
ANSWER5) 1, 3, and 4 are true. Section 4.9 Oxidation-Reduction Reactions (p. 167) (2) is false because certain reactions, such as double displacement reactions, are not redox reactions.
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
36
QUESTIONHow many of the following are oxidation-reduction reactions? NaOH + HCl NaCl + H2O Cu + 2AgNO3
2Ag + Cu(NO3)2 Mg(OH)2
MgO + H2O N2 + 3H2
2NH3
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
37
QUESTION (continued)
1) 0 2) 1 3) 2 4) 3 5) 4
Copyright©2000 by Houghton Mifflin Company. All rights
reserved.
38
ANSWER3) 2 Section 4.9 Oxidation-Reduction Reactions (p. 164) If an element is found on the reactant’s side, this is almost always a redox reaction, since an element usually becomes part of a compound during a chemical reaction.