Chapter 5 Kotz5e Multiple Choice Sample Test

1. Which of the following ionic compounds is insoluble in water?

a.

NH4Cl

b.

Li2CO3

c.

PbSO4

d.

KI

e.

Na2S


2. All of the following compounds are soluble in water EXCEPT

 

a.

NaCl.

b.

ZnCl2.

c.

FeCl2.

d.

BaCl2.

e.

Hg2Cl2.


3. All of the following compounds are insoluble in water EXCEPT

 

a.

CuS.

b.

Hg2Cl2.

c.

(NH4)2S.

d.

Zn(OH)2.

e.

BaSO4.


4. Solutions of the following are mixed. A precipitate would be formed by

 

a.

NaNO3 and NH4Cl.

b.

CuSO4 and KCl.

c.

AgNO3 and CsBr.

d.

NaCl and Fe(NO3)2.

e.

HCl and NaOH.

 

 

 

 

 

 

5. The net ionic equation for neutralization of benzoic acid by a base is

C6H5COOH(aq) + OH-(aq) --> C6H5COO-(aq) + H2O(l)

Therefore,

a.

benzoic acid is a strong acid.

b.

the base is a weak base.

c.

the C6H5COO- ion is a spectator ion.

d.

the ion, K+, could be a spectator ion.

e.

the base in the titration could be NH3.


6. The net ionic equation for the reaction of hydrobromic acid with potassium hydroxide
isTop of Form

a.

HBrO3(aq) + OH-(aq) --> BrO3-(aq) + H2O(l)

b.

HBr(aq) + OH-(aq) --> Br-(aq) + H2O(l)

c.

H+(aq) + OH-(aq) --> H2O(l)

d.

HBrO3(aq) + KOH(aq) --> KBrO3(aq) + H2O(l)

e.

HBr(aq) + KOH(aq) --> KBr(aq) + H2O(l)

 



 

 

7. All of the following are strong acids and weak acids respectively EXCEPT

a.

HNO3 and HNO2.

b.

H2SO4 and H2SO3.

c.

HClO4 and HClO.

d.

HClO3 and HClO2.

e.

H3PO4 and HClO.



8. Which of the following is a weak electrolyte in aqueous solution?

 

a.

H2S

b.

H2SO4

c.

HI

d.

HNO3

e.

HClO3


9. Which of the following nonmetal oxides is paired with the acid which will result from the addition of water to the nonmetal oxide?

 

a.

NO2 and HNO2

b.

SO3 and H2SO4

c.

P4O10 and H3PO3

d.

N2O5 and HNO2

e.

NO and HNO2

 

10. All of the following statements represent characteristic properties of acids EXCEPT

 

a.

proton donors.

b.

react with bases to produce a salt and water.

c.

will hydrolyze and produce hydroxide ions.

d.

turn blue litmus red.

e.

produce carbon dioxide from metal carbonates.


11. Besides its ability to function as an acid, sulfuric acid is able to act as an oxidizing agent. Which one of the following equations illustrates this ability?

a.

CaF2(s) + H2SO4(aq) --> CaSO4(aq) + 2HF(aq)

b.

2NH3(g) + H2SO4(aq) --> 2NH4+(aq) + SO42-(aq)

c.

2H+(aq) + 2NaI(s) + H2SO4(aq) --> I2(s) + 2H2O + SO2(g) + 2Na+

d.

e.

NaCl(s) + H2SO4(aq) --> NaHSO4(aq) + HCl(aq)


12. In the balanced equation

3Na+ + 3OH- + P4 + 3H2O --> 3Na+ + 3H2PO2- + PH3

the reducing agent is

 

a.

Na+.

b.

OH-.

c.

P4.

d.

H2O.

e.

H2PO2-.


13. The oxidation number of boron in the compound H3BO3 is

 

a.

0.

b.

1.

c.

2.

d.

3.

e.

6.



14. The oxidation number of nitrogen in Ca(NO2)2 is

a.

1.

b.

2.

c.

3.

d.

4.

e.

5.



15. Consider the reactions represented by the following net ionic equations:

1. 2Na(s) + 2H3O+(aq) --> 2Na+(aq) + H2(g) + 2H2O(l)
2. O2-(aq) + H2O(aq) --> 2OH-(aq)
3. Cu2+(aq) + H2S(g) --> CuS(s) + 2H+(aq)

The equation(s) which would be classified as oxidation-reduction(s) is (are)

 

a.

1 only.

b.

2 only.

c.

1 and 2 only.

d.

1 and 3 only.

e.

1, 2, and 3.


16. The molarity of a solution is defined as

a.

the number of moles of solute per kilogram of solvent.

b.

the number of moles of solute per liter of solution.

c.

the number of gram-equivalent weights of solute per liter of solution.

d.

the number of gram-equivalent weights of solute per kilogram of solution.

e.

the number of moles of solute per liter of solvent.


17. Calculate the molarity of a solution that contains 56.0 g of HCl in 265 mL of solution.
(Molar Mass HCl = 36.5 g/mol)

a.

2.94

b.

5.79

c.

6.35

d.

7.06

e.

7.60



18. How many g of KOH are contained in 400. mL of 0.250 M KOH solution?

a.

5.61 g

b.

8.98 g

c.

12.4 g

d.

35.1 g

e.

89.8 g



19. The number of mol of sulfate ions in a 0.1 liter solution of 0.02 M Al2(SO4)3 is

a.

0.002 mol

b.

0.004 mol

c.

0.006 mol

d.

0.024 mol

e.

0.06 mol



20. What volume of 0.750 molar H2SO4 must be taken to obtain 0.273 moles of H2SO4?

a.

0.205 L

b.

0.364 L

c.

1.12 L

d.

2.74 L

e.

3.00 L


21. Which one of the following is an example of an oxidation-reduction reaction?

a.

SO3(g) + H2O(l) --> H2SO4(aq)

b.

P4O10(s) + 6Na2O(s) --> 4Na3PO4(s)

c.

I2(aq) + H2O(l) --> HOI(aq) + HI(aq)

d.

CaCO3(s) --> CaO(s) + CO2(g)

e.

Al2O3(s) + 3H2O(aq) + 2OH-(aq) --> 2Al(OH)4-(aq)



22. What volume of 0.500 molar nitric acid, HNO3, is required to react with 3.70 g of calcium hydroxide, Ca(OH)2, according to the following equation?

a.

25.0 mL

b.

50.0 mL

c.

82.0 mL

d.

100.0 mL

e.

200.0 mL

2HNO3 + Ca(OH)2 --> Ca(NO3)2 + 2H2O



 

 

23. How many mL of 0.300 M NaOH are required to react with 500. mL of 0.170 M H3PO4 to yield Na2HPO4? (First write a balanced equation.)

a.

94.4

b.

142

c.

283

d.

567

e.

850



24. To prepare 100. ml of 0.50 M HCl from 2.00 M HCl, what volume of acid must you use?

a.

25.0 ml

b.

50.0 ml

c.

100. ml

d.

200. ml

e.

400. ml



25. How many grams of PbCl2 would be precipitated if an excess of Pb(NO3)2 solution were added to 75.0 mL of 0.200 M KCl solution? (Formula mass PbCl2 = 278.1 g mol-1)

a.

1.04

b.

2.09

c.

4.17

d.

8.34

e.

41.7