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Chapter 8 Prep Test

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 
 

General Solubility Guidelines
1. Most sodium, potassium, and ammonium compounds are soluble in water.
2. Most nitrates, acetates, and chlorates are soluble.
3. Most chlorides are soluble, except those of silver, mercury(I), and lead. Lead(II) chloride is soluble in hot water.
4. Most sulfates are soluble, except those of barium, strontium, and lead.
5. Most carbonates, phosphates, and silicates are insoluble, except those of sodium, potassium, and ammonium.
6. Most sulfides are insoluble, except those of calcium, strontium, sodium, potassium, and ammonium.
 

 1. 
Which of the following pairs of solutions produces a precipitate when combined?
a.
KOH and NH4Cl
c.
Na2SO4 and KCl
b.
Fe(NO)3 and KCl
d.
NH4Cl and AgNO3
 

 2. 
When solutions of NH4OH and K2SO4 are combined, what precipitate(s) forms?
a.
(NH4)2SO4
c.
(NH4)2SO4 and KOH
b.
KOH
d.
None of the above
 

 3. 
What is the driving force in the following reaction?
Ni(NOmc003-1.jpg)mc003-2.jpg(aq) mc003-3.jpg Kmc003-4.jpgS(aq) mc003-5.jpg NiS(s) mc003-6.jpg 2KNOmc003-7.jpg(aq)
a.
A gas is formed.
c.
Ionic compounds are reactants.
b.
A precipitate is formed.
d.
Ionic compounds are products.
 

 4. 
Which compound dissociates to produce the ions Ca2+(aq) and NO3–(aq)?
a.
CaNO3(s)
c.
Ca(NO3)2(s)
b.
Ca2NO3(s)
d.
Ca2(NO3)3(s)
 

 5. 
If a combination/synthesis reaction takes place between rubidium and bromine, the chemical formula for the product is ____.
a.
RuBr
b.
Rbmc005-1.jpgBr
c.
RbBrmc005-2.jpg
d.
RbBr
 

 6. 
Which of the following is NOT a net ionic equation?
a.
Ag+(aq) + Cl–(aq) ® AgCl(s)
b.
Fe2+(aq) + 2Cl–(aq) + 2OH–(aq) ® Fe(OH)2(s) + 2Cl–(aq)
c.
3Ca2+(aq) + 2P3–(aq) ® Ca3P2(s)
d.
Cu2+(aq) + S2–(aq) ® CuS(s)
 

 7. 
Which compound dissociates to produce the ions SO42–(aq) and NH4+(aq)?
a.
NH4SO4(s)
c.
NH4(SO4)2(s)
b.
(NH4)2SO4(s)
d.
(NH4)3(SO4)2(s)
 

 8. 
A double-replacement reaction takes place when aqueous Namc008-1.jpgCOmc008-2.jpg reacts with aqueous Sn(NOmc008-3.jpg)mc008-4.jpg. You would expect one of the products of this reaction to be ____.
a.
Na2COmc008-5.jpg
b.
NaSn
c.
SnCOmc008-6.jpg
d.
CNOmc008-7.jpg
 

 9. 
The equation 2Cmc009-1.jpgHmc009-2.jpgOH mc009-3.jpg 9Omc009-4.jpg mc009-5.jpg 6COmc009-6.jpg mc009-7.jpg 8Hmc009-8.jpgO is an example of which type of reaction?
a.
combustion reaction
c.
double-replacement reaction
b.
single-replacement reaction
d.
decomposition reaction
 

 10. 
Which of the following would form when Al(NO3)3(s) dissolves in water ?
a.
Al+ + (NO3)3–
c.
Al3+ + NO33–
b.
Al3+(aq) + 3NO3–(aq)
d.
Al3–(aq) + 3NO3+(aq)
 

 11. 
When solutions of two ionic compounds are combined and a solid forms, the process is called
a.
hydration.
c.
solvation.
b.
precipitation.
d.
dissociation.
 

 12. 
Which of the following is a balanced equation representing the decomposition of lead(IV) oxide?
a.
PbOmc012-1.jpg mc012-2.jpg Pb mc012-3.jpg 2O
c.
Pbmc012-8.jpgO mc012-9.jpg 2Pb mc012-10.jpg O
b.
PbOmc012-4.jpg mc012-5.jpg Pb mc012-6.jpg Omc012-7.jpg
d.
PbO mc012-11.jpg Pb mc012-12.jpg Omc012-13.jpg
 

 13. 
Which of the following pairs of solutions produce a precipitate when combined?
a.
Cu(NO3)2 and NaCl
c.
Cu(NO3)2 and K2CO3
b.
Fe(NO3)3 and MgCl2
d.
CaCl2 and NaNO3
 

 14. 
The reaction 2Fe mc014-1.jpg 3Clmc014-2.jpg mc014-3.jpg 2FeClmc014-4.jpg is an example of which type of reaction?
a.
combustion reaction
c.
combination/synthesis reaction
b.
single-replacement reaction
d.
decomposition reaction
 

 15. 
What is the net ionic equation for the precipitation reaction between copper(II) chloride and sodium hydroxide?
a.
Cu2+(aq) + 2OH–(aq) ® Cu(OH)2(s)
b.
Na+(aq) + Cl–(aq) ® NaCl(s)
c.
Cu2+(aq) + 2OH–(aq) + 2Cl–(aq) ® Cu(OH)2(s) + 2Cl–(aq)
d.
Cu2+(aq) + 2Cl–(aq) + 2Na+(aq) + 2OH–(aq) ® Cu(OH)2(s) + 2NaCl(s)
 

 16. 
Which of the following dissociates in water?
a.
NaCl
b.
Cl2
c.
AgCl
d.
C6H6
 

 17. 
Which of the following would form when K2S(s) dissolves in water?
a.
2K+(aq) + S2–(aq)
c.
K2+(aq) + S2–(aq)
b.
K22+(aq) + S2–(aq)
d.
2K(aq) + S(aq)
 

 18. 
What is the spectator ion in the equation
2Na+(aq)  + S2–(aq)+ Zn2+(aq) +  2NO3–(aq)® 2Na+(aq)+ 2NO3-(aq) + ZnS(s)?
a.
ZnS(s)
b.
Na+(aq)
c.
S2–(aq)
d.
none of these
 

 19. 
Which of the following statements is true about single-replacement reactions?
a.
They are restricted to metals.
b.
They involve a single product.
c.
One reactant switches places with another.
d.
Any metal replaces any other metal.
 

 20. 
In a double-replacement reaction, the ____.
a.
products are always carbon dioxide and water
b.
reactants are usually two ionic compounds
c.
reactants are two elements
d.
products are a new element and a new compound
 

 21. 
A precipitation is an example of what type of reaction?
a.
composition
c.
single-replacement
b.
decomposition
d.
double-replacement
 

 22. 
A double-replacement reaction takes place when aqueous cobalt(III) chloride reacts with aqueous lithium hydroxide. One of the products of this reaction is ____.
a.
Co(OH)mc022-1.jpg
b.
Co(OH)mc022-2.jpg
c.
LiComc022-3.jpg
d.
LiClmc022-4.jpg
 

 23. 
In a combustion reaction, one of the reactants is always ____.
a.
hydrogen
b.
nitrogen
c.
oxygen
d.
a metal
 

 24. 
The type of reaction that takes place when one element reacts with a compound to form a new compound and a different element is a ____.
a.
combination/synthesis reaction
c.
single-replacement reaction
b.
decomposition reaction
d.
double-replacement reaction
 

 25. 
What are the correct formulas and coefficients for the products of the following acid/base (double replacement) reaction when the reaction is balanced?
RbOH mc025-1.jpg Hmc025-2.jpgPOmc025-3.jpg mc025-4.jpg
a.
Rb(POmc025-5.jpg)mc025-6.jpg mc025-7.jpg Hmc025-8.jpgO
c.
Rbmc025-12.jpgPOmc025-13.jpg mc025-14.jpg 3Hmc025-15.jpgO
b.
RbPOmc025-9.jpg mc025-10.jpg 2Hmc025-11.jpgO
d.
Hmc025-16.jpgRb mc025-17.jpg POmc025-18.jpgOH
 

 26. 
The equation Mg(s) mc026-1.jpg 2HCl(aq) mc026-2.jpg MgClmc026-3.jpg(aq) mc026-4.jpg Hmc026-5.jpg(g) is an example of which type of reaction?
a.
combination reaction
c.
decomposition reaction
b.
single-replacement reaction
d.
double-replacement reaction
 

 27. 
The equation Hmc027-1.jpgPOmc027-2.jpg (aq)mc027-3.jpg 3KOH(aq) mc027-4.jpg Kmc027-5.jpgPOmc027-6.jpg(aq)mc027-7.jpg 3Hmc027-8.jpgO(l) is an example of which type of reaction?
a.
double-replacement reaction
c.
decomposition reaction
b.
combination reaction
d.
single-replacement reaction
 

Matching
 
 
32-34 Match each equation with its correct type
a.
acid-base reaction/double replacement
c.
precipitation reaction/double replacement
b.
single replacement
d.
synthesis
 

 28. 

 Mg(s) ma028-1.jpg 2HCl(aq) ma028-2.jpg MgClma028-3.jpg(aq) ma028-4.jpg Hma028-5.jpg(g)
 

 29. 

 Ba(NOma029-1.jpg)ma029-2.jpg(aq) ma029-3.jpg Kma029-4.jpgSO4(aq) ma029-5.jpg BaSO4(s) ma029-6.jpg 2KNOma029-7.jpg(aq)
 

 30. 

 Hma030-1.jpgPOma030-2.jpg (aq)ma030-3.jpg 3KOH(aq) ma030-4.jpg Kma030-5.jpgPOma030-6.jpg(aq)ma030-7.jpg 3Hma030-8.jpgO(l)
 

 31. 

 2H2(g) + O2(g)  ma031-1.jpg 2H2O(g)
 
 
28 - 31 Match each item with the correct statement below.
a.
combination/synthesis reaction
c.
combustion reaction
b.
single-replacement reaction
d.
decomposition reaction
 

 32. 

 a reaction where one element switches places with the cation of the other reactant
 

 33. 

 a reaction in which a single compound is broken down into simpler substances
 

 34. 

 a reaction in which 2 or more substances react to form one substance.
 

 35. 

 a reaction in which oxygen reacts with another substance, often producing heat or light
 



 
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