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Solubility/Net Ionic Equations/Redox/Molarity/Titration

Total questions: 101

Worksheet time: 2hrs 54mins

Name
Class
Date
1.
What precipitate forms when you mix lead (II) nitrate with sodium chloride?
a)
sodium nitrate 
b)
lead (II) chloride 
c)
sodium lead
d)
chloride nitrate 
2.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
3.
Which of the following does NOT form a precipitate?
a)
Pb(NO3)2(aq) + 2KI(aq) →
b)
Sr(NO3)2 (aq) + K2SO4(aq) →
c)
AgNO3(aq) + Na2S(aq) →
d)
 Pb(NO3)2(aq) + AgNO3(aq) →
4.
What are the spectator ions in the reaction of sodium chloride with silver nitrate?
a)
silver and nitrate
b)
sodium and chloride
c)
sodium and nitrate
d)
silver and chloride
5.
In the reaction
2Ca(s) + O2(g) → 2CaO(s), calcium is...
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
6.

In the reaction Zn + H2O → ZnO2 + H2 which element is oxidized? 

(a)  

7.
What substance is oxidized in the following reaction? 
Fe+2 + MnO4  → Fe+3 + Mn+2   
a)
Fe+2
b)
Mn+3
c)
Mn+2
d)
MnO4
8.

What is the oxidation number of N in NO2-1?

(a)  

9.
What is oxidation number of Mn in MnO2?
a)
0
b)
+2
c)
-2
d)
+4
10.
In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is insoluble?
a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
11.
Which of these results in formation of a precipitate?
a)
BaNO3(aq)  +  NaCl(aq)→
b)
KNO3(aq)  +  LiOH(aq)→
c)
Zn(NO3)2(aq)  +  NaOH(aq)→
d)
NaNO3(aq)  +  Ba(OH)2(aq)→
12.
What are the spectator ions in this reaction?
CuCl2(aq) + NaOH(aq) → Cu(OH)2(s) + NaCl(aq)
 
a)
Cu2+ and OH1-
b)
Na2+ and Cl2-
c)
Na1+ and Cl1-
d)
Na1+ and OH1-
13.
What is the result of the reaction between potassium bromide and ammonium sulfide?
a)
potassium sulfide precipitates
b)
ammonium bromide precipitates
c)
potassium ammonium precipitates
d)
no precipitate is formed
14.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
15.

In this equation,

CuCl2+ NaOH → Cu(OH)2 + NaCl

Identify the insoluble product?

a)

copper(II) hydroxide

b)

sodium chloride

c)

sodium hydroxide

d)

copper(II) chloride

16.

Identify the reaction that results in the formation of a precipitate.

a)

AgNO3(aq) + NaOH(aq)→

b)

BaNO3(aq) + CaCl2(aq)→

c)

NaNO3(aq) + KOH(aq)→

d)

More than one of these form precipitates

17.

Define: Solubility

a)

What is dissolved

b)

What does the dissolving

c)

A measure of how much solute can dissolve in solvent

d)

a charged ion

18.

What is the oxidation number of chlorine in HClO?

a)

0

b)

-1

c)

+1

d)

+5

19.

Oxidation is the (a)   of electrons.

20.

Reduction is the (a)   of electrons.

21.

What is the oxidation number of nitrogen in N2?

a)

-3

b)

0

c)

+4

d)

-1

22.

The sum of the oxidation numbers in SCN- is equivalent to

a)

0

b)

-1

c)

+1

d)

+3

23.

The sum of the oxidation numbers in Na2CO3 is equivalent to

(a)  

24.

Which of the following represents oxidation?

a)

C → CH4

b)

Fe3+ → Fe2+

c)

Cl2 → 2Cl-

d)

Zn → ZnO

25.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
26.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)
Oxidized
b)
Reduced
27.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
28.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

29.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

30.
Which of the following substances is a homogeneous solution?
a)
chocolate chip cookie
b)
italian dressing
c)
apple juice
d)
orange juice
31.
Which of the following substances is a heterogeneous substance?
a)
baby oil
b)
rocky road ice cream
c)
salt water
d)
milk
32.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

33.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

34.

What is the molality of a solution in which 3.0 moles of NaCl is dissolved in 1.5 Kg of water?

(a)  

35.

How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 

(a)  

36.

What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?

(a)  

37.

How many grams of solute are dissolved in 125.0 mL of 5.00 M NaCl (MM = 58.45)?

(a)  

38.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
39.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
40.

How many grams of AgNO3 are needed to prepare 0.125M solution in 250 mL of water? 

(a)  

41.
Which of the following has the most NaCl (MM = 58.44)?
a)
100 mL of a 1.8 M solution
b)
50 mL of a 4.1 M solution
c)
9.35 grams
d)
1 mole
42.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?

(a)  

43.

How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?

(a)  

44.
What volume of 1.50 M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
a)
150. mL
b)
151 mL
c)
1.00 L
d)
100. mL
45.

How many moles are needed to make 2.5 L of a 3.8 M solution? 

(a)  

46.

How many grams of AgNO3 are needed to prepare 0.125M solution in 250 mL of water? 

(a)  

47.
What is the volume in this burette?
a)
24.1mL
b)
24.3mL
c)
24.2L
d)
24.2mL
48.
Forms hydroxide ions in water
a)
Acids
b)
Bases
c)
All
49.

What is the concentration of citric acid if its volume is 25 ml and the titrated volume of the standard solution of 0.75 M is 12.4 ml

(a)  

50.

The concentration of the 30ml of citric acid solution is determined to be 1.23 M. Using the titration equation, predict the titration volume for the standard solution of 2.3 M.

(a)  

51.

Using n = MV, calculate the mass required to prepare 2.5 L of 1.0 M NaOH solution. Given the MM for NaOH is 40 g/mol

a)

1000 g

b)

100 g

c)

10 g

d)

1 kg

52.

In acid-base titration, the equivalent point is when

a)

a certain amount of acid has reacted completely with a certain amount of base according to stoichiometry

b)

a certain amount of acid has reacted partially with a certain amount of base according to stoichiometry

53.

How many moles of Na+ ions are there in

25cm3 of 0.01 mol/ L NaOH solution?

a)

0.25 mol

b)

2.5 mol

c)

2.5 x 10-4 mol

d)

2.5 x 10-3 mol

54.

How many moles of Na+ ions are there

in 0.025 L of 1.0 mol / L of Na2SO4 solution?

a)

0.025 mol

b)

2.5 x 103 mol

c)

0.05 mol

d)

1.0 x 10-3 mol

55.

HCl + NaOH --> NaCl + H2O

How many moles of NaOH will neutralise 18.3cm3 of 1.0 mol / L HCl solution?

a)

6.02 x 1023 mol

b)

1.83 x 104 mol

c)

0.0183 mol

d)

18.3 mol

56.

H2SO4 + 2NaOH --> Na2SO4 + 2H2O

How many moles of H2SO4 will neutralise 14.2 L of 0.01 mol/L NaOH?

a)

1.42 x 104 mol

b)

7.1 x 10-5 mol

c)

1.42 x 10-4 mol

d)

7.1 x 105 mol

57.

HCl + NaOH --> NaCl + H2O

What volume of 0.01 mol HCl solution will neutralise

50 mL of 0.01 mol NaOH solution?

(a)  

58.

HCl + NaOH --> NaCl + H2O

What volume of 0.5 mol/L HCl solution will neutralise

25cm3 of 1.0 mol/L NaOH solution?

a)

0.5cm3

b)

12.5cm3

c)

25cm3

d)

50cm3

59.
Describe a solute.
a)
part of solution present in largest amount
b)
gets dissolved
c)
water
d)
surrounds and breaks apart
60.

(a)   are made up of solutes and solvents.

61.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
62.
If I dissolve carbon dioxide in water, what is my solvent?
a)
Carbon Dioxide
b)
There is no solvent
c)
Oxygen
d)
Water
63.
NH4NO3
a)
soluble
b)
insoluble
64.
AgCl
a)
soluble
b)
insoluble
65.
FeS
a)
soluble
b)
insoluble
66.
BaSO4
a)
soluble
b)
insoluble
67.
NaC2H3O2
a)
soluble
b)
insoluble
68.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
69.

What of these is always soluble?

a)

Nitrates

b)

Phosphates

c)

Carbonates

d)

Hydroxides

70.
Fe(C2H3O2)3
a)
soluble
b)
insoluble
71.
K2SO4
a)
soluble
b)
insoluble
72.

The word "INSOLUBLE" meaning ________

a)

Something which dissolve in water/liquid

b)

Something which cannot dissolve in water/liquid

c)

none

d)

both

73.

Which of the following is not a type of reduction

a)

Gain of hydrogen

b)

loss of electron

c)

loss of oxygen

d)

gain of electron

74.

What is the precipitate formed between CaCl2 and NaOH?

a)

CaCl2

b)

NaOH

c)

Ca(OH)2

d)

NaCl

e)

no precipitate is formed

75.

Will the reaction between Cu(NO3)2 and K2SO4 happen?

a)

yes

b)

no

76.

Which equation is a double displacement reaction?

a)

Cl2 + 2KI --> 2KCl

b)

Fe + O2 --> Fe2O3

c)

CaCO3 --> CO2 + CaO

d)

CaCO3 + 2HCl --> CaCl2 + H2CO3

77.

What is the correct products for a reaction between NaNO3 and CuCl2

a)

NaCu + ClNO3

b)

NaCl + Cu(NO3)2

c)

NaNO3 + CuCl2

d)

No reaction occurs

78.

Which among the following is(are) double displacement

reaction(s)?

(i) Pb + CuCl2 --> PbCl2 + Cu

(ii) Na2SO4 + BaCl2 --> BaSO4 + 2NaCl

(iii) C + O2 --> CO2

(iv) CH4 + 2O2 --> CO2 + 2H2O

a)

(a) (i) and (iv)

b)

(b) (ii) only

c)

(c) (i) and (ii)

d)

(d) (iii) and (iv)

79.

Based on the activity series, will this reaction occur?

Au (s) + HCl (aq) →

a)

Yes

b)

No

80.

Determine the two products when Na3PO4 reacts with SnO2.

a)

NaO and SnPO4

b)

Na2O and Sn(PO4)2

c)

Na2O and Sn3PO4

d)

Na2O and Sn3(PO4)4

81.

___ Na2CO3 + ___ Ag3P → ___ Na3P + ___ Ag2CO3

a)

3, 2, 1, 3

b)

2, 2, 2, 3

c)

3, 2, 2, 3,

d)

3, 2, 3, 2

82.

What is the oxidation number of chlorine in HClO?

(a)  

83.

What is the oxidation number of iodine in KIO3?

a)

0

b)

-1

c)

+5

d)

+1

84.

In the reaction Zn + 2HCl --> ZnCl2 + H2

which element, if any, is oxidized?

a)

Zinc

b)

Hydrogen

c)

Chlorine

d)

None

85.

If I have 340.0 mL of a 0.500 M NaBr solution, what will the concentration be if I add 560.0 mL more water to it? (Remember to use the total new volume)

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

86.

Match the following

a)

term that describes the strength or concentration of a solution

1.

molarity

b)

adding solvent to make solution less concentrated

2.

dilution

c)

describes the ability for a substance to dissolve at a specific temperature

3.

solubility

d)

a substance that dissolves another substance

4.

solvent

e)

a substance that is being dissolved by another substance

5.

solute

87.

The higher the molarity, the ________ the solution

a)

more concentrate

b)

less concentrated

88.

How many mL of 1.0M KBr solution would you need to prepare 250 mL of a 0.2M dilution?

a)

175 mL

b)

250 mL

c)

50 mL

d)

5 mL

89.

If it takes 50 mL of 0.5 M KOH solution to completely neutralize 125 mL of sulfuric acid solution. What is the concentration of the H2SO4 solution?

(a)  

90.

If it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the concentration of the NaOH solution?0.0036

(a)  

91.

A 20.00 mL sample of a solution of Sr(OH)2 is titrated to the equivalence point with 43.03 mL of 0.1159 M HCl. What is the molarity of the Sr(OH)2 solution?

a)

0.06235 M

b)

0.1247 M

c)

0.2494 M

d)

0.1159 M

92.

A 35.00 mL sample of ammonia solution is titrated to the equivalence point with 54.95 mL of a 0.400 M sulfuric acid solution. What is the molarity of the ammonia solution?

a)

0400

b)

0.630 M

c)

1.26 M

d)

2.54 M

93.

A student titrates a 20.00 mL sample of a solution of HBr with unknown molarity. The titration requires 20.05 mL of a 0.1819 M solution of NaOH. What is the molarity of the HBr solution?

(a)  

94.

Vinegar can be assayed to determine its acetic acid content. Determine the molarity of acetic acid in a 15.00 mL sample of vinegar that requires 22.70 mL of a 0.550 M solution of NaOH to reach the equivalence point.

a)

0.416 M

b)

0.832 M

c)

1.66 M

d)

0.550 M

95.
Which is the correct net ionic equation for the reaction of AgNO3 and CaCl2?
a)
Ca2+(aq) +  2Cl1- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl1- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
96.

Which of the following reactions does NOT have a net ionic equation?

a)

C9H20 + O2 --> CO2 + H2O

b)

AgNO3 + CaCl2 --> AgCl + Ca(NO3)2

c)

NH4I + PbOH --> NH4OH + PbI2

d)

Fe(NO3)2 + KOH --> KNO3 + FeOH

97.
Which pair could be spectator ions?
a)
NH4+ and Cl-
b)
Ca+2 and OH-
c)
Ag+ and Br-
d)
Sr+2 and CO3 -2
98.

Write out the full ionic equation and the net ionic equation for the reaction:

sodium sulfate(aq) + silver nitrate(aq) -->

4 lines
99.

Net ionic equations for the reaction: magnesium chloride(aq) + lithium carbonate(aq) -->

4 lines
100.

Net ionic equations for the reaction: potassium hydroxide (aq) + aluminum nitrate (aq)

4 lines
101.
What is the precipitate formed between potassium bromide and ammonium sulfide
a)
potassium sulfide
b)
ammonium bromide
c)
potassium ammonium
d)
no ppt is formed

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