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Davis PAP Chem Solutions Review

Total questions: 77

Worksheet time: 3hrs 30mins

Name
Class
Date
1.
Type of intermolecular force present in HF.
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
2.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
3.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
4.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
5.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
6.

CHECK ALL THAT APPLY:

Electronegative atoms that are often involved in Hydrogen Bonds.

a)

Nitrogen

b)

Carbon

c)

Oxygen

d)

Fluorine

e)

Calcium

7.

The Oxygen atoms in the molecule shown have this charge:

a)

Positive

b)

Partial Positive

c)

Negative

d)

Partial Negative

8.

Hydrogen bonds are VERY important in determining the many properties of this very important molecule

(a)  

9.

Define the term insoluble.

a)

Can dissolve in water.

b)

Cannot dissolve in water.

c)

Partially dissolves in water.

10.

Define the term soluble.

a)

Can dissolve in water

b)

Cannot dissolve in water

c)

Partially dissolves in water

11.

The substance being dissolved in a solution is the?

a)

solution

b)

solute

c)

solvent

d)

mixture

12.

When 40 grams of NaCl is dissolved in 100 grams of water at 90 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

13.

A homogeneous mixture is the same thing as...

a)

a solution

b)

a heterogeneous mixture

c)

a compound

d)

an element

14.

The prefix hetero means...

a)

same

b)

different

c)

together

d)

awesome

15.

A type of mixture that forms when one substance dissolves in another is known as a

a)

heterogeneous mixture

b)

solution

c)

solute

d)

solvent

16.
What does it mean to dilute a solution?
a)
lower the concentration of solute per solvent
b)
increase the concentration of solute per solvent
17.
What is a solvent
a)
the liquid in which a solute is dissolved to form a solution.
b)
Another word for solution
c)
A thing that make drinks turn colors
d)
Its a metal molecole
18.

Which substance is least soluble at 0 ºC?

a)

KI

b)

KNO3

c)

KClO3

d)

Ce2(SO4)3

19.

How many grams are soluble in 100 g of water at 100 ºC?

a)

300 grams

b)

250 grams

c)

100 grams

d)

50 grams

20.

Which solute is most likely a gas?

a)

NH3

b)

NaNO3

c)

KCl

d)

NaCl

21.

When 40 grams of NaCl is dissolved in 100 grams of water at 90 ºC, the solution can be correctly described as:

a)

supersaturated

b)

saturated

c)

unsaturated

22.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
23.
You can make a solution more concentrated by adding __________.
a)
solute
b)
solvent
c)
water
24.
Solution where more solute can still be dissolved at the given temperature. 
a)
Saturated
b)
Unsaturated
c)
Supersaturated
d)
Homogeneous solution
25.
A solution of potassium chlorate, KClO3, has 20 grams of the salt dissolved in 100 grams of water at 70 ºC. Approximately how many more grams of the salt can be added to the solution before reaching the saturation point?
a)
10 grams
b)
30 grams
c)
80 grams
d)
60 grams 
26.

Identify how many grams of KNO3 is required to make a saturated solution at 40'C.

a)

50 g

b)

45 g

c)

55 g

d)

33 g

27.

Water is considered polar due to:

a)

its neutral poles

b)

its charged poles

c)

the odd number of atoms involved

28.
If I dissolve sugar in water, what is the solute?
a)
Water
b)
Hydrogen
c)
Sugar
d)
Carbon
29.
What will allow more solute to be dissolved in a solvent.
a)
adding more solute
b)
stiring
c)
cooling solution
d)
heat
30.
Graph that shows the amount of solute that can be dissolved in 100 g of water at a certain temperature.
a)
Solubility curve
b)
Saturation curve
c)
Concentration curve
d)
Molarity curve
31.

Identify the saturation associated with the product of this experiment.

a)

Unsaturated

b)

Saturated

c)

Supersaturated

32.

What is the solvent example in this picture?

a)

Sugar

b)

Water

c)

Solution

33.
What is a precipitate?
a)
an insoluble reactant formed during a chemical reaction
b)
an insoluble product formed during a chemical reaction
c)
a soluble solvent in a saturated solution
d)
a soluble solute in a saturated solution
34.
Which of the following usually makes a substance dissolve faster in a solvent?
a)
agitating the solution
b)
increasing the particle size of the solute
c)
lowering the temperature
d)
decreasing the number of particles
35.

Polar solutes will dissolve in _________ solvents. Nonpolar solutes will dissolve in ____________ solvents.

a)

polar, polar

b)

polar, nonpolar

c)

nonpolar, polar

d)

nonpolar, polar

36.

Two liquids that are soluble in each other in any proportion are said to be:

a)

insoluble

b)

 immiscible

c)

miscible

d)

soluble

37.

When the solution equilibrium point is reached and no more solute will dissolve, the solution is said to be _________.

a)

unsaturated

b)

saturated

c)

supersaturated

38.

Which of the following best describes a supersaturated solution?

a)

a solution that contains the maximum amount of solute that is capable of being dissolved

b)

a solution that contains less than the maximum amount of solute that is capable of being dissolved.

c)

a solution that contains more than the maximum amount of solute that is capable of being dissolved.

d)

none of the above

39.

A solution with less than the maximum amount of solute completely dissolved.

a)

Saturated solution

b)

Unsaturated solution

c)

Supersaturated solution

40.

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

41.

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

42.

As we dilute a solution.....

a)

The volume increases and the molarity (M) increases

b)

The volume increases and the molarity (M) decreases

c)

The volume decreases and the molarity (M) increases

d)

The volume decreases and the molarity (M) decreases

43.

50 ml of a 1 M solution is diluted until the final volume is 80ml. How much water was added?

a)

50 ml

b)

1.3 ml

c)

30 ml

d)

130 ml

44.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250 mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
45.
What is the molarity of a solution made by adding 1.565 moles of PbNO3 to 500 mL?
a)
300. M
b)
31.3 M
c)
3.13 M
d)
1.56 M
46.

In writing the chemical equation for a reaction that produces a precipitate, what abbreviation of the physical state must appear with one of the products?

a)

(s)

b)

(g)

c)

(l)

d)

(w)

47.

What would be the formula of the precipitate that forms when Pb(NO3)2 (aq) and K2SO4 (aq) are mixed?

a)

K(NO3)2

b)

PbSO4

c)

PbK2

d)

H2O

48.
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)
49.
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) →
50.
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-
51.

What is the net ionic equation for the reaction between K3PO4 (aq) and CuSO4 (aq) that produces K2SO4 (aq) and Cu3(PO4)2 (s)?

a)

2 K+(aq) + SO42-(aq) → K2SO4 (s)

b)

K+(aq) + SO42-(aq) → KSO4 (s)

c)

2 Cu2+(aq) + 3 PO43-(aq) → Cu3(PO4)2 (s)

d)

Cu2+(aq) + PO43-(aq) → CuPO4 (s)

52.
What is the NAME of....
Na2S
a)
sodium (II) sulfide
b)
sodium sulfide
c)
disodium sulfide
d)
sodium sulfur
53.

Name this compound: KF

a)

Potassium fluoride

b)

Potassium fluorite

c)

Fluorine potasside

d)

Potassium fluorate

54.
What is the FORMULA for...
calcium arsenide
a)
Ca3As2
b)
CaAs2
c)
Ca3As
d)
Ca3Ar2
55.

ammonium phosphate

a)

(NH4)3PO4

b)

NPO4

c)

NH4PO4

d)

NH4(PO4)3

56.

What is the formula for manganese(III) oxide?

a)

MnO

b)

MnO3

c)

Mn3O

d)

Mn2O3

57.

What is the correct chemical name for Cu2O ?

a)

Copper oxide

b)

Copper oxalate

c)

Copper (II) oxide

d)

Copper (I) oxide

58.

Which of the following equations is Nickel (II) nitrite ?

a)

Ni2NO2

b)

Ni(NO2)2

c)

Ni(NO3)2

d)

Ni3N2

59.

What is the name of the following ternary ionic compound:

NaMnO4 ?

a)

Sodium Permangante

b)

Sulfur Permanganate

c)

Sodium Manganese Oxide

60.

What is the name of the following ternary ionic compound:

Zn3(PO4)2?

a)

Zinc Phosphate

b)

Zinc Phosphite

c)

Zinc Phosphide

61.

What is the name of the following ternary ionic compound:

KClO4?

a)

Potassium perchlorate

b)

Phosphorus perchlorate

c)

Potassium Chlorine Oxide

62.

What is the name of the following ternary ionic compound:

AgCN?

a)

Silver Cyanide

b)

Silver Carbon Nitride

c)

Silver Carbonoxide

63.

What is the name of the following ternary ionic compound:

NiNO3?

a)

Nickel Nitrate

b)

Nickel Nitrite

c)

Nickel nitogen oxide

64.

What is the name of the following ternary ionic compound:

Al2(SO3)3

a)

Aluminum Sulfite

b)

Aluminum sulfate

c)

aluminum sulfur oxide

65.

What is the name of the following ternary ionic compound:

Ba(OH)2 ?

a)

Barium Hydroxide

b)

Boron Hydroxide

c)

Beryllium Hydroxide

66.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
67.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
68.
From the following ionic compounds, choose the name-formula pair that is not correctly matched.
a)
sodium sulfide  Na2S
b)
ammonium nitrate 
NH4NO3
c)
sodium sulfate 
Na2SO3
d)
calcium oxide  CaO
69.

Name the following ionic compound: MgSO4

a)

magnesium sulfoxide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium oxide

70.
Name the following ionic compound: Cr(NO2)3
a)
chromium nitrite
b)
chromium nitride
c)
chromium III nitride
d)
chromium III nitrite
71.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
72.
The chemical formula of Iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
73.
The chemical compound for sodium phosphate would be:
a)
NaPO4
b)
Na2PO4
c)
Na3PO4
d)
Na(PO4)3
74.

Ammonium chloride

a)

NHCl4

b)

NH4Cl

c)

NHCl

d)

ACl

75.

Lead II Nitrate

a)

PbNO3

b)

Pb(NO3)2

c)

Pb2NO3

d)

LN

76.

Rubidium Chromate

a)

RbCrO4

b)

RbCr2

c)

Rb2CrO4

d)

Rb(CrO4)2

77.

Calcium Nitrite

a)

CaNO2

b)

CaNO3

c)

Ca(NO2)2

d)

Ca(NO3)2

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