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WEEK 3 QUIZ ENCHEM1L

Total questions: 50

Worksheet time: 1hrs 24mins

Name
Class
Date
1.

What does the unit Liters, L, measure?

a)

Volume

b)

Pressure

c)

Temperature

d)

Moles

2.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
3.

Which of the following is the Dilution Formula?

a)

V1M1 = V2M2

b)

M = m/V

c)

V = mT

d)

PV = nRT

4.

A dilution is when

a)

solute is added to the volume of solution

b)

water is added to the volume of solution

c)

solute is removed from the volume of solution

d)

water is removed from the volume of solution

5.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

60.0 mL

c)

100 mL

d)

125 mL

6.

What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250.0 mL?

a)

15.9 M

b)

0.636 M

c)

0.642 M

d)

1.59 M

7.
How many mL of 10.8M HCl are required to make 100.0 mL of 3.00M acid?
a)
27.8 mL
b)
27.78 mL
c)
2.8 mL
d)
278 mL
8.

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

9.

Which of the following will produce crystals if cooled or disturbed?

a)

unsaturated solution

b)

saturated solution

c)

supersaturated solution

d)

all of the above

10.
How many grams of solute are dissolved in 125.0 mL of 5.00M NaCl?
a)
0.625 g NaCl
b)
36.52 g NaCl
c)
36.5 g NaCl
d)
0.625 mol NaCl
11.
What does it mean if a mixture is homogeneous?
a)
you can see the different parts
b)
cannot tell one part from another
c)
chunks of particles
d)
made of elements
12.
Solvent is best defined as-
a)
a mixture in which the substances are spread out evenly between one another and cannot be told apart
b)
the ability of a substance to dissolve in another substance
c)
a substance that dissolves in another substance
d)
a substance into which another substance dissolves
13.
When two liquids mix, they are said to be....
a)
insoluble
b)
miscible
c)
soluble
d)
immiscible
14.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
15.
What is the concentration, in percent by volume, of 15.3 mL of solute in 2.65 L of solution?
a)
0.58%
b)
0.0058%
c)
5.8%
16.
What mass of solute is needed to make 75.0 g of a 3.4% solution?
a)
2.55 g
b)
22 g
c)
0.05 g
17.
What is the volume of solution needed to make a 3.5% by volume solution using 2.0mL of solvent?
a)
57 mL
b)
0.57 mL
c)
7 mL
18.
What is the mole fraction of MgF2 in a solution  that has 0.321 mol of MgF2 dissolved in 4.44 mol of water?
a)
0.0674
b)
0.0722
c)
1.425
19.
What is the mole fraction of ethanol when 0.504 mol of ethanol are mixed with 4.06 mol of water?
a)
0.110
b)
0.124
c)
0.097
20.
The amount of solute actually dissolved in a given amount of solvent.
a)
dilution
b)
concentration
c)
saturated solution
d)
supersaturated mixture
21.
When a solvent contains as much of the solute as it can hold, the solution is said to be
a)
supersaturated
b)
diluted
c)
saturated
d)
unsaturated
22.
How does a solution become supersaturated?
a)
dissolve lots of solute in it.
b)
dissolve a little solute in it. 
c)
dissolve more solute than you should be able to. 
d)
dissolve a super amount of solvent in it. 
23.

What is the molality (not molarity) of a solution when 500g water are used to dissolve 21g CuSO4?

a)

0.3 m

b)

3.4 m

c)

1.6 m

d)

0.8 m

24.

separates solid components of a mixture that are too small for decantation with the use of a filter

a)

MAGNETIC SEPARATION

b)

MANUAL PICKING

c)

DECANTATION

d)

SIEVING

e)

FILTERING

25.

separates soluble solids in a solution by evaporating the liquid component leaving the solid component behind

a)

EVAPORATION

b)

DISTILLATION

c)

FRACTIONAL DISTILLATION

d)

SIEVING

e)

FILTERING

26.

What seperation process is this?

a)

Evaporation

b)

Distillation

c)

Filtration

d)

Condensation

27.

To separate a mixture of salt and water what separation method is used?

a)

Filtration

b)

Distillation

c)

Chromatography

d)

Evaporation to dryness

28.
Air
a)
Heterogeneous
b)
Homogeneous
29.
Soil
a)
Heterogeneous
b)
Homogeneous
30.
Vinegar
a)
Heterogeneous
b)
Homogeneous
31.
Sugar water
a)
Heterogeneous
b)
Homogeneous
32.
Sugar water is a 
a)
solution
b)
suspension
c)
colloid
33.

What are the common sources of error in laboratory techniques?

a)

inadequate quality control, improper storage, experimental design flaws, measurement errors

b)

human error, equipment malfunction, contamination, improper calibration, systematic errors

c)

improper documentation, environmental factors, incorrect measurements, personal bias

d)

lack of training, outdated equipment, insufficient sample size, random errors

34.

How can a student ensure accurate data analysis in a laboratory experiment?

a)

Use outdated equipment and materials.

b)

Skip the data collection step.

c)

Ignore any unexpected results.

d)

Follow proper experimental procedures and protocols.

35.

Dyes in water soluble markers may be separated by means of

a)

Simple distillation

b)

Crystallisation

c)

Chromatography

d)

Filtration

36.

Charcoal powder is insoluble in water. When water is filtered, the charcoal powder becomes the _______.

a)

solute

b)

residue

c)

filtrate

d)

solvent

37.

Which of the following statements is NOT true about the image?

a)

The process is called filtration.

b)

A process known as sedimentation is important to make the separation possible.

c)

The substance that passes through the filter paper is called the filtrate.

d)

This method is used to separate insoluble solids from liquids.

38.

When is manual separation applicable?

a)

When the particles of the mixture are large enough to be seen clearly.

b)

When the solutes in the mixture are totally dissolved by the solvent.

c)

Only colloidal mixtures can be separated manually.

d)

When the mixture is exposed to heat.

39.

The image shows a mixture of concrete nails and saw dusts. What technique is best to use to separate the nails from the saw dusts?

a)

sieving

b)

chromatography

c)

decantation

d)

magnetic separation

40.

Which of the following techniques is used to separate the components of a solution?

a)

filtration

b)

decantation

c)

evaporation

d)

physical manipulation

41.

A solution with a large amount of solute is called _________

a)

dilute

b)

saturated

c)

concentrated

d)

homogeneous

42.

A solution with only  a small amount  of solute is called a ______ solution.

a)

dilute

b)

saturated

c)

concentrated

d)

homogeneous

43.

If a solution is prepared from 5g NaCl in enough water to make a 120mL solution, the mass-volume concentration is:

a)

0.04%

b)

4.2%

c)

24%

d)

6.7%

44.

If a solution is made by taking 70 mL of ethanol and adding enough water to make 750 mL of solution, the percent volume is:

a)

9.3%

b)

10.7%

c)

0.09%

d)

70%

45.

Which formula will you use for a problem looking for concentration by volume of ethanol in a solution?

a)

volume of solutevolume of solutionx100\frac{volume\ of\ solute}{volume\ of\ solution}x100  

b)

mass of solutemass of solutionx100\frac{mass\ of\ solute}{mass\ of\ solution}x100  

c)

mass of solutevolume of solutionx100\frac{mass\ of\ solute}{volume\ of\ solution}x100  

d)

C=mvC=\frac{m}{v}  

46.

A 20g tube of cream contains 1.2% (w/w) of active ingredient. What is the mass of the active ingredient does the cream contain?

a)

0.24%

b)

2.4%

c)

0.94%

d)

9.4%

47.

What variable is represented by mole fraction?

a)

M

b)

m

c)

X

d)

ppm

48.

What volume of isopropyl alcohol is used to make 350 mL of 70 % rubbing alcohol?

a)

245 g

b)

350 g

c)

100 g

d)

250 g

49.

What mass of solute is needed to make 100 g of 3.4% solution?

a)

0.34 g

b)

3.4 g

c)

34 g

d)

0.034 g

50.

It is defined as the ratio of the mass of the solute to the mass of the solution.

a)

mole fraction

b)

percent by volume

c)

percent by mass

d)

ppm

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