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ANALYTICAL CHEMISTRY PRACTICE EXAM_WEEK 4

Total questions: 60

Worksheet time: 1hrs 20mins

Name
Class
Date
1.

Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from  6 moles H2? 

a)

4 moles Fe

b)

6 moles Fe

c)

9 moles Fe

d)

2 moles Fe

2.

How many liters of carbon dioxide at STP are produced from 10.0 L of carbon monoxide at STP?

a)

10.0 L

b)

20.0 L

c)

5010 L

d)

0.0199

3.
Using the balanced equation in question 1,
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
What is the mass in grams of H₂ gas when 4.0 moles of HCl is added to the reaction?
a)
0.99 g
b)
4.0 g
c)
2.0 g
d)
6.0 g
4.
Balance the following reaction:
Mg(s)   +   HCl(aq)  -->   MgCl₂(aq)   +   H₂(g)
a)
1,2,1,2
b)
2,1,1,2
c)
1,2,1,1
d)
1,2,2,2
5.

Convert 175 K to °C.

a)

-98°C

b)

-100°C

c)

-95°C

d)

-97°C

6.

Convert 25°F to °C.

a)

-3.9°C

b)

-4°C

c)

-3.8°C

d)

-3.7°C

7.

1 tbsp = ___ tsp

a)

2

b)

3

c)

4

d)

5

8.

A truck weighs 60,000 pounds. How many short tons does it weigh?

a)

600 tons

b)

300 tons

c)

80 tons

d)

30 tons

9.

What is the first stage of the two-stage two-dimensional PAGE?

a)

SDS-PAGE

b)

HPLC

c)

Isoelectric focusing

d)

Sedimentation

10.

What would the conjugate base of HCO3- be?

a)

H2CO3

b)

CO32-

c)

H2CO3-

d)

CO3-

11.

Which acid/base definitions classify acids as donating protons and bases accepting protons?

a)

Arrhenius

b)

Brønsted-Lowry

c)

Lewis

d)

Hall-Higgins

12.

When an acid and a base are mixed, what is the reaction called?

a)

Neutralization

b)

Hydrolyzed

c)

Hydro Ionization

d)

A salt and a water reaction

13.

What is the molality of a solution made by dissolving 2 moles of NaOH in 400 grams of water?

a)

a. 5 mol/kg. solvent

b)

b. 4 mol/kg solvent

c)

c. 3 mol/kg. solvent

d)

d. 2.5 moles /kg solvent

14.

Molar mass of NaOH is ______________________

Correct

a)

a. 40 grams/mol

b)

b. 50 grams/mol

c)

c. 45 grams/mol

d)

d. 38 grams/mol

15.

Choose the correct definition of a primary standard solution/reference standard solution

a)

substances that are stable chemical compounds and available in high purity

b)

substances that are stable chemical compounds and contain high moisture

c)

substances that are volatile chemical compounds and available in high purity

d)

substances that are volatile chemical compounds and available in high moisture

16.

What do we determine using volumetric analysis?

a)

Amount

b)

Concentration

c)

Density

d)

Solubility

17.

FIND THE NORMALITY OF 0.4 M Ba(OH)2

a)

a. 0.5 N

b)

b. 0.2 N

c)

c. 0.8 N

d)

d. 4 N

18.

Find the NORMALITY OF 1.4 M H2SO4

a)

a. 2.8 N

b)

b. 1.4 N

c)

c. 2.2 N

d)

d. 0.14 N

19.

Find the normality of 0.15M HCl

a)

a. 0.015 N

b)

b. 0.15N

c)

c. 15N

.

d)

d. 1.5N

20.
What is the molarity in 650. ml of solution containing 63 grams of sodium chloride?
a)
2.4 M
b)
0.86 M
c)
1.7 M
d)
0.54 M
21.
What is the molarity of 4 grams of sodium chloride in 3,800 mL of solution?
a)
0.018 M
b)
0.018 mol
c)
1.052 M
d)
1.052 mol
22.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
23.

Molality (m) = moles of solute / _________________________.

a)

kilogram of solvent

b)

kiloliter of solvent

c)

kilometer of solvent

d)

ounces of solvent

24.

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

25.

What is a benefit of sending specimens to a reference laboratory?

a)

a) Reduced turnaround times for test results

b)

b) Increased availability of specialized tests

c)

c) Higher quality analysis of patient specimens

d)

d) Lower cost per test due to high test volume

26.

The glassware used to determine the Specific Gravity of a liquid.

a)

thermometer

b)

stirring rod

c)

Pycnometer

d)

column

27.

What do you call to the procedure for preparing a less concentrated

solution from a more concentrated one?

a)

quantitative analysis

b)

dilution

c)

redox titration

d)

gravametric analysis

28.

What are the concentrated solutions stored in the

laboratory stockroom for use as needed?

a)

phenolphthalein

b)

indicators

c)

stock solution

d)

aliquot

29.
How many moles of propane gas are in a 7.0 L tank at 20°C and 5.45atm of pressure?
a)
0.629 mol
b)
1.59 mol
c)
23.2 mol
d)
917 mol
30.

3. Which pertains to materials that are toxic and may cause pollution?

a)

Useful

b)

Harmful

c)

Dangerous

d)

Pathogenic

31.

Type of Chemical with high degree of purity suitable for use in most analytical procedures

a)

Analytical Reagent Grade

b)

Ultrapure Grades

c)

Chemically Pure Grade

d)

United States Pharmacopeia

32.

How many electrons is needed to transform Fe2+ ion to solid state?

a)

1

b)

2

c)

3

d)

4

33.

Which of the following statement is false

a)

flow of ions takes place in both direction

b)

conductivity of electrolyte is generally low

c)

electrolysis involves physical changes

d)

flow of electrons is unidirectional

34.

Which of the following substances would conduct electricity if dissolved in water to form a solution?

a)

C6H12O6

b)

CH4

c)

KI

d)

CO2

35.
Which property of matter is determined by dividing its mass by its volume?
a)
elasticity
b)
buoyancy
c)
density
d)
viscosity
36.

Which of these materials is least useful as an insulator?

a)

Cardboard

b)

Aluminum

c)

Rubber

d)

Plastic

37.

Which of the following are good properties when choosing a precipitating reagent? Check all that applies.

a)

easily filtered for contaminants

b)

reactive to constituents of the atmosphere

c)

composition is unknown after dried

d)

its solubility is low

38.

What is the main component int the ICP-MS that cannot be found in ICP-OES?

(a)  

39.

Which of the following is the atomic emission spectroscopy methods?

a)

Graphite Furnace Atomic Emission Spectroscopy

b)

Inductively Couple Plasma- Optical Emission Spectroscopy

c)

Flame Atomic Emission Spectroscopy

d)

Hydride Generation Atomic Emission Spectroscopy

40.

Flame photometer is quite similar to UV-Visible but what is the major difference between these 2 methods?

a)

Detector

b)

Source of light

c)

Monochomator

d)

Data processor

41.

What is E waste?

a)

Electro Magnetic Waste

b)

Electronic Waste

c)

Economy Waste

d)

Environmental Waste

42.

Which of the following is the most preferred in waste management hierarchy?

a)

Disposal

b)

Recovery

c)

Prevention

d)

Reduction

43.

What does the term PPE mean?

a)

Perfect Parameters of Experiment

b)

Personal Protective Equipment

c)

Please Participate in Experiment

d)

Pouring Pleasantly and Equitably

44.

Which of the following is the best fire extinguisher to use in electrical equipments?

a)

Water

b)

Foam

c)

Dry chemical

d)

Carbon Dioxide

45.

What is the formula for: silver oxide

a)

AgO2

b)

AgO

c)

Ag2O

d)

SiO2

46.

The red numbers in the image below represent ________

a)

subscripts

b)

coefficients

c)

Number of molecules

d)

Molecular weight

47.

What is the correct name for CCl4?

a)

carbon tetrachloride

b)

monocarbon tetrachloride

c)

tetracarbon monochloride

d)

carbon chloride

48.

When naming compounds, how can you tell it is a polyatomic compound?

a)

There is a H in the front of the formula

b)

There are more than 2 elements in the formula

c)

The elements are on left and right hand side of the periodic table

d)

The elements are in the middle and right hand side of the periodic table

e)

The elements are on the right hand side of the periodic table

49.

When writing chemical formulas, how do you know it is a molecular compound?

a)

The elements are on the left and right hand sides of the periodic table

b)

Its name ends in

-ate or -ite

c)

The name contains prefixes

d)

Its name ends in -ide

e)

The elements are on the right hand side of the periodic table

50.

When writing chemical formulas, how do you know it is a multivalent ionic compound?

a)

The word acid is in its name

b)

Its name ends in

-ate or -ite

c)

Its name has roman numerals

d)

Its name ends in

-ide

51.

When writing chemical formulas, how do you know it is a polyatomic compound?

a)

The word acid is in its name

b)

Its name ends in

-ate or -ite

c)

Its name has roman numerals

d)

Its name ends in

-ide

52.

What is the formula for: potassium fluoride

a)

KF

b)

KFl

c)

K2F2

d)

K2F

53.

What is the formula for: aluminum phosphide

a)

AlP

b)

AlP3

c)

Al3P3

d)

Al3P2

54.

Which situation best demonstrates the difference between a compound and a mixture?

a)

Mixing salt and pepper in a container

b)

Dissolving sugar in water

c)

Reacting hydrogen with oxygen to form water

d)

Stirring sand and iron filings

55.

What chemical will be formed from the combination of a hydrogen ion (H+) and a hydroxide ion (OH-)?

a)

Hydrogen Peroxide

b)

Table Salt

c)

Table Sugar

d)

Water

56.

Which group of the periodic table is composed of inert (not reactive)  gases?

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

57.

What is the difference between Co and CO?

a)

CO is an element but Co is a compound

b)

Nothing is different. They are the same thing.

c)

CO is two elements and Co is only one element

d)

Co is not a pure substance

58.

An important benefit of implementing a HACCP system in a food business is

a)

reduced employee wages

b)

increased consumer confidence

c)

reduced employer support

d)

increased food wastage

59.

What is the primary focus of Quality Control (QC)?

a)

Preventing defects in processes

b)

Developing training programs

c)

Improving customer satisfaction

d)

Identifying and fixing defects in products

60.

When NaOH solution is added to Zinc Nitrate solution

a)

Chalky White ppt formed

b)

Gelatinous White ppt formed

c)

Dirty Green ppt formed

d)

Reddish-brown ppt formed

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