Analytical Chemistry Exam Bank - 3504 Verified Questions

Analytical Chemistry Exam Bank

Course Introduction

Analytical Chemistry is a branch of chemistry focused on the qualitative and quantitative determination of the chemical components of substances. This course introduces students to classical and modern analytical techniques, including gravimetric, titrimetric, spectroscopic, and chromatographic methods. Emphasis is placed on sampling, data analysis, error minimization, and the interpretation of results. Laboratory sessions provide hands-on experience in applying these techniques to real-world samples, preparing students for roles in research, quality control, and regulatory environments.

Recommended Textbook

Chemistry The Central Science 12th Edition by Theodore E. Brown

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24 Chapters

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Page 2

Chapter 1: Introduction: Matter and Measurement

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Sample Questions

Q1) The volume of a regular cylinder is V = r²h. Using the value 3.1416 for the constant , the volume (cm³)of a cylinder of radius 2.34 cm and height 19.91 cm expressed to the correct number of significant figures is __________.

A)342.49471

B)342.495

C)342.49

D)343

E)342

Answer: E

Q2) There are __________ ng in a pg.

A)0.001

B)1000

C)0.01

D)100

E)10

Answer: A

Q3) 1 milligram = __________ micrograms

Answer: 1,000

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3

Chapter 2: Atoms, Molecules, and Ions

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Sample Questions

Q1) The formula for zinc phosphate is Zn₃(PO₄)₂.

What is the formula for cadmium arsenate?

A)Cd₄ (AsO₂)₃

B)Cd₃ (AsO₄)₂

C)Cd₃ (AsO₃)₄

D)Cd₂ (AsO₄)₃

E)Cd₂ (AsO₄)₄

Answer: B

Q2) Oxygen forms an ion with a charge of __________.

A)2-

B)2+

C)3-

D)3+

E)6+

Answer: A

Q3) The formula for potassium sulfide is __________.

Answer: K₂S

Q4) What is the name of an alcohol derived from hexane?

Answer: hexanol

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Chapter 3: Stoichiometry: Calculations With Chemical

Formulas and Equations

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Sample Questions

Q1) Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO₃ are produced by the reaction of 5.0 grams of O₂ with 6.0 grams of S. What is the % yield of SO₃ in this experiment? S (s)+ O₂ (g) SO₃ (g)(not balanced)

A)32

B)63

C)75

D)95

E)99

Answer: D

Q2) When a hydrocarbon burns in air, what component of air reacts?

A)oxygen

B)nitrogen

C)carbon dioxide

D)water

E)argon

Answer: A

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Chapter 4: Aqueous Reactions and Solution Stoichiometry

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Q1) One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

A)zinc

B)cobalt

C)lead

D)copper

E)none of these

Q2) What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H₂SO₄ solution is required to neutralize a 25.0-mL sample of the NaOH solution?

A)0.801

B)0.315

C)0.629

D)125

E)0.400

Q3) The solvent in an aqueous solution is __________.

Q4) How many grams of H₃PO₄ are in 265 mL of a 1.50 M solution of H₃PO₄?

Q5) What is aqua regia?

Page 6

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Chapter 5: Thermochemistry

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Sample Questions

Q1) Petroleum is a liquid composed of hundreds of compounds.

A)True

B)False

Q2) For which one of the following reactions is the value of H°_rxn equal to H°_f for the product?

A)H₂ (g)+ 1/2 O₂ (g) H₂O (l)

B)H₂ (g)+ O₂ (g) H₂O₂ (l)

C)2 C (s, graphite)+ 2 H₂ (g) C₂H₄ (g)

D)1/2 N₂ (g)+ O₂ (g) NO₂ (g)

E)all of the above

Q3) The average fuel value of sugars is 17 kJ/g. A 2.0 L pitcher of sweetened Kool-Aid contains 400 g of sugar. What is the fuel value (in kJ)of a 500 mL serving of Kool-Aid? (Assume that the sugar is the only fuel source.)

A)4.2 × 10⁴

B)1.7 × 10³

C)1.7 × 10⁶

D)1.7 × 10²

E)17

Q4) __________ is defined as the energy used to move an object against a force.

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Chapter 6: Electronic Structure of Atoms

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Sample Questions

Q1) [Ne] 3s²3p³ is the electron configuration of a(n)__________ atom.

A)As

B)V

C)P

D)Sb

E)Sn

Q2) The __________ subshell contains only one orbital.

A)5d

B)6f

C)4s

D)3d

E)1p

Q3) An electron cannot have the quantum numbers n = __________, l = __________, m_l = __________.

A)2, 0, 0

B)2, 1, -1

C)3, 1, -1

D)1, 1, 1

E)3, 2, 1

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Chapter 7: Periodic Properties of the Elements

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Sample Questions

Q1) The effective nuclear charge acting on an electron is larger than the actual nuclear charge.

A)True

B)False

Q2) Which equation correctly represents the first ionization of phosphorus?

A)P (g)+ e^- P^- (g)

B)P (g) P^- (g)+ e^-

C)P (g) P⁺ (g)+ e^-

D)P^- (g) P (g)+ e^-

E)P⁺ (g)+ e^- P (g)

Q3) Of the following statements, __________ is not true for oxygen.

A)The most stable allotrope of oxygen is O₂.

B)The chemical formula of ozone is O₃.

C)Dry air is about 79% oxygen.

D)Oxygen forms peroxide and superoxide anions.

E)Oxygen is a colorless gas at room temperature.

Q4) As successive electrons are removed from an element, the ionization energy __________.

Q5) [Kr]5s² is the electron configuration for __________.

Q6) All of the group VIA elements are solids except __________.

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Chapter 8: Basic Concepts of Chemical Bonding

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Sample Questions

Q1) There are __________ valence electrons in the Lewis structure of CH₃CH₂Cl.

A)14

B)12

C)18

D)20

E)10

Q2) The chloride of which of the following metals should have the greatest lattice energy?

A)potassium

B)rubidium

C)sodium

D)lithium

E)cesium

Q3) Based on the octet rule, magnesium most likely forms a __________ ion.

A)Mg²⁺

B)Mg²^-

C)Mg^6-

D)Mg⁶⁺

E)Mg^-

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Chapter 9: Molecular Geometry and Bonding Theories

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Sample Questions

Q1) For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity?

A)1

B)2

C)1 or 2

D)3

E)1 or 3

Q2) Using the VSEPR model, the electron-domain geometry of the central atom in SF₄ is __________.

A)linear

B)trigonal planar

C)tetrahedral

D)trigonal bipyramidal

E)octahedral

Q3) What are the three bond angles in the trigonal bipyramidal structure?

Q4) XeF₄ is a polar molecule.

A)True

B)False

Q5) In molecular orbital theory the stability of a covalent body is related to its

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Chapter 10: Gases

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Sample Questions

Q1) Calcium hydride (CaH₂)reacts with water to form hydrogen gas: CaH₂ (s)+ 2H₂O (l) Ca(OH)₂ (aq)+ 2H₂ (g)

How many grams of CaH₂ are needed to generate 48.0 L of H₂ gas at a pressure of 0.888 atm and a temperature of 32°C?

A)50.7

B)0.851

C)143

D)35.8

E)71.7

Q2) 30.0 grams of argon and 15.0 grams of xenon are placed in a 120.0 ml container at 22.0°C. The partial pressure of xenon is __________ atm.

A)8.70

B)22.9

C)0.700

D)174

E)5.60

Q3) What is the density (in g/L)of oxygen gas at 77.0°C and 700.0 torr?

Q4) The rms speed of methane molecules at 45.0°C is __________ m/sec.

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Chapter 11: Liquids and Intermolecular Forces

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Sample Questions

Q1) The vapor pressure of any substance at its normal boiling point is

A)1 Pa

B)1 torr

C)1 atm

D)equal to atmospheric pressure

E)equal to the vapor pressure of water

Q2) In general, the vapor pressure of a substance increases as __________ increases.

A)surface tension

B)molecular weight

C)hydrogen bonding

D)viscosity

E)temperature

Q3) What types of intermolecular forces exist between PH₃ and N₂?

A)dispersion forces and dipole-dipole forces

B)dispersion forces and dipole-induced dipole forces

C)dispersion forces and hydrogen bonds

D)dispersion forces, hydrogen bonds, and induced dipole-induced dipole forces

E)dispersion forces, hydrogen bonds, and dipole-induced dipole forces

Q4) The direct conversion of a solid to a gas is called __________.

Page 13

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Chapter 12: Solids and Modern Materials

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Sample Questions

Q1) Alloys generally differ from compounds in that

A)the former always contain some carbon.

B)the former always contain some iron.

C)the former always have semiconductor properties.

D)the atomic ratios of the constituent elements in the former are not fixed and may vary over a wide range.

E)the former never contain a transition element.

Q2) __________ are solid-state materials that can be made either semiconducting or metallic without any doping.

Q3) Which one of the following is an addition polymer with the same structure as polyethylene except that one hydrogen on every other carbon is replaced by a benzene ring?

A)polyvinyl chloride

B)polypropylene

C)polystyrene

D)polyurethane

E)nylon 6, 6

Q4) When lattice points occur only at the corners of a unit cell, the cell is called

Q5) Nylon is formed by the reaction of a __________ with a __________.

Page 14

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Chapter 13: Properties of Solutions

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Sample Questions

Q1) The freezing point of ethanol (C₂H₅OH)is -114.6°C. The molal freezing point depression constant for ethanol is 2.00°C/m. What is the freezing point (°C)of a solution prepared by dissolving 40.0 g of glycerin (C₃H₈O₃, a nonelectrolyte)in 200.0 g of ethanol?

A)-115.0

B)-4.34

C)-132.3

D)-118.9

E)-114.6

Q2) At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density of 1.0344 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g/mol.

A)2.55

B)0.0449

C)2.32

D)0.446

E)12.00

Q3) The formula weight of FeCl₃^.6H₂O is

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Page 15

Chapter 14: Chemical Kinetics

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Sample Questions

Q1) Of the following, all are valid units for a reaction rate except __________.

A)mol/L

B)M/s

C)mol/hr

D)g/s

E)mol/L-hr

Q2) The average rate disappearance of A between 20 s and 30 s is __________ mol/s.

A)5.0 × 10^-4

B)1.6 × 10^-2

C)1.5 × 10^-3

D)670

E)0.15

Q3) What is the order of the reaction with respect to OH^-?

A)0

B)1

C)2

D)3

E)4

Q4) The uptake of molecules into the interior of another substance is referred to as

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Chapter 15: Chemical Equilibrium

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Sample Questions

Q1) In what year was Fritz Haber awarded the Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen?

A)1954

B)1933

C)1918

D)1900

E)1912

Q2) If Reaction A + Reaction B = Reaction C, then K_cReaction C =

Q3) Which one of the following is true concerning the Haber process?

A)It is a process used for shifting equilibrium positions to the right for more economical chemical synthesis of a variety of substances.

B)It is a process used for the synthesis of ammonia.

C)It is another way of stating Le Châtelier's principle.

D)It is an industrial synthesis of sodium chloride that was discovered by Karl Haber.

E)It is a process for the synthesis of elemental chlorine.

Q4) Pure __________ and pure __________ are excluded from equilibrium-constant expressions.

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Chapter 16: Acid-Base Equilibria

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Sample Questions

Q1) The pH of an aqueous solution at 25.0 °C is 10.30. What is the molarity of H⁺ in this solution?

A)5.0 × 10^-11

B)2.0 × 10^-4

C)3.70

D)1.0 × 10^-13

E)2.0 × 10¹⁰

Q2) The pH of a 0.15 M aqueous solution of NaZ (the sodium salt of HZ)is 10.7. What is the K_a for HZ?

A)1.6 × 10^-6

B)6.0 × 10^-9

C)8.9 × 10^-4

D)1.3 × 10^-12

E)3.3 × 10^-8

Q3) Of the following, which is the weakest acid?

A)HIO

B)HIO₄

C)HIO₂

D)HIO₃

E)The acid strength of all of the above is the same.

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Chapter 17: Additional Aspects of Aqueous Equilibria

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Q1) How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M butanoic acid to the equivalence point? The K_a of butanoic acid is 1.5 × 10^-5.

A)4.90

E)4.65

Q2) A solution is prepared by dissolving 0.23 mol of hydrofluoric acid and 0.27 mol of sodium fluoride in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the __________ present in the buffer solution. The K_a of hydrofluoric acid is 1.36 × 10^-3.

A)H₂O

B)H₃O⁺

C)fluoride ion

D)hydrofluoric acid

E)This is a buffer solution: the pH does not change upon addition of acid or base.

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Chapter 18: Chemistry of the Environment

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Q1) Compounds found in fossil fuels that contain __________ are primarily responsible for acid rain.

A)sulfur

B)carbon

C)hydrogen

D)phosphorus

E)neon

Q2) The dissociation energy of the C-Cl bond in CF₃Cl is 339 kJ/mol. The maximum wavelength of light that has enough energy per photon to dissociate the C-Cl bond is __________ nm.

A)1130

B)3.53 × 10^-4

C)3.53 × 10^-7

D)3.53 × 10⁵

E)353

Q3) The salinity, density, and temperature of seawater varies with __________.

Q4) The production of dead and decaying plant material is a process called

Q5) How can the presence of biodegradable waste in a lake result in the death of fish in the lake?

Page 20

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Chapter 19: Chemical Thermodynamics

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Q1) A reversible change produces the maximum amount of ________ that can be achieved by the system on the surroundings.

Q2) S is negative for the reaction __________.

A)2H₂O (g) 2H₂(g)+ O₂ (g)

B)Mg(NO₃)₂ (aq)+ 2NaOH(aq) Mg(OH)₂ (s)+ 2NaNO₃ (aq)

C)H₂O (l) H₂O (g)

D)C₆H₁₂O₆ (s) 6C (s)+ 6H₂ (g)+ 3O₂ (g)

E)NaCl (aq) Na⁺ (aq)+ Cl^- (aq)

Q3) The standard Gibbs free energy of formation of __________ is zero. (a)Si (s) (b)F₂ (g)

(c)Ni (s)

A)(a)only

B)(b)only

C)(c)only

D)(b)and (c)

E)(a), (b), and (c)

Q4) Calculate G° for the autoionization of water at 25°C. K_w = 1.0 × 10^-14

Page 21

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Chapter 20: Electrochemistry

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Q1) The standard cell potential (E°_cell)for the voltaic cell based on the reaction below is __________ V. Sn²⁺ (aq)+ 2Fe³⁺ (aq) 2Fe²⁺ (aq)+ Sn⁴⁺ (aq)

A)+0.46

B)+0.617

C)+1.39

D)-0.46

E)+1.21

Q2) The balanced half-reaction in which sulfate ion is reduced to sulfite ion is a __________ process.

A)four-electron

B)one-electron

C)two-electron

D)three-electron

E)six-electron

Q3) The standard reduction potential of X is 1.23 V and that of Y is -0.44 V therefore X is oxidized by Y.

A)True

B)False

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Chapter 21: Nuclear Chemistry

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Q1) Carbon-11 is used in medical imaging. The half-life of this radioisotope is 20.4 min. What percentage of a sample remains after 60.0 min?

A)71.2

B)5.28

C)13.0

D)34.0

E)2.94

Q2) Who is credited with first achieving fission of uranium-235?

A)Fermi

B)Rutherford

C)Curie

D)Dalton

E)Faraday

Q3) Radioactive seeds that are implanted into a tumor are coated with __________ to stop alpha and beta ray penetration.

Q4) The SI unit of an absorbed dose of radiation is the gray.

A)True

B)False

Q5) What happens in the nucleus of an atom that undergoes positron emission?

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Chapter 22: Chemistry of the Nonmetals

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Q1) Which group 6A element is not commonly found in a positive oxidation state?

A)sulfur

B)selenium

C)oxygen

D)tellurium

E)polonium

Q2) Boron can violate the octet rule in its compounds in that

A)it can have an expanded octet.

B)it can exist in a molecule with an odd number of electrons.

C)its compounds are all ionic.

D)it can have fewer than eight valence electrons.

E)boron cannot violate the octet rule.

Q3) Chains of silicate tetrahedra are called __________.

Q4) Which of the following would produce the most strongly acidic aqueous solution?

A)HCO₃^-

B)CO

C)CO₂

D)CO₃^2-

E)CaCO₃

Q5) Why are nitric acid solutions sometimes yellowish?

Page 24

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Chapter 23: Transition Metals and Coordination Chemistry

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Q1) In what two ways can an object appear blue?

Q2) What are the respective central-metal oxidation state, coordination number, and overall charge on the complex ion in Na₂[Cr(NH₃)₂ (NCS)₄]?

A)+3; 6; -1

B)+3; 6; +1

C)+2; 6; -2

D)+2; 4; -1

E)+1; 6; -2

Q3) The most common coordination numbers are __________.

Q4) Draw a diagram of the short-hand ground state electron configuration of zinc.

Q5) Name the compound: K₂[Cr(H₂O)₄(CO₃)₂]

Q6) What is the charge on the complex ion in Mg₂[FeCl₆]?

A)2-

B)2+

C)3-

D)3+

E)4-

Q7) What is meant by the prefix tetrakis-, and when is it used?

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Chapter 24: The Chemistry of Life: Organic and Biological Chemistry

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Q1) What is the general formula for a ketone?

A)R-O-R

B)R-CO-R'

C)R-CO-OH

D)R-OH

E)R-CHO

Q2) Predict the product of the catalytic hydrogenation of 6-ethyl-3-decene.

Q3) Which of the following compounds do not contain an sp³ hybridized oxygen atom?

A)ketones

B)alcohols

C)ethers

D)esters

E)water

Q4) Which substance would be the most soluble in gasoline?

A)water

B)NaNO₃

C)HCl

D)hexane

E)NaCl

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