When potassium iodide reacts with lead(II) nitrate, a yellow precipitate (PbI₂) is produced. If 0.78 g of lead(II) iodide was produced, how many grams of lead(II) nitrate was used? You may assume the reaction yield was 100%, and an excess of potassium iodide was used.

Choose one answer.

	A. 0.78 g
	B. 1.6 g
	C. 0.46 g
	D. 0.56 g
	E. Not enough information is given.

Question 2

If 4.94 grams of KOH is dissolved in water to make a final volume of 2.0 L, what is the molarity of the solution?

Choose one answer.

	A. 0.088 M
	B. 0.044 M
	C. 2.5 M
	D. 0.025 M
	E. 0.18 M

Question 3

If 21.3 g of glucose (C₆H₁₂O₆) is dissolved in 5.00 L of deionized water, what is the molality of the solution? (The density of water is 1.00 g/mL.)

Choose one answer.

	A. 0.0237 m
	B. 0.592 m
	C. 0.118 m
	D. 4.26 m
	E. 0.00426 m

Question 4

Which of the following is the equivalent of 4.3 ppm sodium ion (Na⁺) concentration?

Choose one answer.

	A. 0.0043 ppb
	B. 0.043 ppb
	C. 430 ppb
	D. 4300 ppb
	E. None of the above

Question 5

How many milliliters of a 0.100 M potassium permanganate stock solution would be needed to make 100 mL of 0.0250 M potassium permanganate?

Choose one answer.

	A. 10.0 mL
	B. 4.00 mL
	C. 40.00 mL
	D. 2.50 mL
	E. 25.0 mL

Question 6

The concentration of a solution is known to be 0.101 M. A student determines the concentration to be 0.088 M, 0.087 M, and 0.089 M for each titration performed. Which of the following best describes these results?

Choose one answer.

	A. The results are accurate but not precise.
	B. The results are precise but not accurate
	C. The results are neither accurate nor precise.
	D. The results are both accurate and precise.
	E. The results are not enough information is given to determine accuracy or precision.

Question 7

Concentrated hydrochloric acid is 12 M and has a density of 1.18 g/mL. What is the weight percent (% w/w) of concentrated HCl?

Choose one answer.

	A. 14%
	B. 5.1%
	C. 12%
	D. 98%
	E. 37%

Question 8

A stock solution of sodium acetate is 1.0 M. To make Solution A, 2.00 mL of the stock solution is transferred and diluted to a total volume of 100 mL. Solution B is made by transferring 5.0 mL of Solution A and diluting it to a total volume of 250 mL. Solution C is made by transferring 1.0 mL of Solution B and diluting it to a total volume of 25 mL. What is the concentration of solution C?

Choose one answer.

	A. 1.6 µM
	B. 16 µM
	C. 1.6 mM
	D. 0.16 mM
	E. None of the above

Question 9

The equation for a normal calibration curve for the detection of iron(II) is determined experimentally to be: S = 12.93 M - 1 * C + 0.0017. Analysis of a sample with unknown concentration gives an absorbance reading of 0.106. What is the concentration of iron(II) in the unknown?

Choose one answer.

	A. 1.37 M
	B. 6.50 mM
	C. 9.90 mM
	D. 8.06 mM
	E. 8.83 mM

Question 10

When performing calculations for standard additions, which of the following must be true?

Choose one answer.

	A. The volume of the standard added must be added with the volume of the sample used to give a new sample volume.
	B. The volume of the standard added is subtracted from the total volume of the sample used.
	C. The volume of the standard added can be ignored, because it is so small.
	D. The volume of the standard added can be ignored, because volumes are not used in the calculations.
	E. The volume of the standard added can be ignored, because it is part of the blank correction.

Question 11

Which of the following statements about the sensitivity of an analytical method is true?

Choose one answer.

	A. The sensitivity of an analytical method is the same as its detection limit.
	B. The sensitivity of an analytical method is a measure of ability to determine whether slight differences in experimental results are significant.
	C. The sensitivity of an analytical method is the smallest amount of analyte that the instrument is able to measure.
	D. The sensitivity of an analytical method is the response of the instrument to human error.
	E. None of the above

Question 12

Which of the following statements is true of the detection limit of an instrument?

Choose one answer.

	A. The detection limit of an instrument is the same as its sensitivity.
	B. The detection limit of an instrument is a measure of ability to determine whether slight differences in experimental results are significant.
	C. The detection limit of an instrument is the smallest amount of analyte that the instrument is able to measure.
	D. The detection limit of an instrument is the ability of the instrument to respond to an error.
	E. None of the above

Question 13

Fill in the blank. Precipitation, volatilization, and particulation are all types of ____________________.

Choose one answer.

	A. Electrochemical analysis methods
	B. Gravimetric analysis methods
	C. Tritrimetric analysis methods
	D. Spectroscopic analysis methods
	E. Photochemical analysis methods

Question 14

Fill in the blank. Gravimetric analysis relies heavily on the principle of __________________.

Choose one answer.

	A. Conservation of energy
	B. Conservation of mass
	C. Constant compostition
	D. Definite proportions
	E. The law of gravity

Question 15

Coprecipitates (inclusions, occlusions, and surface adsorbates) are a common problem in gravimetric analysis, but can be controlled by which of the following?

Choose one answer.

	A. Carefully controlling the solution conditions
	B. Reprecipitation of the solid
	C. Digestion of the precipitate
	D. Thoroughly washing and drying the filtrate
	E. All of the above

Question 16

Volatilization gravimetry would be most useful in determining which of the following?

Choose one answer.

	A. The amount of silver in a solution of silver nitrate
	B. The acidity of a water sample
	C. The amount of water in eposom salts
	D. All of the above
	E. None of the above

Question 17

Which of the following statements about the equivalence point of an acid-base titration is true?

Choose one answer.

	A. The equivalence point of an acid-base titration is the same as the indicator endpoint.
	B. The equivalence point of an acid-base titration is the point where there is an equivalent amount of titrant and titrand.
	C. The equivalence point of an acid-base titration is where the pH = 7.0 (neutral).
	D. The equivalence point of an acid-base titration is where the entire volume of the buret has been used.
	E. The equivalence point of an acid-base titration is the average value of the dissociation constants.

Question 18

What is the stoichiometry of EDTA with metal ions?

Choose one answer.

	A. It is 1:6, because EDTA is a hexaprotic weak acid with six distinct acid dissociation values.
	B. It is 1:4, because EDTA has four binding sites upon loss of the four carboxylic acid protons.
	C. It is 1:2, because EDTA has two binding sites upon loss of the two ammonium protons.
	D. It is 1:1, because EDTA forms a cage-like structure around the metal ion.
	E. It is dependent on the metal ion present.

Question 19

A 58.3 mg sample containing Sn²⁺ is dissolved in 1.0 M HCl. If 23.6 mL of 0.010 M Tl³⁺ was required to titrate to endpoint, what is the mass percent (w/w%) of tin in the original sample?

Choose one answer.

	A. 48%
	B. 28%
	C. 24%
	D. 40%
	E. 14%

Question 20

A 0.357 g sample contains only lead(II) iodide and sodium iodide in 100 mL of distilled water. Titration to the Fajan's end point requires 22.37 mL of 0.050 M silver nitrate. What is the mass percent (w/w%) of lead(II) iodide in the sample?

Choose one answer.

	A. 18%
	B. 36%
	C. 1.6%
	D. 53%
	E. 47%

Question 21

Which variable in Beer's law represents how well a chemical species absorbs light at a given wavelength?

Choose one answer.

	A. c - concentration
	B. ε - molar absorptivity coefficient
	C. A - absorbance
	D. b - path length of the sample
	E. λ - wavelength

Question 22

According to Beer's Law, what happens to the absorbance reading if the concentration of the solution is halved?

Choose one answer.

	A. The absorbance will double.
	B. The absorbance will quadruple.
	C. The absorbance will be halved.
	D. The absorbance will be quartered.
	E. There is no way to tell, because concentration and absorbance are not a linear relationship.

Question 23

Why must solutions with high concentrations be diluted prior to analysis via Beer's Law?

Choose one answer.

	A. The relationship between absorbance and concentration is not linear at high concentrations.
	B. The detector will reach its detection threshhold.
	C. The photon source is too weak to provide accurate results.
	D. The molar absorptivity of a compound is dependent on its concentration.
	E. There is no need to work with dilute concentrations; any concentration will work.

Question 24

Which of the following transitions is NOT possible in UV-Vis absorption?

Choose one answer.

	A. σ → σ*
	B. σ → n
	C. σ → π*
	D. n → π*

Question 25

Which of the following typically exhibits the largest molar absorptivities?

Choose one answer.

	A. σ → σ* absorbances
	B. σ → n absorbances
	C. σ* → π* absorbances
	D. π → π* absorbances
	E. Metal to ligand charge transfer (MLCT) absorbances

Question 26

Which of the following is the correct order in which light passes through a UV-Vis spectrometer?

Choose one answer.

	A. Detector, sample, source, monochromator
	B. Source, monochromator, sample, detector
	C. Source, sample, monochromator, detector
	D. Monochromator, source, sample, detector
	E. Sample, source, monochromator, detector

Question 27

What is the purpose of a monochromator?

Choose one answer.

	A. To remove stray light from the room
	B. To serve as a polychromatic light source
	C. To interpret the photon signal into a digital readout
	D. To allow only light of a certain wavelength to pass from the source to the sample
	E. To focus light from the sample onto the detector

Question 28

The regression line from a plot of absorbance vs. concentration yields: A = 2.31 c + 0.002. If the absorbance of an unknown is measured to be 0.124, what is the concentration of the analyte?

Choose one answer.

	A. 0.29 M
	B. 0.053 M
	C. 1.86 M
	D. 0.093 M
	E. 2.43 M

Question 29

The method of continuous variations, also known as Job's method, uses the intersection of the ligand-line and the metal-line to determine which of the following?

Choose one answer.

	A. The concentration at which the detector can no longer respond to the signal
	B. The mole ratio between the metal and ligand in a complex
	C. The maximum intensity of source photons transmitted
	D. The number of dimeric molecules formed
	E. The oxidation number of the metal

Question 30

Ultraviolet and visible radiation affect which of the following?

Choose one answer.

	A. Core electrons
	B. Valence electrons
	C. Nuclear spin
	D. Molecular vibrations
	E. Molecular rotations

Question 31

Infrared radiation affects which of the following?

Choose one answer.

	A. Core electrons
	B. Valence electrons
	C. Molecular vibrations
	D. Molecular rotations
	E. Nuclear spin

Question 32

Complete the sentence. All of the following are used to describe the bending modes in infrared spectroscopy, EXCEPT:

Choose one answer.

	A. In-plane rocking.
	B. In-plane scissoring.
	C. Assymetric stretching.
	D. Out-of-plane twisting.
	E. Out-of-plane wagging.

Question 33

What is the advantage of using a silver chloride sample cell rather than a sodium chloride sample cell for IR spectroscopy?

Choose one answer.

	A. Aquesous samples can be measured; AgCl is not water soluble.
	B. There is no advantage.
	C. Silver chloride does not absorb IR radiation.
	D. Silver chloride is translucent.
	E. Sodium chloride is less expensive.

Question 34

In order for a compound to be IR active, it must undergo which of the following?

Choose one answer.

	A. A change in polarizability
	B. A change in dipole moment
	C. Emission of an electron
	D. Transfer of an electon
	E. Metal-ligand charge transfer

Question 35

Complete the sentence. All of the following are infrared sources, EXCEPT:

Choose one answer.

	A. The Nernst glower.
	B. The Globar source.
	C. An incandescent wire.
	D. A pyroelectric glower.

Question 36

Complete the sentence. All of the following are detectors used in infrared spectroscopy, EXCEPT:

Choose one answer.

	A. A charge-coupled diode.
	B. A thermocouple.
	C. A pyroelectric detector.
	D. A photoelectric detector.

Question 37

Fill in the blank. NMR affects a molecule's ________________.

Choose one answer.

	A. Nuclear spin
	B. Valence electrons
	C. Core electrons
	D. Molecular vibrations
	E. Molecular rotations

Question 38

In ¹H-NMR spectroscopy, if a CH₂ neighbors a CH₃, the hydrogen nuclei of the CH₃ will appear as which of the following?

Choose one answer.

	A. A doublet, with a peak integration of 2
	B. A doublet, with a peak integration of 3
	C. A triplet, with a peak integration of 2
	D. A triplet, with a peak integration of 3
	E. A single peak, with an integration of 5

Question 39

Where does spin-lattice relaxation occur?

Choose one answer.

	A. It occurs between neighboring nuclei with identical frequencies but different quantum states via energy transfer.
	B. It occurs between the excited nuclei and nuclei within the sample matrix.
	C. It occurs between atoms in the same molecule.
	D. It occurs between the nuclei of the sample and the signal source.
	E. All of the above

Question 40

The value of the chemical shift in NMR spectroscopy is directly related to which of the following?

Choose one answer.

	A. The amount of shielding
	B. The applied magnetic field
	C. The identity of the reference sample
	D. The electronegativity of the nucleus
	E. All of the above

Question 41

Fluorescence occurs as a result of which of the following?

Choose one answer.

	A. Relaxation from a singlet excited state to a singlet ground state
	B. Relaxation from a triplet excited state to a singlet ground state
	C. Nonradiative (vibrational) relaxation
	D. Intersystem crossing (isc)
	E. All of the above

Question 42

Phosphorescence occurs as a result of which of the following?

Choose one answer.

	A. Relaxation from a singlet excited state to the singlet ground state
	B. From a triplet excited state to the singlet ground state
	C. Intersystem crossing (isc)
	D. Nonradiative (vibrational) relaxation
	E. All of the above

Question 43

Why are flourescence and phosphorescence spectra measured at a 90 degree angle to the source?

Choose one answer.

	A. To ensure that incident (source) photons are not observed
	B. Because the sample cell is darkened on two adjacent sides
	C. Because the monochromator directs the light at a 90 degree angle
	D. Because the process of fluorescence and phosphorescence are too intense to observe directly
	E. To make the overall instrument smaller

Question 44

Complete the sentence. Fluorescence and phosphorescence can be used for detection of all of the following, EXCEPT:

Choose one answer.

	A. Vitamins.
	B. Environmental pollutants.
	C. Uncomplexed metal ions.
	D. Pharmaceuticals.
	E. Aromatic amino acids.

Question 45

A fluorescence quantum yield of 0.93 would suggest that most excited state molecules are doing which of the following?

Choose one answer.

	A. Returning to the ground state by fluorescence
	B. Returning to the ground state by non-radiative decay
	C. Returning to the ground state by intersystem crossing
	D. Remaining in the excited state past the experimental timeframe
	E. None of the above

Question 46

Why are photomultiplier tubes often used in fluorescence spectroscopy?

Choose one answer.

	A. Because the photon sources are too weak to vibrationally excite the samples
	B. Because sample cells are small
	C. Because they supply a reference signal
	D. Because fluorescence intensities are usually low
	E. None of the above

Question 47

Why is fluorescence spectroscopy often carried out in a liquid nitrogen environment?

Choose one answer.

	A. Phosphorescence is more likely to coccur at low temperatures in a viscous medium.
	B. Phosphorescent molecules tend to also have explosive properties.
	C. The monochromator slows down the radiation before it hits the sample.
	D. The detector requires lower temperatures for operation.
	E. The source radiation can overheat and destory the analyte.

Question 48

How does turbidimetry differ from nephelometry?

Choose one answer.

	A. Turbidimerty measures the decrease in transmittance of incident radiation; nephelometry measures the intensity of scattered radiation.
	B. Nephelometry measures the decrease in transmittance of incident radiation; turbidimetry measures the intensity of scattered radiation.
	C. Nephelometry measures the total metal ion, or inorganic, content; turbidimetry measures total organic content.
	D. Turbidimetry measures the total metal ion, or inorganic, content; nephelometry measures total organic content.
	E. The terms are synonymous; there is no difference.

Question 49

Turbidimetry and nephelometry are analytical methods based on which of the following?

Choose one answer.

	A. Light scattering
	B. Photon emission
	C. Photon absorption
	D. Nuclear repulsion
	E. Paramagnetism

Question 50

What is the advantage of an inductively coupled plasma source rather than a flame?

Choose one answer.

	A. Better atomiza higher population of excited statestion and a
	B. Lower operating temperatures and less expensive replacement costs
	C. Minimization of scattering and ionization of analytes
	D. All of the above
	E. None of the above

Question 51

Atomic absorption spectroscopy results are highly reproducible but have low sensitivity and efficiency. This is due to which of the following?

Choose one answer.

	A. The small amount of analyte that actually reaches the flame
	B. The high temperatures of analysis often destroy the atoms
	C. The amount of dilution due to mixing with large volumes of combustion gases
	D. A and B only
	E. A and C only

Question 52

Fill in the blank. The relationship between the analyte concentration and the intensity of measured radiation from thermal excitation methods, such as a flame or plasma, is ________________.

Choose one answer.

	A. Linear
	B. Exponential
	C. Parabolic
	D. Polynomial
	E. Asymptopic

Question 53

Flame atomic absorption measures absorption of radiation of analytes in which phase?

Choose one answer.

	A. Solid phase
	B. Liquid (neat) phase
	C. Gas phase
	D. Aquesous phase
	E. Plasma phase

Question 54

Why is a hollow cathode tube lamp necessary in atomic absorption?

Choose one answer.

	A. Because cathode lamps are cheaper to operate and maintain
	B. Because continuous spectrum lamps do not emit at the proper intensity
	C. Because the width of an atom's absorption band is narrow
	D. Because continuous spectrum lamps cause ionization of the molecules
	E. All of the above

Question 55

Fill in the blank. Background correction in flame atomic absorption spectroscopy can minimize the effect of ___________________.

Choose one answer.

	A. Ionization of the analyte
	B. Scattering and absorption by the matrix of the analyte
	C. Reactions between the analyte and matrix
	D. Non-volatilization of the analyte

Question 56

Chemical interferences in atomic absorption that cannot be accounted for using a background correction, but can be minimized, include which of the following?

Choose one answer.

	A. Nonvolatilization of the analyte
	B. Ionization of the analyte
	C. Absorption or scattering of radiation by the matrix
	D. All of the above
	E. A and B only

Question 57

Which of the following are forms of radiationless deactivation of an excited state?

Choose one answer.

	A. Intersystem crossing
	B. Internal conversion
	C. External conversion
	D. Vibrational relaxation
	E. All of the above

Question 58

When does intersystem crossing occur?

Choose one answer.

	A. When a molecule transfers to a higher vibrational energy level of a lower energy electronic state with a different spin
	B. When a molecule moves to a lower vibrational energy level in the same electronic state
	C. When a molecule transfers to a higher vibrational energy level of a lower energy electronic state with the same spin
	D. energy is emitted as a photon from a singlet or triplet spin state
	E. When energy is passed to the solvent or to another component of the sample's matrix

Question 59

Fill in the blank. The lowest vibrational energy level of the lowest electronic singlet state (S₀) is referred to as the ___________________.

Choose one answer.

	A. Ground state
	B. Zero state
	C. Newtonian state
	D. Bohring state
	E. Non-excited state

Question 60

Whether an electron is in the triplet state or singlet state depends on which of the following?

Choose one answer.

	A. Its spin-pairing with the ground state
	B. The amount of radiation it was exposed to
	C. Its ability to undergo radiationless decay
	D. Its initial energy level before absorption
	E. Its availability to become excited

Question 61

In a chromatographic analysis of an unknown mixture, compound A has a retention time of 5.56 minutes and a baseline width of 0.87, and compound B has a retention time of 6.32 minutes and a baseline width of 0.53 minutes. Are these peaks resolved, and what is the resolution between the two peaks?

Choose one answer.

	A. Yes, 0.54
	B. No, 0.54
	C. Yes, 1.09
	D. No, 1.09
	E. There is not enough information given to determine resolution.

Question 62

The "void peak" in a chromatogram corresponds to which of the following?

Choose one answer.

	A. Components that had no interaction with the stationary phase
	B. The peak that arises from poor selection of a stationary phase
	C. The peak that arises from the mobile phase only
	D. Components that had no interaction with the mobile phase
	E. All peaks after the first peak in the chromatogram

Question 63

If a compound has a retention time of 5.30 minutes with a baseline width of 0.64 minutes on a 2.0 m silica gel column, what is the average height of a theoretical plate?

Choose one answer.

	A. 1.8 mm/plate
	B. 15 mm/plate
	C. 29 mm/plate
	D. 0.24 mm/plate
	E. 2.7 mm/plate

Question 64

Which of the following statements about columns containing more theoretical plates is true?

Choose one answer.

	A. Columns containing more theoretical plates make separations imposssible.
	B. Columns containing more theoretical plates take a long time to perform separations.
	C. Columns containing more theoretical plates are better suited to separate a complex mixture.
	D. Columns containing more theoretical plates interact irreversibly with the analyte.
	E. Columns containing more theoretical plates lend themselves to component mixing.

Question 65

"Tailing" of a chromatographic peak is a result of which of the following?

Choose one answer.

	A. Interactions of the solute with the stationary phase
	B. Overloading the column with sample
	C. Interactions between the stationary and mobile phases
	D. Too many theoretical plates
	E. Small theortetical plate heights

Question 66

"Fronting" of a chromatographic peak is a result of which of the following?

Choose one answer.

	A. Interactions between the stationary and mobile phase
	B. Overloading the column with sample
	C. Interactions of the solute with the stationary phase
	D. Small theortetical plate heights

Question 67

Band broadening in column chromatography is a result of which of the following?

Choose one answer.

	A. Mass transfer in the stationary phase
	B. Mass transfer in the mobile phase
	C. Longitudinal diffusion
	D. Variations in path lengths (Eddy diffusion)
	E. All of the above

Question 68

Complete the sentence. All of the following are common carrier gases from gas chromatography, EXCEPT:

Choose one answer.

	A. Oxygen.
	B. Nitrogen.
	C. Helium.
	D. Argon.
	E. Carbon dioxide.

Question 69

When using gas chromatography, how is optimum column efficiency obtained?

Choose one answer.

	A. When the samples are injected slowly and in large quantities
	B. When the samples are injected slowly and in small quantities
	C. When the samples are injected quickly and in large quantities
	D. When the samples are injected quickly and in small quantities
	E. None of the above

Question 70

What is the most common support material for a packed GC column?

Choose one answer.

	A. Silica gel
	B. Alumina
	C. Fused silica
	D. Glass
	E. Diatomaceous earth

Question 71

WCOT, SCOT, PLOT, and FSOT are all types of which of the following?

Choose one answer.

	A. Open tubular GC columns
	B. Capillary GC columns
	C. Packed GC columns
	D. Both A and B
	E. Both A and C

Question 72

Which of the following GC detectors would most likely allow recovery of a sample after analysis?

Choose one answer.

	A. Flame ionization detector (FID)
	B. Thermal conductivity detector (TCD)
	C. Flame photometric detector (FPD)
	D. Hall electrolytic conductivity detector
	E. Nitrogen-phosphorus detector

Question 73

Which of the following GC detectors would be least affected by the carrier gas?

Choose one answer.

	A. Thermal conductivity detector (TCD)
	B. Electron capture detector (ECD)
	C. Photoionization detector (PID)
	D. Flame photometric detector (FPD)
	E. None of these detectors would be affected by the carrier gas.

Question 74

In size exclusion chromatography, what happens to the larger particles?

Choose one answer.

	A. They elude first, before smaller particles.
	B. They are broken down into smaller particles.
	C. They become oxidized as they move through the column.
	D. They remain on the column longer than smaller particles.
	E. They bind permanently to the stationary phase.

Question 75

Fill in the blank. Ion exchange chromatography is best suited to separate ___________________.

Choose one answer.

	A. Hydrophilic molecules
	B. Hydrophobic molecules
	C. Mixed metal sulfides and oxides
	D. Large molecules, such as DNA and RNA
	E. Cations and anions

Question 76

Which of the following statements about the mobile phase in Supercritical fluid chromatography (SFC) is false?

Choose one answer.

	A. It requires lower pressures than those needed for HPLC.
	B. It gives better resolution than GC.
	C. It has densities similar to a liquid.
	D. Its mobile phase has the viscosity properties of a gas.
	E. It has solvent properties of a liquid.

Question 77

The stationary phase in ion exchange chromatography is a cross-linked polymer resin with covalently attached functional groups. Which of the following is NOT a typical functional group used for IEC?

Choose one answer.

	A. Sulfonic acid (-SO₃^-)
	B. Carboxylic acid (-COO^-)
	C. Quarternary amine (-CH₂N(CH₃)₃⁺)
	D. Amine (-NH₃⁺)
	E. Hydroxyl (-OH^-)

Question 78

Reversed-phase chromatography refers to which of the following?

Choose one answer.

	A. A stationary phase and mobile phase of similar polarities
	B. A nonpolar stationary phase and a nonpolar mobile phase
	C. A polar stationary phase and a nonpolar mobile phase
	D. A nonpolar stationary phase and a polar mobile phase
	E. A polar stationary phase and a polar mobile phase

Question 79

Which of the following would elute first when using capillary zone electrophoresis?

Choose one answer.

	A. Ca²⁺
	B. CH₃NH₃⁺
	C. Cl^-
	D. HCOO^-
	E. CH₃COO^-

Question 80

How are separations by electrophoresis carried out?

Choose one answer.

	A. Via applying an electric current
	B. Via saponification of the analyte
	C. Via polymerization of the analyte
	D. Via oxidation reactions at stationary phase sites
	E. Via reduction reactions at stationary phase sites

Question 81

Fill in the blank. Cd wire used to measure the concentration of cadmium ion is an example of a _______________________.

Choose one answer.

	A. Metallic electrode of the second kind
	B. Metallic electrode of the first kind
	C. Saturated calomel electrode
	D. Reference electrode
	E. Silver/silver chloride electrode

Question 82

Fill in the blank. Ag wire used to measure the concentration of Br- ion is an example of a ______________________.

Choose one answer.

	a. Saturated calomel electrode
	b. Metallic electrode of the first kind
	c. Metallic electrode of the second kind
	d. Silver/silver chloride electrode
	e. Reference electrode

Question 83

What is the process of the loss of an electron called?

Choose one answer.

	A. Oxidation
	B. Reduction
	C. Transference
	D. Sublimation
	E. Neutralization

Question 84

What is the process of the gain of an electron called?

Choose one answer.

	A. Oxidation
	B. Reduction
	C. Sublimation
	D. Transference
	E. Neutralization

Question 85

Which of the following is a substrate that is oxidized?

Choose one answer.

	A. Cationic species
	B. Anionic species
	C. Neutral species
	D. Reducing agent
	E. Oxidizing agent

Question 86

Which of the following is a substrate that is reduced?

Choose one answer.

	A. Oxidizing agent
	B. Reducing agent
	C. Cationic species
	D. Anionic species
	E. Neutral species

Question 87

What is the purpose of the salt bridge in a galvanic (voltaic) cell?

Choose one answer.

	A. To complete the electrochemical circuit
	B. To provide free electrons for redox processes
	C. To provide a site for oxidative reduction
	D. To serve as a working electrode
	E. To serve as a reference electrode

Question 88

If a redox couple is at equilibrium in an electrochemical cell, then which of the following statements about the current and potential is most accurate?

Choose one answer.

	A. The current is zero, and the potential is given by the Nernst equation.
	B. The current and potential are both zero.
	C. The current is negative, and the potential is zero.
	D. The current is positive, and the potential is zero.
	E. The potential is zero, and the current is given by the Nernst equation.

Question 89

Complete the sentence. The basic setups for electrochemical measurement include all of the following, EXCEPT:

Choose one answer.

	A. Measure the potential at zero current.
	B. Measure the potential while controlling the current.
	C. Measure the potential and current simultaneously.
	D. Measure the current while controlling the potential.
	E. All of the above

Question 90

Which of the following is a static (i = 0) electrochemical technique?

Choose one answer.

	A. Potentiometry
	B. Controlled-current coulometry
	C. Controlled-potential coulometry
	D. Cyclic voltammetry
	E. Amperometry

Question 91

Where does the reduction reaction occur?

Choose one answer.

	A. At the anode
	B. At the cathode
	C. Within the potentiometer
	D. Within the salt bridge
	E. Within the bulk solution

Question 92

Where does the oxidation reaction occur?

Choose one answer.

	A. Within the potentiometer
	B. Within the salt bridge
	C. At the anode
	D. At the cathode
	E. Within the bulk solution

Question 93

The use of the Nerst equation to calculate potentials is really a simplistic model. Which of the following does it ignore?

Choose one answer.

	A. Matrix effects
	B. Temperature effects
	C. Junction potentials
	D. All of the above
	E. None of the above

Question 94

Fill in the blank. The potential that develops at the interface of two solutions due to differences in concentrations and ionic mobility is called the _________________ potential.

Choose one answer.

	A. Osmotic
	B. Bridging
	C. Coulombic
	D. Reference
	E. Junction

Question 95

Which of the following statements about the standard hydrogen electrode, the calomel electrode, and the silver/silver chloride electrode is true?

Choose one answer.

	A. These electrodes combine to make a complete electrochemical cell.
	B. These electrodes are typically used as reference electrodes.
	C. These electrodes are typically used as working (indicator) electrodes.
	D. These electrodes are examples of membrane electrodes.
	E. These electrodes have the same electrochemical potential.

Question 96

A pH meter is an example of which type of membrane electrode?

Choose one answer.

	A. Glass ion selective electrode
	B. Potentiometric biosensor (enzyme electrode)
	C. Solid-state ion selective electrode
	D. Liquid-based ion selective electrode
	E. Gas-sensing electrode

Question 97

In a cyclic voltammogram, the peak current(i) is directly related to which of the following?

Choose one answer.

	A. The concentration of anayte
	B. The surface area of the working electrode
	C. The number of electrons involved in the redox process
	D. The diffusion coefficient of the electroactive species
	E. All of the above

Question 98

One electrochemical technique involves first depositing an analyte on the surface of an electrode, then using an applied current to remove the analyte via a reduction or oxidation reaction. What is this method called?

Choose one answer.

	A. Hydrodynamic voltammetry
	B. Stripping voltammetry
	C. Amperometry
	D. Polarography
	E. Cyclic voltammetry

Question 99

Which of the following is NOT a variable in voltammetric methods?

Choose one answer.

	A. Type of working electrode
	B. How the potential is applied
	C. The inclusion of convection
	D. How the current is applied
	E. All of the above

Question 100

Fill in the blank. Coulometric techniques result in a plot of ____________________.

Choose one answer.

	A. Current versus time
	B. Electrochemical potential versus time
	C. Current versus electrochemical potential
	D. Current only
	E. Potential only