Chem 313: Quantitative
Analysis Student Competencies
Quantitative Chemical Analysis, 6th. Ed.,
Daniel C. Harris, 2002.
Chapter 1 Student competencies
Upon completion of this chapter, students should
be able to:
- Know SI units,
including prefixes ranging from 1012 to 10-12, and
be able to inter-convert among units.
- Know the
definitions of concentration units: molarity, molality, normality,
formality, ppm, ppb, and % composition. Be able to calculate and
inter-convert among these. Understand how these concentrations units
are used for solutions and gases.
- Describe how to
prepare solutions of given concentration.
- Understand and
describe how to dilute a solution.
- Carry out
calculations for solution preparation.
- Know how to solve
problems that require an understanding of solution stoichiometry.
Chapter
6 Student competencies
Upon completion of this chapter, students should be able to:
- Write and
manipulate equilibrium constants from balanced chemical equations.
- Relate thermodynamic
quantities, including enthalpy, entropy, and free energy, to equilibrium
constants.
- Apply Le
Châtelier’s Principle to systems disturbed from equilibrium, including
temperature, pressure, and concentration changes.
- Define solubility and
saturated solutions.
- Write reactions for
solid salts dissolved in water, and the corresponding solubility product
expression.
- Calculate the
concentration of a dissolved species in a saturated solution.
- Calculate the
concentration of a dissolved species in a saturated solution containing a
common ion.
Chapter 7 Student competencies
Upon completion of this chapter, students should be able to:
·
Explain the terms titrant,
equivalence point, and end point, indicator, standardization, primary standard
solution, blank titration, direct titration, and back titration.
·
Perform rigorous stoichiometric
calculations involved in volumetric analysis.
·
Describe a Kjeldahl nitrogen
analysis.
·
Explain and give examples of
spectrophotometric titrations.
·
Explain p-functions.
·
Perform rigorous stoichiometric
calculations for a precipitation titration curve.
·
Utilize a spreadsheet for
calculation of a titration curve.
·
Describe Volhard and Fajans
endpoint detection for argentometric titrations.
Chapter 8 Student competencies
Upon completion of this chapter, students should be able to
·
Explain how an inert salt can
increase the solubility of an ionic compound.
·
Calculate the ionic strength of
a solution.
·
Explain the terms activity and
activity coefficient.
·
Write equilibrium constant
expressions in terms of activity.
·
Utilize the extended Debye-Hückel
equation for evaluating activity coefficients.
·
Utilize interpolation and
activity coefficient tables for evaluating activity coefficients.
·
Utilize activity concepts for stoichiometric
calculation of pH and solubility.
Chapter 9 Student competencies
Upon completion of this chapter, students should be able to
·
Describe and write charge
balance equations in solutions.
·
Describe and write mass balance
equations in solutions.
·
Utilize systematic equilibrium
procedures for stoichiometric calculation of pH and solubility.
·
Utilize spreadsheets for the
calculation of equilibrium concentrations for solutions.
Chapter
10 Student competencies
Upon completion of this chapter, students should be able to
·
Calculate pH and pOH for strong
acids and bases at moderate and low concentrations.
·
Write equilibrium expressions
for weak acids and bases, and calculate equilibrium concentrations and
fractions of dissociation.
·
Describe the properties of
buffer solutions.
·
Derive the
Henderson-Hasselbalch equation from weak acid and weak base equilibrium
expressions.
·
Calculate the pH of buffer
solution.
·
Calculate the pH of a buffer
solution with added strong acid or base.
·
Explain what is meant by buffer
capacity.
Chapter 11 Student competencies
Upon completion of this chapter, students should be able to
·
Calculate pH, protonated,
intermediate, and deprotonated concentrations for diprotic acid systems.
·
Utilize spreadsheets and
successive approximations for calculating the pH, protonated, intermediate, and
deprotonated concentrations for diprotic acid systems.
·
Calculate pH for diprotic acid
buffer systems.
·
Explain the term isoelectric pH
and isoionic pH for diprotic amino acids
Chapter 12 Student competencies
Upon completion of this chapter, students should be able to
·
Utilize rigorous stoichiometric
calculations to determine pH at various points in a strong acid/strong base
titration.
·
Utilize rigorous stoichiometric
calculations to determine pH at various points in a weak acid/strong base
titration.
·
Utilize rigorous stoichiometric
calculations to determine pH at various points in a strong acid/weak base
titration.
·
Determine and utilize spreadsheets
for first and second derivative titrations curves in the detection of endpoint.
·
Derive the Gran equation and construct
Gran plots to determine acid ionization constants.
·
Describe how to correctly
choose an appropriate color indicator for titration experiments.
Chapter
14 Student competencies
Upon completion of this chapter, students should be able to
·
Define oxidation and reduction,
anode, and cathode.
·
Balance oxidation-reduction
reactions.
·
Utilize concepts of charge,
current, voltage, resistance, power, work, and free energy for problem-solving
·
Describe the construction of a
galvanic cell.
·
Describe the function of a salt
bridge.
·
Describe the standard hydrogen
electrode.
·
Utilize standard reduction
potentials to determine standard cell potentials.
·
Utilize the Nernst equation to
determine non-standard cell potentials.
·
Utilize standard cell
potentials to determine equilibrium constants.
Chapter 15 Student competencies
Upon completion of this chapter, students should be able to
·
Describe silver-silver and
calomel reference electrodes.
·
Explain junction potential.
·
Describe a glass electrode for
pH measurement.
·
Explain the calibration of a pH
electrode and sources of error in pH measurements.
·
Discuss the construction of
several ion selective electrodes and utilize problem solving for quantitative
measurements.
·
Describe p and n-type
semiconductors, and how FETs can be used as pH sensors.
Chapter
19 Student competencies
Upon completion of this chapter, students should
be able to:
- Know how to
calculate wavenumber, wavelength, frequency, and energy of a given photon.
- Understand
the spectral regions associated with changes in electronic, vibrational,
rotational, and magnetic energy levels.
- Explain on
the atomic/molecular level, why atomic and molecular spectra are so
different. Relate this to the methods necessary to measure atomic spectra.
- Understand
absorption, spontaneous emission, and stimulated emission processes.
- Understand
Beer's law and how to use it to determine an unknown concentration.
- Diagram
single beam and double beam spectrometers and discuss how they are used to
measure the absorbance of a sample.
- Explain why
most organic liquids are clear and most organic solids appear to be white.
- Understand
the relative energies of singlet and triplet states; discuss the relative
probabilities of singlet-to-singlet and singlet-to-triplet transitions.
- Diagram the
physical processes that can occur after a molecule has absorbed an
ultraviolet or visible photon. Use it to explain the basis for
fluorescence and phosphorescence.
- For
luminescent signals, relate the intensity of the emission source to signal
strength.
Chapter 20 Student competencies
Upon completion of this chapter, students should
be able to:
- Outline the
steps taken to use Beer's law to determine the concentration of mixture
components when the spectra are well resolved.
- Explain what
isosbectic points are and how to identify them.
- Outline the
steps for Job's method and what it is used for.
- Discuss flow
injection analysis and the advantages / disadvantages of it.
- Discuss
ELISA and the major advantages / disadvantages of it. Understand how
time-resolved fluorescence immunoassays are carried out and the basis for
their use.
- Understand
what is meant by quantum yield. Discuss how luminescent quenching
can be used to detect oxygen. Diagram the layout and function of a
portable instrument to do this.
Chapter 21 Student competencies
Upon completion of this chapter, students should
be able to:
- Know how to use
refractive indices to calculate the amount of light reflected at each
interface.
- Use Snell's law to
calculate changes in direction for refracted rays. Use Snell's Law
to determine the minimum critical angle for internal reflections to occur.
- Explain how
internal reflection techniques work.
- Understand thermal
radiation (black-body radiation). Explain how the energy and
wavelength of maximum intensity changes with temperature.
- Explain how a
four-level laser works.
- Explain how grating
monochromators and prisms work. Explain how filters are used.
- Understand how
photomultiplier tubes and silicon diodes are used to detect
electromagnetic radiation. Know the wavelengths that can be detected
with silicon diodes.
- Explain how an
FT-IR instrument works and the mathematical operations necessary to obtain
an absorbance spectrum.
- Understand the
relationship between sampling time and signal to noise ratio.
Chapter 22 Student competencies
Upon completion of this chapter, students should
be able to:
- Explain the basis
for atomic absorption and emission instruments.
- Describe the three
methods to atomize samples in atomic spectroscopic instruments.
- Know the Boltzman distribution
and use it to calculate relative populations of energy levels.
Understand how this relative population changes with temperature and with
energy gaps.
- Explain how
nebulizers and hollow cathode lamps work.
- Outline the
potential interferences in atomic spectroscopy. Discuss how
background corrections are carried out.
- Understand the
basis for line widths in atomic spectroscopy.
- Understand what
matrix modifiers are used for.
Chapter 23 Student competencies
Upon completion of this chapter, students should
be able to:
- Know the partition
relation for solvent extraction procedures and be able to solve problems
using it.
- Understand the use
of pH adjustment for extraction procedures
- Understand what a
distribution coefficient is, what systems it applies to, and how to use
it.
- Understand and
explain the basis for chromatography; define mobile and stationary phases,
eluent, eluate, packed and open tubular columns.
- Understand and
explain the basis for these types of chromatography:
- Adsorption
chromatography
- Partition
chromatography
- Ion-Exchange
chromatography
- Molecular
Exclusion chromatography
- Affinity
chromatography
- From a given
chromatogram, know how to calculate each of the following:
- Adjusted
retention times
- Relative
retention
- Capacity
factor
- Partition
coefficient
- Resolution
- Number
of theoretical plates
- Plate
Height
- Understand the van
Deemter equation and apply it to various forms of chromatography.
- Understand the two
major asymmetries associated with chromatographic band shapes and explain
the underlying cause for each.
- Understand and
explain the silanization process.
Chapter 24 Student competencies
Upon completion of this chapter, students should
be able to:
- Diagram a
gas chromatograph and be able to explain the features and functions of
each component.
- Describe
open tubular (WCOT and PLOT) and packed columns; be able to discuss the
stationary phases most often used; Describe the most common applications
for the various column types.
- Determine
the retention index for a given compound.
- Discuss
isothermal and temperature-programmed GC and the advantages of each.
- Understand
the basis and applicability of split, split less, and on-column GC
injection techniques.
- Understand,
diagram, and describe the most important GC detectors to include TCD, FID,
ECD and MS.
- Understand
and describe solid-phase micro extraction (SPME) techniques; outline the
advantages and disadvantages of SPME.
- Describe
purge and trap GC.
- Understand
the basis for GC method development.
- Understand
and diagram the four major types of mass selectors and two ionization
methods used in mass spectrometry.
Chapter 25 Student competencies
Upon completion of this chapter, students should
be able to:
- Diagram the
layout of an HPLC instrument and explain the design and function of
each component.
- Explain why
packed columns are used in lieu of open tubular ones for HPLC; identify
and explain the effect of particle size on resolution and pressure.
- Discuss the
effect of temperature on HPLC retention times and explain why a column
heater is sometimes used.
- Describe the
geometry of HPLC columns and the use of guard columns.
- Describe in
detail the structure of silica particles. Outline the pH limitations
for the use of silica; identify the support particles used outside of
silica's pH range. Explain how bonded stationary phases can be
attached to silica. Identify the chromatographic technique that
relies on bare silica.
- Explain what
is meant by an eluotropic series and by eluent strength.
- Discuss
normal-phase and reverse-phase HPLC. Understand the relation between
eluent strength and polarity for both normal and reverse phase
separations.
- Understand
isocratic and gradient elution and the utility of each.
- Understand
the steps taken to treat solvents in HPLC.
- Know what is
meant by dead volume; what effect dead volume has on peaks, and what steps
to take to minimize its effects.
- Explain how
injection is accomplished in HPLC.
- Understand
and describe the major detection schemes for HPLC to include refractive
index, fluorescence, absorbance, and electrochemical.
- Describe and
explain atmospheric pressure chemical ionization and pneumatically
assisted electrospray techniques for introducing the liquid eluate from an
LC column into a mass spectrometer.
- Compare the
advantages and disadvantages of selective ion monitoring and full scan
monitoring using MS detectors.
- Explain why
30 mM of triethylamine, ammonium acetate or triethyl ammonium acetate are
sometimes added to an HPLC mobile phase.
Chapter 26 Student competencies
Upon completion of this chapter, students should
be able to:
- Discuss the
structure of ion exchange resins, the structure of strongly and weakly
acidic cation exchangers, the structure of strongly and weakly basic
anion exchangers, and the effect of increasing cross-linking on ion
selectivity.
- Discuss
cellulose and dextran ion exchangers; identify their features and the
types of applications they are used for.
- Understand
and explain the effects of charge, hydrated radius, and polarizability on
ion-exchange selectivity. Predict the relative values of selectivity
coefficients for various ions and amounts of cross-linking.
- Explain what
Donnan equilibrium is and the basis for ion exclusion chromatography.
- Outline the
major applications of ion exchange.
- Discuss ion
chromatography and the basis for suppressed anion and suppressed cation
chromatography.
- Discuss the
basis for separation in molecular exclusion (gel permeation)
chromatography and the applications to which it is applied.
- Outline the
basic principles and uses of affinity chromatography.