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2.S: Basic Tools of Analytical Chemistry (Summary)

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    70463
  • [ "article:topic", "Author tag:Harvey", "authorname:harveyd", "showtoc:no" ]

    There are a few basic numerical and experimental tools with which you must be familiar. Fundamental measurements in analytical chemistry, such as mass and volume, use base SI units, such as the kilogram. Other units, such as energy, are defined in terms of these base units. When reporting measurements, we must be careful to include only those digits that are significant, and to maintain the uncertainty implied by these significant figures when transforming measurements into results.

    The relative amount of a constituent in a sample is expressed as a concentration. There are many ways to express concentration, the most common of which are molarity, weight percent, volume percent, weight-to-volume percent, parts per million and parts per billion. Concentrations also can be expressed using p-functions.

    Stoichiometric relationships and calculations are important in many quantitative analyses. The stoichiometry between the reactants and products of a chemical reaction are given by the coefficients of a balanced chemical reaction.

    Balances, volumetric flasks, pipets, and ovens are standard pieces of equipment that you will routinely use in the analytical lab. You should be familiar with the proper way to use this equipment. You also should be familiar with how to prepare a stock solution of known concentration, and how to prepare a dilute solution from a stock solution.

    2.8.1 Key Terms

    analytical balance
    concentration
    desiccant
    desiccator
    dilution
    formality
    meniscus
    molality
    molarity
    normality
    parts per million
    parts per billion
    p-function
    quantitative transfer
    scientific notation
    significant figures

    SI units
    stock solution
    volume percent
    volumetric flask
    volumetric pipet
    weight percent
    weight-to-volume percent

    Additional Resources

    Gathered here are three types of resources: suggested experiments, mostly from the Journal of Chemical Education and The Chemical Educator, that provide practical examples of concepts in the textbook; additional readings from the analytical literature that extend and supplement topics covered in the textbook. Although primarily intended for the use of instructors, these resources also will benefit students who wish to pursue a topic at more depth.

    The following two web sites contain useful information about the SI system of units.

    For a chemist’s perspective on the SI units for mass and amount, consult the following papers.

    • Freeman, R. D. “SI for Chemists: Persistent Problems, Solid Solutions,” J. Chem. Educ. 2003, 80, 16-20.
    • Gorin, G. “Mole, Mole per Liter, and Molar: A Primer on SI and Related Units for Chemistry Students,” J. Chem. Educ. 2003, 80, 103-104.

    The following are useful resources for maintaining a laboratory notebook and for preparing laboratory reports.

    • Coghill, A. M.; Garson, L. M. (eds) The ACS Style Guide: Effective Communication of Scientific Information, 3rd Edition, American Chemical Society: Washington, D. C.; 2006.
    • Kanare, H. M. Writing the Laboratory Notebook, American Chemical Society: Washington, D. C.; 1985.

    The following texts provide instructions for using spreadsheets in analytical chemistry.

    • de Levie, R. How to Use Excel® in Analytical Chemistry and in General Scientific Data Analysis, Cambridge University Press: Cambridge, UK, 2001.
    • Diamond, D.; Hanratty, V. C. A., Spreadsheet Applications in Chemistry, Wiley-Interscience: New York, 1997.
    • Feiser, H. Concepts and Calculations in Analytical Chemistry: A Spreadsheet Approach, CRC Press: Boca Raton, FL, 1992.

    The following is a classical text emphasizing the application of intuitive thinking when solving problems.

    • Harte, J. Consider a Spherical Cow: A Course in Environmental Problem Solving, University Science Books: Sausalito, CA, 1988.

    References

    1. Murray, R. W. Anal. Chem. 2007, 79, 1765.
    2. For a review of other types of electronic balances, see Schoonover, R. M. Anal. Chem. 1982, 54, 973A-980A.