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  2. Karl Fischer titration - Wikipedia

    en.wikipedia.org/wiki/Karl_Fischer_titration

    This elementary reaction consumes exactly one molar equivalent of water vs. iodine. Iodine is added to the solution until it is present in excess, marking the end point of the titration, which can be detected by potentiometry. The reaction is run in an alcohol solution containing a base, which consumes the sulfur trioxide and hydroiodic acid ...

  3. Titration - Wikipedia

    en.wikipedia.org/wiki/Titration

    A back titration is useful if the endpoint of the reverse titration is easier to identify than the endpoint of the normal titration, as with precipitation reactions. Back titrations are also useful if the reaction between the analyte and the titrant is very slow, or when the analyte is in a non-soluble solid. [44]

  4. Bjerrum plot - Wikipedia

    en.wikipedia.org/wiki/Bjerrum_plot

    Example Bjerrum plot: Change in carbonate system of seawater from ocean acidification.. A Bjerrum plot (named after Niels Bjerrum), sometimes also known as a Sillén diagram (after Lars Gunnar Sillén), or a Hägg diagram (after Gunnar Hägg) [1] is a graph of the concentrations of the different species of a polyprotic acid in a solution, as a function of pH, [2] when the solution is at ...

  5. Gravimetric analysis - Wikipedia

    en.wikipedia.org/wiki/Gravimetric_analysis

    The drying agent absorbs any aerosolized water and/or water vapor (reaction 3.). The mix of the drying agent and NaOH absorbs the CO 2 and any water that may have been produced as a result of the absorption of the NaOH (reaction 4.). [11] The reactions are: Reaction 3 - absorption of water NaHCO 3 (aq) + H 2 SO 4 (aq) → CO 2 (g) + H 2 O(l ...

  6. Thermometric titration - Wikipedia

    en.wikipedia.org/wiki/Thermometric_titration

    An excellent application is the sequential determination of calcium and magnesium. Although calcium reacts exothermically with EDTA (heat of chelation ~-23.4 kJ/mol), magnesium reacts endothermically with a heat of chelation of ~+20.1 kJ/mol. This is illustrated in the titration plot of EDTA with calcium and magnesium in sea water (Figure 14).

  7. Argentometry - Wikipedia

    en.wikipedia.org/wiki/Argentometry

    An example of back titration, the Volhard method, named after Jacob Volhard, involves the addition of excess silver nitrate to the analyte; the silver chloride is filtered, and the remaining silver nitrate is titrated against ammonium thiocyanate, [1] with ferric ammonium sulfate as an indicator which forms blood-red [Fe(OH 2) 5 (SCN)] 2+ at the end point:

  8. Neutralization (chemistry) - Wikipedia

    en.wikipedia.org/wiki/Neutralization_(chemistry)

    For pH control, popular chemicals include calcium carbonate, calcium oxide, magnesium hydroxide, and sodium bicarbonate. The selection of an appropriate neutralization chemical depends on the particular application. There are many uses of neutralization reactions that are acid-alkali reactions. A very common use is antacid tablets.

  9. Kjeldahl method - Wikipedia

    en.wikipedia.org/wiki/Kjeldahl_method

    Thus, one standard solution is needed (e.g. HCl) in the direct titration, while two are needed (e.g. HCl and NaOH) in the back-titration. One of the suitable indicators for these titration reactions is Tashiro's indicator. [3] In practice, this analysis is largely automated; specific catalysts accelerate the decomposition. Originally, the ...