EXPT 10:

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Experiment 10 - Acid-Base Titrimetry


  1. To standardize an acid, HCl, solution.
  2. To determine the concentration of an unknown Na2CO3, sodium carbonate solution.


Alkaline conditions are found in many natural waters and may arise in boiler water due to the accumulation of calcium carbonate and other minerals derived from the water supply.

Since the alkalinity is due to a mixture of substances, no single neutralization reaction can be written. The sample is simply titrated to pH 4.6, and the result calculated as if all of the alkalinity is due to calcium carbonate.

This experiment involves the titration of sodium carbonate, Na2CO3, by a strong acid, HCl. 

Na2CO3 (aq) + 2 HCl (aq) 2 NaCl (aq) + CO2 (g) + H2O (l)

Note that each mole of carbonate requires two moles of acid for complete titration.  Titration to the bromocresol green end-point ensures that all of the carbonate are converted to CO2 and H2O.

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