CHEM 1B Chapter Notes - Chapter 8: Antacid, Titration, Chemical Equation
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CHEM 1B Full Course Notes
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In this experiment, the amount of calcium carbonate (caco3) in a tums tablet was determined by a back titration. A back-titration was necessary because caco3, the active ingredient in tums, is relatively insoluble in water. The antacid tablet used in this experiment was dissolved in 50 ml of excess hcl, allowing the remaining hcl to react with the naoh titrated slowly into the solution. By determining the volume of hcl that reacted with naoh to form a neutral solution, the amount of acid that was consumed in the reaction with the antacid can be calculated. This value was calculated to be 10. 005 millimoles of hcl. Using this number, the amount of caco3 present in the tums tablet can be calculated. The reaction that occurred when the antacid tablet was dissolved in hcl is as follows: Caco3(s) + 2hcl(aq) cacl2(aq) + co2(g) + h2o(l) The net ionic equation for the reaction that then occurred in the titration is as follows:
