CHEM 1B Chapter Notes - Chapter 8: Burette, Antacid, Titration
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CHEM 1B Full Course Notes
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Antacid tablets (tums) dissolved in excess hcl and titrated with naoh. Final volume in the burette (ml) (light pink end point) Millimoles of hcl reacted with millimoles of naoh. Identify the active ingredient in the antacid from the manufacturer"s label. Write the balanced equation for the base in the antacid reacting with hcl. Calculate the mass of caco3 in the antacid tablet. Calculate actual % caco3 in the antacid tablet, which is (mass of caco3/mass of tablet) x 100. % deviation=| (500 mg experimental mass of caco3) 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.
