acidcontentofacommericlasodalabreport

# acidcontentofacommericlasodalabreport - moles of NaOH used...

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Week of October 6, 2008 CH116-J1 Acid Content of a Commercial Soda 1. Experimental Procedure . a. The KHP solution was prepared by first dissolving a weighed sample of KHP in 50 mL of water in an Erlenmeyer flask, with a couple drops of phenolphthalein. Then a 50-mL buret was filled with an aqueous NaOH solution, and titrated with the KHP solution until a pink end-point is seen. This was repeated three times, for three different KHP-sodium hydroxide solutions, to find the molarity of the NaOH. b. A 50-mL buret was then filled with NaOH, and titrated with 10 mL of an uncarbonated, light colored soda with a few drops of phenolphthalein added, until a pink end-point is seen. 2. Conceptual Basis of Calculation . To determine the acid concentration of the soda, chemical andmathematical equations were used. The equation M = moles/L was first used to find the molarity of the NaOH used in the titrations. To use it, the moles of KHP used were divided by the liters of NaOH used to titrate the KHP. The liters of NaOH used to titrate the soda were then multiplied by the molarity of NaOH to find the

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Unformatted text preview: moles of NaOH used to titrate the soda, to find H 3 Cit. Because there is 1 mole H 3 Cit to 3 moles NaOH, the moles of NaOH is multiplied by 3and then divided by the liters of soda used, which is 0.01 L. The result is the molarity of H 3 Cit. H 3 Cit (aq) + 3NaOH (aq) Na 3 Cit (aq) + 3H 2 O (l) 3. Acid Concentration in Soda . The acid concentration of soda is 0.08199 ± 0.00091 M. The reported uncertainty is acceptable because of the small standard deviation. 4. Acid Content in Other Consumables . The acid concentration of an orange is 0.0001 M and a lemon, 0.1 M. The acid concentration of soda is between that of an orange and lemon, two fruits which are none to be harmful to teeth, so soda must be harmful as well. 5. Effects of the Carbonation . Carbonation must be removed from the soda prior to the titration because the escape of a gas from the solution removes ions, which are the basis of pH....
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## This note was uploaded on 08/07/2009 for the course CH 116 taught by Professor March during the Spring '09 term at University of Alabama at Birmingham.

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acidcontentofacommericlasodalabreport - moles of NaOH used...

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