CHEM 1&2 Lab Manual & worksheets pg 163

CHEM 1&2 Lab Manual & worksheets pg 163 -...

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Experiment 15: Titration of Vinegar General Chemistry I and II Lab Manual Dakota State University page 163 of 232 weaker than the original vinegar. To take this dilution factor into account, multiply the concentration of the diluted sample by 10 to get the concentration of the original vinegar. Titration of the Acid: Measure out 10.00 mL of the diluted solution using a pipette. If your lab instructor requests you to do so, add a couple of drops of phenolphthaliene. Titrate the sample either to the endpoint, or using the Pasco system to collect data as your lab instructor requests. Perform at least three titrations; if any of the runs are off by more than 0.04 mL from any other run, perform a fourth titration and discard the titration that seems to most significantly disagree with the other runs. Determine the concentration of
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Unformatted text preview: the acid from this step. Calculations: Standardization: KHP is a monoprotic acid, so the reaction can be simplified as KHP (aq) + NaOH (aq) & KNaP (aq) + H 2 O (l) Using standard stoichiometric techniques, calculate the molarity of NaOH for each run. Take the average and determine the standard deviation. Concentration of the Acetic Acid: The acid is monoprotic, so again, we can write HA (aq) + NaOH (aq) & NaA (aq) + H 2 O (l) Use standard stoichiometric techniques to calculate the moles of acid for each run. Don’t forget to take the dilution into account; once you calculate the concentration of acetic acid in the diluted solution, multiply by four to get the concentration of the original vinegar. Convert the concentration from molarity to % w/v in the standard method. Take the average and determine the standard deviation....
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This note was uploaded on 01/27/2012 for the course CHM 2045 taught by Professor Josephwalter during the Fall '11 term at Dakota State.

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