CHM12 Experiment 6 Determination of the Equilibrium Constant for Bromocresol Green

# Finding the molarity of acetic acid hc2h3o2 in

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Unformatted text preview: olution used in dilution in liters (1000 mL = 1L) Moles of sodium acetate solution used in dilution (n = MV) 2. Finding the molarity of acetic acid (HC2H3O2) in solution B Molarity of acetic acid solution on bottle Volume of acetic acid solution used in dilution in milliliters Volume of acetic acid solution used in dilution in liters Moles of acetic acid solution used in dilution (n = MV) Total volume of solution in dilution in milliliters Total volume of solution in dilution in liters (1000 mL = 1 L) Molarity of acetic acid in diluted solution (M = n/V) Department of Physical Sciences Kingsborough Community College The City University of New York Spring 2012 Experiment 6: Determination of the Equilibrium Constant for Bromocresol Green 9 1. Moles of Acetic Acid Now we need to calculate the number of moles of acetic acid each time we added 2.00 mL of acetic acid solution to the bromocresol green solution in Part 2. The volume of acetic acid solution added was 2.00 mL through 8.00 mL. Convert these volumes to liters. The molarity of the acetic acid solution was calculated on the previous page and is the same for each addition. The moles of acetic acid added can be found from n = MV. Volume of Acetic Acid Solution Added (mL) Volume of Acetic Acid Solution Added (L) Molarity of Acetic Acid Solution (mol/L)* M = n/V Moles of Acetic Acid Added (mol) 2.00 mL 4.00 mL 6.00 mL 8.00 mL *From the previous page. This amount should be the same for each addition. 2. Moles of Sodium Acetate (NaAc) We also need to know the number of moles of sodium acetate used in the mixture for Part 2. This was calculated on the previous page. 3: Calculating the pH of the acetate solutions The following table shows the progression of the calculations needed to find the pH of each solution in Part 2. We first use the moles of the acetic acid and the moles of sodium acetate (already calculated) to find the ratio of sodium acetate to acetic acid. We then take the log (base 10) of this ratio. The pH of a mol NaAc . The pKa for mol HAc solution that contains a weak acid and its conjugate base is: pH = pKa + log acetic acid is 4.74. Find the pH of each solution. Volume of Acetic Acid Solution Added (mL) 2.00 mL Moles of Acetic Acid* (mol) Moles of Sodium Ace...
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## This note was uploaded on 02/11/2014 for the course CHEM 12 taught by Professor Patricklloyd during the Spring '13 term at CUNY Kingsborough Community College.

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