CHM12 Experiment 6 Determination of the Equilibrium Constant for Bromocresol Green

2 clearly indicate in your report the value of the

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: al data tables, calculation tables, graphs, calculations and results. 2. Clearly indicate in your report the value of the equilibrium constant of BCG, Ka, and how you calculated it. Ka can be found from the yintercept (B): B = log (Ka) Ka = 10B 3. When we calculate the pH of the solutions it’s found by using the following equation: pH=pK+log (moles sodium acetate ) (moles acetic acid) Bromocresol green is a weak acid, just like acetic acid. But our calculations assume that bromocresol green doesn’t affect the overall acidity (pH) of the acetate solution. Why is this a good assumption? To prove this point, calculate the number of moles of bromocresol green (the indicator itself) in the sodium acetate solution and compare this number to the number of moles of sodium acetate and the number of moles of acetic acid used. 4. Type a discussion of your primary result. Compare your result to literature values. Discuss the accuracy of your result. Be sure to list the sources of your literature values. 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 12...
View Full Document

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.

Ask a homework question - tutors are online