Laboratory assignment for module 4: equilibrium constants


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Thomas Edison State College

General Chemistry II with Labs (CHE-122)

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Laboratory Assignment for Module 4: Equilibrium Constants
(eScience Lab 5 [17])




I.       PURPOSE (10 POINTS)








Table 1. Equilibrium Constants Data

Syringe Reading, mL

pH after each 0.5 mL increment

Color Observations




















































Volume of NaOH when solution turns dark pink/orange:


Volume of NaOH at the equivalence point (the point on the graph midway between the vertical rise; see Lab 7 [19], Figure 2):


pH at the equivalence point (should be approximately 8–9):


Volume of NaOH at equivalence point:


Volume at half-equivalence point:


pH at the half-equivalence point:

pH = pKa  at this point


Ka (equilibrium constant):

pKa = –log Ka                                    



Show calculations









Experimental Ka of acetic acid:



Theoretical Ka of acetic acid:












1.      Compare your experimental value for the equilibrium constant to the theoretical value. Do you notice any variation? If so, why? (10 points)


2.      Write the dissociation of acetic acid, HC2H3O2.(10 points)




3.      Write the equilibrium expression for acetic acid. (10 points)


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