Equilibrium Constant of an Ester Hydrolysis Reaction Essay examples

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The Equilibrium Constant of an Ester Hydrolysis Reaction


The first step in determining the equilibrium constant of an ester hydrolysis

reaction is to prepare five different reaction mixtures with the volume given in

Table 1. the bottles have different mixtures of HCl, H2O, an unknown ester, and

one bottle has alcohol. We will later determine the equilibrium constant for the

reaction between the unknown ester and water to produce an unknown alcohol,

and unknown acid. Once the bottles were shooken vigorusly we stored them in

our drawer until chemical equilibrium was reached, which took about two weeks.

We were then to make a base solution of 0.7 M NaOH. In order to standardize

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The equilibrium constant

formula is simple, multiply the concentrations of the products and divide that

by the concentraions of reactants multipled. So what we need to do is find the

concentrations, or molarity, and we have all the tools in order to do that from the



The first thing we needed to do to start this expirament was to prepare five

different bottles, each with a specific amount of reaction mixtures as shown in

Table 1. We used 3.0 M HCL at a constant of 5.0 ml in every bottle.HCL already

has a little water in it but we did add more deionized H20 to different bottles. We

also had an unknown ester sample we received from the stockroom and an

alcohol sample. Once the bottles were prepared, we needed to make a base

for titrating the mixtures after equilibrium. The amount of sodium needed to

prepare 0.5 L of a .7 M NaOH solution was about 14 grams, so we weghed out

14g of MaOH pellets and dissolved them in deionized water and let them

dissolve. The total solution was approximatley 500 ml. The amount of potassium

hydrogen phthalate (KHP) needed to neutralize 35 ml of the base we made was

about 5 grams. We dissolved the KHP in 50 ml of deionized water. Aftr adding

some phenolphthalein we could triate with the base three different times and

take the average molarity, and our base is then standardized. After

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