Abstract:

The results from this experiment show four different Kc equilibrium constants of: .1522 for bottle two, .1853 for bottle three, .2094 for bottle four, and .2678 for bottle five. The average Kc value came out to be .2037 for all four bottles. Purpose:

The purpose of this lab is to determine the equilibrium concentrations of an organic acid, an alcohol, an ester, and water in four bottles with varying measurements of each compound in of the four solutions. Once the concentrations are determined, one is then to discover the Kc, equilibrium constant, of those solutions by dividing the concentrations of alcohol and acid by the concentrations of ester and water. Methods/Procedure:

First begin by mixing up and standardizing a 500mL solution of NaOH to titrate. For each of the six bottles, measure the directed amounts of ester, water, alcohol, and HCl. The bottles of different solutions will be left to come to equilibrium for two weeks. Once the NaOH is standardized, the solutions in the bottles have come to equilibrium, and a molarity is calculated, use the molarity of NaOH to discover how many mols were used to neutralize the solutions in each bottle. Once all of the calculations are complete, use an ICE chart to discover the mols of ester, water, acid, and alcohol at equilibrium to then calculate the Kc for each bottle. After a Kc has been calculated for all bottles, the last step is to determine an average Kc for all of the solutions. Calculations/Results:

Grams of KHP needed:

.7mol x 35ml x 1molKHP x 204gKHP1000ml x 1 x 1molNaOH x 1molKHP=5.00gKHP Grams of NaOH:

.7molNaOH x .500L x 1mol 1L x 1 x 40g~14gNaOH

Mass of dish: 1.80g Mass of bottle 1: 17.1145g Mass of HCl 1: 4.8778g Mass of NaOH 14.0g Mass of bottle 1A: 17.3521g Mass of HCl 1A: 5.2319g Mass of dish: 2.0097g Mass of dish and KHP: 6.0548g Mass of KHP: 5.0378g mL of NaOH used to neutralize KHP: 1. 36.90mL 2. 30.80mL 3. 36.40mL g of KHP: 1. 5.0378g 2. 4.2074g 3. 4.9722g

Molarity of NaOH:

.6690M|

.6689M|

Avg M: .6688M NaOH|

5.0378gKHP x 1molKHP x 1molNaOH x 1 x 1000mL1 x 204.2g x 1molKHP x 36.90mL x 1L=.6686M

mL of NaOH used:

1A: 6.20mL – 24.90mL = 18.70mL|

1: 17.00mL|

2: 60.54mL|

3: 58.60mL|

4: 45.55mL|

5: 40.75mL|

Ethanol: Water:Ethyl Acetate:

Density: .7893g/mL Density: .9982g/mLDensity: .9003g/mL

Molar Mass: 46.07g/molMolar Mass: 18.02g/molMolar Mass: 88.11g/mol mL of solutions in each bottle:

Bottle #| 3M HCl (mL)| H2O (mL)| Ester (mL)| Alcohol (mL)| 1| 5.00| 5.00| 0| 0|

1A| 5.00| 5.00| 0| 0|

2| 5.00| 0| 5.00| 0|

3| 5.00| 1.00| 4.00| 0|

4| 5.00| 3.00| 2.20| 0|

5| 5.00| 2.00| 2.00| 1.00|

Bottles 1 and 1A M HCl:

17.00mLNaOH x .6688molNaOH x 1 molHCl x 11 x 1000ml x 1molNaOH x .005LHCl=2.27MHCL x .005L= .01137molHCl

.01251 molHCl

Average mol HCl of bottles 1 and 1A:

(.01251mol + .01137mol)/2 = .01194molHCl

Mol NaOH for bottles 2-5:

.6688MNaOH x 1L x 60.54mLNaOH1L x 1000mL x 1= .04049molNaOH

.03919molNaOH

.03046molNaOH

.02725molNaOH

Density of HCl:

5.2319gHCl x 11 x 5.00mL=1.046g/mLHCl

Grams of HCl and H2O:

1.046gHCl x 5.00mLH2O1mL=5.230gHCl+H20

Grams of HCl:

.01194molHCl x 36.54gHCl1 mol HCl= .4352gHCl

Grams of HCl and H2O – Grams of HCl:

5.230gHCl+H2O - .4352gHCl = 4.794gH2O from 5.00mL of HCl in bottles 1-5 Grams of H2O made + grams H2O given for bottles 2-5:

4.794gH2O + 0.00mLH2O x .9982gH2O/mL = 4.794gH2O

5.792gH2O

7.789gH2O

6.790gH2O

Grams to mols of H2O for bottles 2-5:

4.794gH2O x 1molH2O1 x 18.02gH2O= .2661molH2O

.3214molH2O

.4322molH2O

.3768molH2O

Mols of ester for bottles 2-5:...