Unit 4 Learning Aim B Year 12 L3 BTEC
In this assignment I will be describing the industrial manufacturing and testing of organic
liquids. Analysing and concluding on my test for purity on a organic liquid ,comparing
the production and testing of an organic liquid in a lab and an industrial setting. I will be
demonstrating my skillful application of techniques in preparing and testing the purity of
an organic liquid and draw detailed conclusions.I will examine the elements influencing
an organic liquid's purity and yield in the lab and how they apply to the production of the
liquid in industry.
I will now be explaining the method we used in the laboratory to prepare ethyl
ethanoate using the esterification method.
The reaction principle of esterification is where a carboxylic acid reacts with an alcohol
to produce a ester and water. The techniques used are separation , syntheses ,
purification and analysis of results. The aim of this practical is to find out how
successful the results are.
Preparing Ethyl Ethanoate
An ester is an organic material that reacts with water to form alcohols and organic/
inorganic compounds.
Esterification is the process of combining an organic acid with an alcohol to form a
ester and water. It does this by separating ethyl ethanoate and water through distillation.
The goal of this practical is to use the method esterification to turn a carboxylic acid into
an ester. Reflux is the condensation of vapours, while distillation is the separation of
liquids by cooling and heating.
Here is the equation for the esterification of a carboxylic acid :
C 2 H 5 OH ( l ) Ethanol + CH 3 COOH ( aq ) Ethanoic acid → conc . H 2 SO 4 CH 3
COOC 2 H 5 ( l ) Ethyl ethanoate + H 2 O ( l ) Water.
*Equipment list
50 cm round bottomed flask with delivery arm
Thermometer
Condenser
1
,Unit 4 Learning Aim B Year 12 L3 BTEC
250 cm* besker
Clamp and stand
Bung
Electric hester
Dropping pipette
Messuring cylinder
Access to a tap and sink
Chemicals required
o Ethanoic acid
o Ethanol
o Concentrated sulfuric acid
o Sodium carbonate
o Calcium chloride solution
Method
1. Set up the apparatus as shown in figure one below. The round bottom flask
should be held in a clamp stand and the condenser should be connected to the
round bottomed flask vis the delivery tube. Set up the condenser so it is at an
angle just below horizontal, with water entering at the bottom. Place a beaker at
the open end of the condenser.
2. Add 10 cm: ethanol, 12 cm ethanoic acid and 15 drops of concentrated sulfuric
acid to the round bottom.
3. Reconnect the round bottomed flask to the rest of the apparatus. Turn on the tap
for the condenser.
4. Gently heat the mixture using an electric heater. The ester will evaporate and
condense in
5. 5. Stop testing when no more esters seem to be vaporising.
Small quantities of sulfuric acid, ethanol and ethanoic acid may also have
collected in the beaker. Add sodium carbonate to the solution to remove any
acidic impurities. Stop adding sodium carbonate when the solution stops fizzing.
Add calcium chloride solution to remove the ethanol.
The image below is how the practical was set up.
2
, Unit 4 Learning Aim B Year 12 L3 BTEC
In order to conclude the yield of ethyl ethanoate I needed to calculate the moles of
ethanol
1:1 molar ratio
C4 H8 O2=(4x12.01) + (8 x1.01) + (2x16)=88.1g/mol
Ethanol=10cm3
Ethanoic acid = 12cm3
Mr of C2H608 =46
10/46=0.22 mol
88.1 x 0.22= 19.382
Actual yield
16.91 - 10.61=6.3g
Percentage yield = actual yield / theoretical yield x100
6.3/19.382 x100= 18.57%
Testing the purity through measuring the boiling point
3
In this assignment I will be describing the industrial manufacturing and testing of organic
liquids. Analysing and concluding on my test for purity on a organic liquid ,comparing
the production and testing of an organic liquid in a lab and an industrial setting. I will be
demonstrating my skillful application of techniques in preparing and testing the purity of
an organic liquid and draw detailed conclusions.I will examine the elements influencing
an organic liquid's purity and yield in the lab and how they apply to the production of the
liquid in industry.
I will now be explaining the method we used in the laboratory to prepare ethyl
ethanoate using the esterification method.
The reaction principle of esterification is where a carboxylic acid reacts with an alcohol
to produce a ester and water. The techniques used are separation , syntheses ,
purification and analysis of results. The aim of this practical is to find out how
successful the results are.
Preparing Ethyl Ethanoate
An ester is an organic material that reacts with water to form alcohols and organic/
inorganic compounds.
Esterification is the process of combining an organic acid with an alcohol to form a
ester and water. It does this by separating ethyl ethanoate and water through distillation.
The goal of this practical is to use the method esterification to turn a carboxylic acid into
an ester. Reflux is the condensation of vapours, while distillation is the separation of
liquids by cooling and heating.
Here is the equation for the esterification of a carboxylic acid :
C 2 H 5 OH ( l ) Ethanol + CH 3 COOH ( aq ) Ethanoic acid → conc . H 2 SO 4 CH 3
COOC 2 H 5 ( l ) Ethyl ethanoate + H 2 O ( l ) Water.
*Equipment list
50 cm round bottomed flask with delivery arm
Thermometer
Condenser
1
,Unit 4 Learning Aim B Year 12 L3 BTEC
250 cm* besker
Clamp and stand
Bung
Electric hester
Dropping pipette
Messuring cylinder
Access to a tap and sink
Chemicals required
o Ethanoic acid
o Ethanol
o Concentrated sulfuric acid
o Sodium carbonate
o Calcium chloride solution
Method
1. Set up the apparatus as shown in figure one below. The round bottom flask
should be held in a clamp stand and the condenser should be connected to the
round bottomed flask vis the delivery tube. Set up the condenser so it is at an
angle just below horizontal, with water entering at the bottom. Place a beaker at
the open end of the condenser.
2. Add 10 cm: ethanol, 12 cm ethanoic acid and 15 drops of concentrated sulfuric
acid to the round bottom.
3. Reconnect the round bottomed flask to the rest of the apparatus. Turn on the tap
for the condenser.
4. Gently heat the mixture using an electric heater. The ester will evaporate and
condense in
5. 5. Stop testing when no more esters seem to be vaporising.
Small quantities of sulfuric acid, ethanol and ethanoic acid may also have
collected in the beaker. Add sodium carbonate to the solution to remove any
acidic impurities. Stop adding sodium carbonate when the solution stops fizzing.
Add calcium chloride solution to remove the ethanol.
The image below is how the practical was set up.
2
, Unit 4 Learning Aim B Year 12 L3 BTEC
In order to conclude the yield of ethyl ethanoate I needed to calculate the moles of
ethanol
1:1 molar ratio
C4 H8 O2=(4x12.01) + (8 x1.01) + (2x16)=88.1g/mol
Ethanol=10cm3
Ethanoic acid = 12cm3
Mr of C2H608 =46
10/46=0.22 mol
88.1 x 0.22= 19.382
Actual yield
16.91 - 10.61=6.3g
Percentage yield = actual yield / theoretical yield x100
6.3/19.382 x100= 18.57%
Testing the purity through measuring the boiling point
3
