Chemistry Investigated Project for CBSE Class 12 To get the whole "WORD" file DM me at wadhawan.maanit@yahoo.com Or Watsapp- 6389004709 ( INCLUDING COVER PAGE, CERTIFICATE, AKNOWLEDGEMENT,INDEX, THEORY AND BIBLIOGRAPHY)

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2. [2]
This is to certify that <NAME>, a student of class 12,
Roll number <X> has successfully completed the
research project on the topic “Amount of Acetic Acid
Present in Vinegar”, under the guidance of
<TEACHER’S NAME>. The progress of the report has
been continuously reported and been in the
aforementioned teacher’s knowledge consistently.
References taken in making this project have been
declared at the end of the report.
CHEMISTRY TEACHER EXTERNAL EXAMINER

3. [3]
I feel proud to present my investigatory project in
chemistry on the topic “Amount of Acetic Acid
Present in Vinegar”, which aims at investigating
the amount and strength of acetic acid present in
different samples of vinegar. This project would
not have been feasible without the proper and
rigorous guidance of my chemistry teacher
<TEACHER’S NAME>. An investigatory project
involves experiments that are very critical and in
case of failure may result in disastrous
consequences. Thereby I would like to thank our
teacher <TEACHER’S NAME>. and the chemistry
lab assistant for guiding me on a step by step
basis and ensuring that I completed my
experiments with ease. I would also like to thank
my parents and friends for their suggestions and
constructive criticism.

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Acetic acid is the major acid that is found in vinegar.
Acetic acid is also known as Ethanoic acid, and its
molecular formula is C2H4O2. It is found in many other
substances other than vinegar, such as explosives,
sugars, and starch. Acetic acid can be formed in the
atmosphere and it can also be produced when
biological waste decomposes. Humans are regularly
exposed to acetic acid through foods and also from the
air and are not in any danger from this exposure.
Acetic acid by itself is clear and colorless. It gives
vinegar its distinct odor.
In this experiment, the content of acetic acid present in
vinegar was determined by titrating a sample of
vinegar with a base and using phenolphthalein
indicator.
Fig: Structure of Acetic Acid

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One can use this method to find out if the commercial
company/local product maker is actually cheating by
claiming the wrong amount of acetic acid present in
the vinegar. One can also use this method to prevent
buying products which may contain harmful amounts
of acetic acid. In short, this method will help us to
differentiate between genuine and fake products
effectively making our lifestyle healthier.

7. [7]
Vinegar is a solution made from the fermentation of ethanol
(CH3CH2OH), which in turn was previously fermented from
sugar. The fermentation of ethanol results in the production
of acetic acid (CH3COOH)There are many different types of
vinegar, each starting from a different original sugar source
(e.g., rice, wine, malt, etc.). The amount of acetic acid in
vinegar can vary, typically between 4 to 6% for table
vinegar, but up to three times higher (18%) for pickling
vinegar. In this project, we will determine the amount of acid
in different vinegars using titration, a common technique in
chemistry. Titration is a way to measure the unknown
amount of a chemical in a solution (the titrant) by adding a
measured amount of a chemical with a known concentration
(the titrating solution). The titrating solution reacts with the
titrant, and the endpoint of the reaction is monitored in
some way.
The concentration of the titrant can now be calculated from
the amount of titrating solution added, and the ratio of two
chemicals in the chemical equation for the reaction. To
measure the acidity of a vinegar solution, we can add enough
hydroxyl ions to balance out the added hydrogen ions from
the acid.

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The hydroxyl ions will react with the hydrogen ions to
produce water. In order for a titration to work, we need
three things:
o A titration solution (contains hydroxyl ions with a
precisely known concentration),
o A method for delivering a precisely measured volume of
the titrating solution, and
o A means of indicating when the endpoint has been
reached.
For the titrating solution, we’ll use a dilute solution of
Sodium Hydroxide (NaOH). Sodium Hydroxide is a strong
base, which means that it dissociates completely in water. So
for every NaOH molecule that we add to the solution, we can
expect to produce a hydroxyl ion. To dispense an accurately
measured volume of the titrating solution, we will use a
burette. A burette is a long tube with a valve at the bottom
and graduated markings on the outside to measure the
volume contained in the burette.
The burette is mounted on a ring stand, directly above the
titrant solution. Solutions in the burette tend to creep up the
sides of the glass at the surface of the liquid. This is due to
the surface tension of water. The surface of the liquid thus

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forms a curve, called a meniscus. To measure the volume of
the liquid in the burette, always read from the bottom of the
meniscus. In this experiment, we will use an indicator
solution called phenolphthalein. Phenolphthalein is colorless
when the solution is acidic or neutral.
When the solution becomes slightly basic, Phenolphthalein
turns pinkish, and then light purple as the solution becomes
more basic. So when the vinegar solution starts to turn pink,
we know that the titration is complete.
Required amount of sodium hydroxide (NaOH) can be
calculated using the following formula:
W= (0.05 x 40 x 100)/1000
W=2 g
The acetic acid content of vinegar may be determined by
titrating a vinegar sample with a solution of sodium
hydroxide of known molar concentration (molarity).

10. [10]
CH3COOH + NaOH --> CH3COONa + H2O
(Acid) + (Base) --> (Salt) + (Water)
At the end point in the titration stoichiometry between the
both solutions lies in a 1:1 ratio.
Strength of acid in vinegar can be determined by the
following formula:
Strength of acetic acid = MCH3COOH × 60

11. [11]
To do this experiment we will need the following materials
and equipment:
➢ Vinegar, three different types.
➢ Distilled water
➢ Small funnel
➢ 0.5% Phenolphthalein solution in alcohol (pH indicator
solution)
➢ 0.1 M sodium hydroxide solution
➢ 125 mL Conical flask
➢ 25 or 50 mL burette
➢ 10 mL graduated cylinder
➢ Ring stand
➢ Burette clamp

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I. Poured 1.5 ml of vinegar in a conical flask.
II. Added distilled water to dissolve the vinegar so that the
volume of the solution became 20 mL.
III. Added 3 drops of 0.5% phenolphthalein solution.
IV. Used the burette clamp to attach the burette to the ring
stand.
V. The opening at the bottom of the burette should be just
above the height of the conical flask we use for the
vinegar and phenolphthalein solution.
VI. Rinsed the burette with a small amount of NaOH
solution.
VII. Used a funnel to fill the burette with a 0.1 M solution of
sodium hydroxide. Noted the starting level of the
sodium hydroxide solution in the burette.
VIII. Put the vinegar solution to be titrated under the burette.
Slowly dripped the solution of sodium hydroxide into
the vinegar solution.
IX. Swirled the flask gently to mix the solution, while
keeping the opening underneath the burette. At one
point we saw a pink color in the vinegar solution when

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the sodium hydroxide was added, but the color quickly
disappeared as the solution was mixed. When this
happened, we slowed the burette to drop-by-drop
addition. When the vinegar solution turned pink and
retained that color even when mixed, the titration was
confirmed to be complete.
X. Closed the tap (or pinch valve) of the burette. Noted the
remaining level of the sodium hydroxide solution in the
burette.
XI. Subtracted the initial level from the remaining level to
figure out how much titrating solution we have used.
XII. For each vinegar that we tested, repeated the titration
at least three times.

14. [14]
S.NO. Volume of
Vinegar Solution
(in mL)
Burette Reading Volume of
NaOH Solution
used(in mL)
Initial
(in mL)
Final
(in mL)
1. 10 0 13 13
2. 10 13 25 12
3. 10 25 37 12
Concordant Volume=12mL
CALCULATIONS:

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fruit
S.NO. Volume of
Vinegar Solution
(in mL)
Burette Reading Volume of
NaOH Solution
used(in mL)
Initial
(in mL)
Final
(in mL)
1. 10 0 17 17
2. 10 17 33 16
3. 10 33 49 16
Concordant Volume=16mL
CALCULATIONS:

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Strength of acetic acid in laboratory vinegar =
Strength of acetic acid in household vinegar =
ORDER OF AMOUNT OF ACETIC ACID IN DIFFERENT
SAMPLES OF VINEGAR IS:

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 NCERT Class XII Textbook
 Comprehensive Lab Manual
 www.icbse.com
 www.seminarsonly.com
 www.slideshare.com