Project on:

Saturated Solutions:
Moaeurino Sohihilitv
CERTIFICATE

this is to certify that Perghya gautam of class 12th B

has successfully carried out the project entitled
" saturated solution measuring solubility"
under my supervision

ALL THE WORKS RELATED TO THE THESIS WAS DONE BY THE

CANDID HIMSELF.
THE APPROACH TOWARDS THE SUBJECT HAS BEEN SINCERE
AND SCIÄNTIFIC
 ACKNOWLEDGMENT
Iam to Almighty for giving me the strength to
eru conduct my experiment and for sustaining
my efforts which many a times did oscillate.
Iam deeply indebted to Mr Sanjeev bhatnagar sir
our physics faculty without whose constructive guidance
this project would not have been a success. His valuable
advice and suggestions for the corrections,
modifications and improvement did enhance the
perfection in performing my job well.
l am obliged to Mr Suneelour principal for providing
the best of facilities and environment to bring out our
innovation and spirit of inquiry through this venture.
Iam grateful to My Parents and My Brother whose
blessings and wishes have gone a long way in the
completion of this arduous task.
Last but not the least I thank all My Friends and Batch
Mates, without their prompt support my efforts wQuld
have been in vain.
 BASICCONCEPTS

Asaturated solution is a mixture in which no more

solute can be practically dissolved in a solvent at a given
temperature. It is said practical because theoretically
infinite amount of solute can be added to a solvent, but
after a certain limit the earlier dissolved solute particles
start rearranging and come out at a constant rate. Hence
overall it appears that no solute is dissolved after a given
amount of solute is dissolved. This is known as a
saturated solution.
In an unsaturated solution, if solute is dissolved in a
solvent the solute particles dissociate and mix with the
solvent without the re-arrangement of earlier dissolved
solute particles.
Solubility depends on various factors like the Ksp of the
salt, bond strength between the cation and anion,
covalency of the bond, extent of inter and intramolecular
hydrogen bonding, polarity, dipole moment etc. Out of
these the concepts of H-bonding, covalency, ionic bond
strength and polarity play a major role if water is taken
as a solvent.
Also physical conditions like temperature and pressure
also play very important roles as they affect the kinetic
energy of the molecules.
RESULT

The saturated solutions of NaCI, MgSO4 and C12H22011

were made and observed. The observations agreed with
the related theory within the range of experimental error.
PRECAUTIONS

1. While adding the solute to the solvent, the solution

should be stirred slowly so as to avoid the formation
of any globules.
2. Stirring should not be vigorous as the kinetic energy
of the molecules might change due to which solubility
can increase.

3. While stirring, contact with the walls of the container

should be avoided as with every collision, an impulse
is generated which makes the dissolved solute
particles rearrange themselves. As a result solubility
can decrease.
4. The temperature while conducting all the three
experiments should be approximately same.
5. Epsom salt should be first dried in order to remove
the water of crystallization (Mgs04.7H20)
CONCLUSIONS

The solubility of NaClis the highest as it an ionic

salt and easily dissociates in water. Also since the
size of both the cation and anion are small, the
collisions are more and hence probability of
dissociation is high. The solubility of MgSO4 is
also high as it is also an ionic salt, but due to a
larger anion, collisions are not very effective. The
solubility of CizH22011 is the least as it a very
large molecule due to which hydrogen bonding
with the water molecules is not very effective.
Also due to the large number of carbon and
Oxygen atoms, inter molecular H-bonding is more
dominant than intramolecular H-bonding.
Solution of NaCI.
OB$ERVATIONS
Amount of Moles
SALT salt dissolved dissolved
in 100mL
water to make
saturated
solution.
(in gms.)
NaCl(Non 36.8 0.7
lodised
Common Salt)
MgSO4 32.7 0.255

Sucrose(C12H22 51.3 0.15

O1Adding more solute at the same temperature to the
saturated solutions yielded no significant changes in NaC
and Epsom salt. However at all temperatures the
saturation point of sucrose could not be obtained exactly
as due to the large size of the molecule the solution
became thick and refraction was more prominent.
Neglecting this observation in the room for error, the
experiments agreed with the theory. Adding more solute
to heated solutions increased the solubility in all the 3
cases. The largest increase was shown by NaCI, followed
by Epsom salt and sucrose. These facts too agreed with
the theory as at high temperatures the kinetic energy of
molecules increases and the collisions are more effective.
EXPERIMENTAL
PROCEDURE

Determining Solubility
1. Measure 100 mL of distilled water and pour into a
clean, empty beaker or jar.
2. Use the kitchen balance to weigh out the suggested
amount (see below) of the solute to be tested.
3. (a) 50 g Non-iodized table salt (NaC) (b) 50 g
Epsom salts (MgSO4) () 250 g Sugar (sucrose,
Ci2H220i)
4. Add a small amount of the solute to the water and stir
with a clean disposable spoon until dissolved.
5. Repeat this process, always adding a small amount
until the solute will no longer dissolve.
6. Weigh the amount of solute remaining to determine
how much was added to the solution.
7. Try and add more solute at the same temperature and
observe changes if any.
MATERIALS AND
EQUIPMENT
To do this experiment following materials and
equipment are required:
" Distilled water
" Metric liquid measuring cup (or graduated
cylinder)
" Three clean glass jars or beakers
" Non-iodized table salt (NaCI)
Epsom salts (MgS04)
" Sugar (sucrose, Ci2H22011)
"Disposable plastic spoons
Thermometer
" Three shallow plates or saucers
" Oven
" Electronic kitchen balance (accurate to 0.g
INTRODUCTION
Agood part of the substances we deal with in daily life, such
as milk, gasoline,shampoo, wood, steel and air are
mixtures. When the mixture is homogenous, that is to say,
when its components are intermingled evenly, it is called'a
solution. There are various types of solutions, and these can
be categorized by state (gas, liquid, or solid), The chart
below gives some examples of solutions in different states.
Many essential chemical reactions and natural processes
Occur in liquid solutions, particularly those taining water
(aqueous solutions) because so many things di
dissolveeiin
water. In fact, water is sometimes referred to as the
universal solvent. The electrical charges in water molecules
help dissolve different kinds of substances. Solutions form
when the force of attraction between solute and solvent is
greater than the force of attraction between the particles in
the solute. Two examples of such important processes are
the uptake of nutrients by plants, and the chemical
weathering of minerals. Chemiçal weathering begins to take
place when carbon dioxide in the air dissolves in rainwater.
A solution called carbonic acid is formed. The process is
then completed as the acidic water seeps into rocks and
dissolves underground limestone deposits. Sometimes, the
dis:issolving or of minerals in rocks can even lead to the
SouuEOne
formation takes a moment to consider
aqueous solutions, one quickly observes that they exhibit
many interesting properties. For example, the tap water in
your kitchen sínk does not freeze at exactly 0°C. This is
because tap water is not pure water; it contains dissolved
solutes. Some tap water, commonly known as hard water,
contains mineral solutes such as calcium carbonate,
magnesium sulphate, calcium chloride, and iron sulphate.
Another interesting solution property is exhibited with salt
and ice. Another example comes from the fact that salt is
spread on ice collected on roads in winters. When the ice
begins sto melt, the salt dissolves in the water fand
water. The reason is that with the addition
S Sthe
alt
melting point of water increases and as a result the snow
melts away faster. Even some organisms have evolved to
survive freezing water temperatures with natural
"antifreeze." Certain arctic fish have blood containing a high
concentration of a specific protein. This protein behaves like
a solute in a solution and lowers the freezing point of the
blood. Going to the other end of the spectrum, one can also
observe th¡t the boiling point of a solution is affected by the
addition of a solute. These two properties, namely freezing
point depression and boiling-point elevation, are called
OBJECTIVE

The goal of this project is to measure the

solubilities of some common chemicals:
Table salt (NaCI)
Epsom salts (MgSO4)
sugar (sucrose, Ci2H22011).
INDEX

CERTIFICATE
II. ACKNOWLEDGEMENT
III. OBJECTIVE
IV. INTRODUCTION
V. BASIC CONCEPTS
VI. MATERIALS & EQUIPMENT
VIl. EXPERIMENTAL PROCEDURES
VIIL.OBSERVATION
IX. CONCLUSION
X. RESULT
XI. PRECAUTIONS
XI. BIBLIOGRAPHY

SALT
kendriya vidyalaya mathura

Chemistry
Project
Session:2024-25
A Project Report On
Saturated solution measuring solubility

Submittedby Perghya Gautam

Class - XIrÁ (Science)
Roll no. (cbse) -

Under the Guidance of

Mr- Sanjeev sir
PGT (Chemistry)