Project on solubility of saturated solution for class 12th

Today we will see how to make project on 'Project on solubility of saturated solution for class 12th' this project is only for class 12th student and this project is belongs to 'solution' in this project we will cover following steps


1. OBJECTIVE

2. INTRODUCTION

3. BASIC CONCEPTS

4. MATERIALS & EQUIPMENT

5. EXPERIMENTAL PROCEDURES

6.OBSERVATION

7. CONCLUSION

8. RESULT

9. PRECAUTIONS


10. BIBLIOGRAPHY

                 OBJECTIVE

The goal of this project is to measure the solubilities of some common chemicals:

Table salt (NaCl)

Epsom salts (MgSO4)


sugar (sucrose, C12H22O11).

               INTRODUCTION

A good 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 containing water
(aqueous solutions) because so many things dissolve in
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. Chemical 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
dissolving of soluble minerals in rocks can even lead to the
formation of caves. If one takes a moment to consider
aqueous solutions, one quickly observes that they exhibit
many interesting properties. For example, the tap water in
your kitchen sink 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 to melt, the salt dissolves in the water and forms salt
water. The reason is that with the addition of salt the
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 that the boiling point of a solution is affected by the
addition of a solute.

                BASIC CONCEPTS

A saturated 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.

      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 (NaCl)
• Epsom salts (MgSO4)
• Sugar (sucrose, C12H22O11)
• Disposable plastic spoons
• Thermometer
• Three shallow plates or saucers
• Oven

• Electronic kitchen balance (accurate to 0.1 g)

  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 (NaCl) (b) 50 g Epsom salts (MgSO4) (c) 250 g Sugar (sucrose, C12H22O11)

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.

8. Now heat the solutions and add more solute to the

solutions.

                  OBSERVATIONS

SALT                Amount of salt dissolved             Moles 

                            in 100mL water to make          dissolved      

                              saturated solution.

                                    (in gms.)

NaCl (Non-                    36.8                                   0.7

Iodised

Common Salt)

MgSO4 32.7 0.255      51.3                                     0.15

Sucrose(C12H22 

O11)

Adding more solute at the same temperature to the

saturated solutions yielded no significant changes in NaCl

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 NaCl, 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.

             CONCLUSIONS

The solubility of NaCl is 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 C12H22O11 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 NaCl.

                 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 (MgSO4.7H2O)

                     RESULT

The saturated solutions of NaCl, MgSO4 and C12H22O11

were made and observed. The observations agreed with

the related theory within the range of experimental error.

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