Solutions jee

Molarity and mass %

Molarity and molality

Molality and mole fraction

Molarity and mole fraction

For Solubility of a solid in a liquid the endothermic dissolution favours

Solubility increases with increase in temperature

For solubility of a solid in liquid effect of pressure

Pressure has no effect

Henry’s law

Partial pressure of a gas in vapour phase is proportional to mole fraction of the gas in the solution.

Raoult’s law

For a solution of volatile liquids the partial pressure of each component in the solution is directly proportional to its mole fraction

Dalton’s law of partial pressure

Raoults law for volatile solvent and non volatile solute

Ideal solution

Binary liquid solutions of volatile components which obey raoults law over the entire range of concentration

For an ideal solution the solvent solute interaction (A-B) is

Nearly Same as AA and BB interaction

For an ideal solution heat and volume mix change is

Examples of ideal solutions

Benzene + ______

N hexane +_______

Ethylbromide +________

Chloro benzene +________

Toluene

N heptane

Ethyl iodide

Bromobenzene

Mole fraction in vapour phase of an ideal solution

Solutions which show positive deviation of from raoults law

Examples of solitons with positive deviations

(12)

Acetone + ethanol

Acetone + cs2

Acetone + ccl4

Acetone + benzene

Cyclohexane + ethanol

Cyclohexane + benzene

Methanol + h2O

Ethanol + h2O

Propanol + h2O

Ccl4 + toluene

Ccl4 + chloroform

Ccl4 + Methanol

Solutions that show negative deviation form raoults law

Azeotropes

Binary mixture that have same composition. In liquid and vapour phase and boil at a constant temperature

Minimum boiling azeotrope

Show large positive deviation from raoults law. In this car booking point of azeotrope is less than that of components

Example of min boiling azeotrope

Maximum boiling azeotrope

Solutions which show large negative deviation n from raoults law. Boiling point of azeotropes in greater that that of its components

Example of max boiling azeotrope

Relative lowering of vapour pressure for dilute solutions

Relative lowering of vapour pressure for not dilute solution

Elevation of boiling point

Relation between molal elevation constant and enthalpy of vapourisation

Depression of freezing point

Principle of pressure cooker

Elevation of boiling point

Applications of depression of freezing point

Back of anhydrous cacl2 use to clear snow , this is because they depress the freezing point of h2o to such an extent that it cannot freeze to form ice

35% of V/v aquous solution of ethylene glycol (antifreeze) as a coolant in automobile radiators

Osmosis

The spontaneous movement of solvent molecules form lower to higher concentrations (or viceversa) through semi preameable memberane

Osmotic pressure

The excess pressure that must be applied to solution side to stop osmosis

Why use osmotic pressure method

because it is easier to find out the molecular mass of macro molecules and polymers as it is more accurate and can be measure at room temp

Isotonic solutions

Solutions with same osmotic pressure at a particular temperature

Ex - 0.9 % mass / volume back solution and blood

Hypertonic solution

Higher osmotic pressure

Plasmolysis or crenation

Shrinking of plant cells due to exo osmosis when placed in a hypertonic solution

Edema

People taking a lot of slat or salty food experiences water retention in tissues and inter cellular spaces due to osmosis, the resulting puffiness or selling is called edema

Reverse osmosis

When we apply greater pressure that osmotic pressure to the solution side then the solvent molecules migrates from solution to pure solvent through the spm

Used in desalination of sea water

Abnormal molecular mass

Due to dissolution of solute the number of particles and colligative particles increases so the resultant molecular mass will be lower the original

Similarly in association it will be grater that that of actual molecular mass

vant hoff factor

i > 1 dissociation

i = 1

Urea , sugar , glucose , ethanol

Acetic and benzoin acid

Associates in benzene but dissociate in water

Collogative property and i

Degree of association or dissociation

It is the fraction of total number of mole that undergo association or dissociation

Degree of dissociation and i

Degree of association and i