Category: chemistry

Emulsion is the type of colliodal mixture :- In which the dispersion medium is oil and dispersed phase is water. for example ‘Butter’ In which the dispersion medium is water and dispersed phase is oil. for example ‘milk’ . Applications or examples of emulsification In case of cleaning action of soap, the soap solution acts

On the application of electric field , the colloidal particles move towards the oppositely charged electrode. on reaching at the electrode , the particles get discharged and they coagulate there. this process is also known as the Electrophoresis.

Soaps and detergents are associated colloids.

In case of chemisorption there is a partial bond like interaction between the adsorbate and adsorbent . During such an interaction the higher amount of energy is required because bond formation and breaking will require more energy. but on the other hand in case of physisorption the adsorbate and adsorbent particles are simply held together

In case of As2S3 the colloidal particles scatter the light passing through solution and show Tyndall effect.

In case of enzyme catalyst , they have specific sites for the attachment of substrate or the reactant. Any other molecule or substrate can not join with the catalyst. here is a diagram to show the phenomenon.

Multimolecular colloids :- These kind of colloids are formed when many small molecules or atoms are forced to aggregate in the dispersion medium. Thses colliods are lyophobic (solvent hating) in nature. for example gold solution Macromolecular colloids :- These are colloids which are formed of such a molecules which are enough large to have colloidal

the depression in freezing point (which is a colligative property) depends upon the number of solute particles present in the solution. when sodium chloride is mixed in the water it dissociates into Na+ and Cl– ions thus this increases the number of particles . but glucose don’t dissociate and its freezing point is higher than

The elevation in boiling point depends upon the number of solute particles present in the solution. when sodium chloride is mixed in the water it dissociates into Na+ and Cl– ions thus this increases the number of particles . but glucose don’t dissociate and its boiling point is lower than Sodium chloride.

Molality of the given solution = 0.1539m ∆Tf = 273.15 – 271 = 2.15 K Therefore ∆Tf  = Kf .m Kf = ∆Tf / m Kf = 2.15/0.1539  Now mass of the solute W2 = 5g Molar mass of the solute M2 = 180g Mass of the solution W1 = 100g  Now the mass of

Solution:- Mass of ethylene glycol (solute) = 222.6 g Molar mass of ethylene glycol ( C2H4(OH)2 = 62g Number of moles of the solute = 222.6 / 62  = 3.59 moles Mass of the solvent (water) in solution = 200g = 0.200Kg Volume of the solution = 422.6 / 1.072 = 394.2 ml                                                 =

In case of zinc its outer d-subshell is fully filled. So it can not make interatomic bonds like the other elements of the same transition series. The other elements with partially filled d-subshell can undergo multiple metallic bonds . Thus the enthalpy of atomization in case of Zinc ix the lowest.

In case of silver , it involves the filling of outer 4d sub shell in its outer shell in its ground state. Moreover its ion is Ag+ . its outer configuration and its behavior matches with the d-block elements thus it is placed in transition metals.

Acetic acid is a weak electrolyte , and in case of weak electrolytes , their molar conductivity keeps on increasing on dilution . we can not achieve a constant value. Thus its is difficult to explain the molar conductivity of acetic acid.

Solution The mixtures showing positive and negative deviations are as follows:- Mixtures showing positive deviation is mixture of ethanol and acetone. The reason behind this is :- in this case the solute and solvent interactions are weaker than the solute-solute and solvent-solvent interactions. Mixtures showing negative deviation is mixture of chloroform and acetone. The reason

Solution :-

this question is solved as follow :-