Chemisorption increases and physisorption decreases with rise in temperature.

Coagulation is generally brought about by the addition of electrolytes. When an electrolyte is added to a colloidal solution, the particles of the sol take up the ions which are oppositely charged. As a result their charge gets neutralised.
Electrophoresis The movement of colloidal patticles under an applied electric potential is called electrophoresis.
Electroosmosis may be defined as a phenomenon in which the molecules of the dispersion medium are allowed to more under the influence of an electric field whereas colloidal particles are not allowed to more.
Tyndall effect is the scattering of light by sol particles, which cannot be affected by charge on them.

Lyophilic colloids have a unique property of protecting lyophobic colloids. When a lyophilic sol is added to the lyophobic sol, the lyophilic particles form a layer around lyophobic particles and thus protect the latter from electrolytes. Lyophilic colloids used for this purpose are called protective colloids

Colloidal gold is prepared by Bredig's arc method.

Micelles are the clusters formed by the association of colloids. They are formed by lyophilic and lyophobic groups. As the concentration increases, the lyophobic parts receding away from the solvent approach each ( non-polar part ) other and form a cluster, the lyophobic ends are in the interior, lyophilic groups ( polar part ) projecting outward in contact with the solvent.

Lyophobic sol is protected since a film of lyophilic sol is formed over lyophobic sol.

Chemisorption first increases with temperature as it requires energy of activation.

The separation of an emulsion into its constituents is called demulsification. Various methods of demulsification are freezing, boiling, centrifugation or chemical methods.

Let the weight of acetic acid initially be w₁ in 50 ml of 0.060 N solution.
$$\eqalign{ & {\text{Let}}\,{\text{the}}\,N = \frac{{{w_1} \times 1000}}{{M.wt. \times 50}}\,\,\,\,\,\,\,\,\left( {{\text{Normality}} = 0.06\,N} \right) \cr & 0.06 = \frac{{{w_1} \times 1000}}{{60 \times 50}} \cr & \Rightarrow \,\,\,{w_1} = \frac{{0.06 \times 60 \times 50}}{{1000}} \cr & = 0.18\,g \cr & = 180\,mg. \cr} $$
After an hour, the strength of acetic acid = 0.042 N
so, let the weight of acetic acid be w₂
$$\eqalign{ & N = \frac{{{w_2} \times 1000}}{{60 \times 50}} \cr & 0.042 = \frac{{{w_2} \times 1000}}{{3000}} \cr & \Rightarrow {w_2} = 0.126\,g \cr & = 126\,mg \cr} $$
So amount of acetic acid adsorbed per 3g
= 180 -126 $$mg$$  = 54 $$mg$$
Amount of acetic acid adsorbed per g
$$ = \frac{{54}}{3} = 18mg$$

Greater the surface area, greater the van der waal forces of attraction and therefore at lesser concentration micelle formation will take place. In case of $$C{H_3}{\left( {C{H_2}} \right)_{15}}\mathop N\limits^ \oplus {\left( {C{H_3}} \right)_3}B{r^ - }$$      due to greater chain length, greater will be van der waal forces.