Solutions

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(ii) Water will  move from side (B) to side (A) if a pressure greater than osmotic pressure is applied on piston (B).

Explanation:  Due to reverse osmosis, water will travel from side (B) to side (A) if a pressure greater than osmotic pressure is applied to the piston (B).

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(ii) Greater for gases with lower solubility.

Explanation : Because of the mathematical relationship, the value of Henry's constant K_H is bigger for gases with lesser solubility-

p= k_H x

k_H=p/x

Where, K_H represents Henry's constant, p is partial pressure of the gas in vapour phase, and x denotes mole fraction of  the gas in solution. Thus K_H is inversely proportional to mole fraction of gas in solution (representing  its solubility)

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(i) Increases with increase in temperature.

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(ii) In reverse osmosis, solvent molecules move through a semipermeable membrane from a region of lower concentration of solute to a region of higher concentration.

Explanation:

Solvent molecules pass through a semipermeable membrane in reverse osmosis from an area of higher solute concentration to a region of lower concentration, hence the supplied assertion at (ii) is untrue. 

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(ii) 2, 2 and 3

Explanation: The van't Hoff factor's values are determined by the degree of dissociation. Strong electrolytes include KCl, NaCl, and K₂SO₄. When compared to KCl and NaCl, the extent or degree of dissociation with Na₂SO₄ is the largest. 

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(i) Two different solutions of sucrose of the same molality prepared in different solvents will have the same depression in freezing point.

Explanation: T_f = K_f m

The dip in freezing the point of the solution would not be the same since K_f values are dependent on the composition of the solvent.

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(i) Is higher than that at a dilute solution.

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(iv) It loses water due to osmosis.

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(iii) About three times

Explanation:  A colligative property is a decrease in freezing point. In the case of MgCl₂, the van't Hoff factor will be higher. When a molecule of MgCl₂ dissociates in its aqueous solution, it produces 3 ions. One molecule of 0.01M MgCl₂ produces three particles/ions in solution, resulting in a threefold increase in the number of particles present in the solution. As a result, the freezing point of 0.01M MgCl₂ will be three times lower than that of 0.01M glucose solution, because there will be no dissociation of the molecule.