For a solution of the gases A, B, C and D in water at 298 K, the values of Henry's law constant (KH) are 30.40, 2.34, 1.56 $$\times$$ 10$$-$$5 and 0.513 k bar respectively. In the given graph, the lines marked as 'p' and 's' correspond respectively to :
Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).
Assertion (A) : At 10$$^\circ$$C, the density of a 5 M solution of KCl [atomic masses of K & Cl are 39 & 35.5 g mol$$-$$1 respectively], is 'x' g ml$$-$$1. The solution is cooled to $$-$$21$$^\circ$$C. The molality of the solution will remain unchanged.
Reason (R) : The molality of a solution does not change with temperature as mass remains unaffected with temperature.
In the light of the above statements, choose the correct answer from the options given below :
Solute A associates in water. When 0.7 g of solute A is dissolved in 42.0 g of water, it depresses the freezing point by 0.2$$^\circ$$C. The percentage association of solute A in water, is :
[Given : Molar mass of A = 93 g mol$$-$$1. Molal depression constant of water is 1.86 K kg mol$$-$$1.]