Solutions practice · Medium

Assertion (A): Azeotropic mixtures are formed only by non-ideal solutions.

Reason (R): The composition of the vapour phase is same as that of the liquid phase of an azeotropic mixture.

Statement I: Molarity of a solution is always greater than that of molality.

Statement II: Ratio of molarity and molality depends on density of solvent.

Relation between partial pressure and mole fraction is stated by

A solution which boils at constant temperature is called:

One component of a solution follows Raoult’s law over the entire range $0 \le {x_1} \le 1$ . The second component must follow Raoult’s law in the range when ${x_2}$ is

Total vapour pressure of mixture of 1 mol of volatile
Component A $\left( {P_A^\mathrm{o} = 100\,\,mm\,Hg} \right)$ and 3 mol of volatile
Component B $\left( {P_B^\mathrm{o} = 80\,\,mm\,Hg} \right)$ is 90 mm Hg, for such case:

Assertion: The molarity of a solution depends on the temperature of the solvent.

Reason: Molarity is defined as the number of moles of solute per litre of solution, and the volume of the solvent changes with temperature.

The van’t Hoff factor (i) for a dilute aqueous solution of the strong electrolyte barium hydroxide is

Henry’s constant (in kbar) for four gases $\alpha$, $\beta$, $\gamma$ and $\delta$ in water at 298 K is given below:
$\begin{array}{cccccccccccccccccccc} {}&\alpha &\beta &\gamma &\delta \\ {{K_H}}&{50}&2&{2 \times {{10}^{ - 5}}}&{0.5} \end{array}$
(density of water $= {10^3}\,kg\,{m^{ - 3}}$ at 298 K)
This implies that

The degree of dissociation '$\propto$' of a weak electrolyte is

Molal depression constant is given by the expression:

The condition for the validity of Henry’s law are :

Vapour pressure of dilute aqueous solution of glucose is $750\;mm$ of mercury at $373\;K$. The mole fraction of solute is

On mixing $10\,mL$ of carbon tetrachloride with $10\,mL$ of benzene the total volume of the solution is:

Two solutions of different osmotic pressure. The solution of lower osmotic pressure is called

Assertion (A): Van't Hoff factor for benzoic acid in aqueous medium is 2 assuming complete ionisation.

Reason (R): Van't Hoff factor for $100 \%$ ionised solute equal to the number of ions produced.

18g glucose $\left( {{C_6}{H_{22}}{O_6}} \right)$ is added to 178.2 g water. The vapor pressure of water (in torr) for this aqueous solution is.

Which one of the following electrolyte has the same value of the vant Hoff factor (i) as that of ${A_2}{\left( {S{O_4}} \right)_3}$ (if all are 100% ionised)

Which is correct representation of phase rule?

Which of the given solutions has highest osmotic pressure?

What happen at increasing pressure at constant temperature

If 0.2 m aqueous solution of ${K_4}\left[ {Fe{{\left( {CN} \right)}_6}} \right]$ is 100% ionized then the freezing point of the solution will be $\left( {{K_f} = 1.86\,K\,kg\,mo{l^{ - 1}}} \right)$

The melting point of most of the solid substances increase with an increase of pressure acting on them. However, ice melts at a temperature lower than its usual melting point, when the pressure increase. This is because :

The van't Hoff factor (i) for a dilute aqueous solution of glucose is:

Assertion (A): Molality is independent of temperature.

Reason (R): There is no volume factor in the expression of molality.

A liquid freezes at $7^{\circ} \mathrm{C}$ and boils at $77^{\circ} \mathrm{C}.$ If the $K_{\mathrm{f}}$ and $K_{\mathrm{b}}$ values for the liquid are $5.6$ and $2.5 \, \mathrm{deg} / \mathrm{molal},$ respectively, then the ratio of molar latent heat of fusion to molar latent heat of vaporization is

An open beaker of water in equilibrium with water vapour is in a sealed container. When few grams of glucose are added to the beaker of water, the rate at which water molecules

Statement I : Mole fraction is the ratio of moles of a substance to the total moles in the solution.

Statement II : Mole fraction does not depend on temperature of solution.

In the light of the above statements, choose the correct answer from the options given below.

An acid '$A$' is $0.4 \mathrm{~N}$. In a neutralization process $50 \mathrm{~ml}$ of '$A$' is mixed with $30 \mathrm{~ml}$ of sodium carbonate solution (42.49/litre) and $10 \mathrm{~mL}$ of the resulting solution is diluted to $50 \mathrm{~mL}$ and then $5 \mathrm{~mL}$ of this solution $(B)$ is completely neutralised with certain volume of 40 times diluted solution of $(A)$. find the volume of diluted solution. of $(A)$ required for the neutralization of $B$ (in $\mathrm{mL}$)

Solubility of a substance is its maximum amount that can be dissolved in a specified amount of solvent.
It depends upon

(i) nature of solute $\quad$ (ii) nature of solvent $\quad$ (iii) temperature $\quad$ (iv) pressure