Solutions practice · Medium

The distribution law holds good for :

Which of the following associated with isotonic solutions is not correct?

For an ideal binary liquid solution with $P_A^ \circ > P_B^ \circ$ which relation between ${X_A}$ (mole fraction of A in liquid phase) and ${Y_A}$ (mole fraction of A in vapour phase) is correct, ${X_B}$ and ${Y_B}$ are mole fraction of B in liquid and vapour phase respectively :

Which of the following compounds can be used as antifreeze in automobile radiators?

The osmotic pressure of a solution can be accurately measured in the shortest possible time by :

The solubility of iodine in water is ${0.8\;g/L}$. If the partition coefficient of iodine between ${\mathrm{CC}{\mathrm{l}_4}}$ and water (in favour of ${\mathrm{CC}{\mathrm{l}_4}}$) is 82, the solubility of iodine in ${\mathrm{CC}{\mathrm{l}_4}}$ is :

A solution that obeys Raoult’s law is called

If vapour pressure of two liquids A and B in pure state are 400 and 500 mm of Hg respectively then mole fraction of A in vapour phase of solution obtained by mixing equal moles of A and B is

Consider the following statements about osmotic pressure method of molar mass determination.

I. Molarity of the solution is used instead of molality.

II. Magnitude of osmotic pressure is very large even for dilute solutions.

III. Molar mass of biomolecules can be determined as they are not stable at higher temperatures.

IV. Determine the molar mass of polymer as they have poor solubility.

Which of the above statements are responsible for advantage of osmotic pressure for determination of molar mass over the other colligative properties?

The vapour density of undecomposed ${\mathrm{N}_2}{\mathrm{O}_4}$ is 46. When heated, vapour density decreases to 24.5 due to its dissociation to $\mathrm{N}{\mathrm{O}_2}.$ The per cent dissociation of ${\mathrm{N}_2}{\mathrm{O}_4}$ at the final temperature is :

When a substance is distributed between two immiscible solvents and remains in the same state in the solvent I, while, dissociates in the solvent II. If the concentration of solute are ${c_\mathrm{I}}\;\mathrm{and}\;{c_{\mathrm{II}}}$ in phase I and II respectively then :

Assertion (A): Sum of mole fraction of all components in a mixture is 1.

Reason (R): Mole fraction is temperature dependent mode of concentration.

Which of the following statements is not correct about homogeneous mixtures?

Which one of the following aqueous solutions will exhibit highest boiling point?

The vapour pressure of the solution of two liquids $A\left(P^{\circ}=80 \mathrm{mm}\right)$, and $B\left(P^{\circ}=120 \mathrm{mm}\right)$ is found to be $100 \mathrm{mm}$ when $X_{A}=0.4$. The result shows that

If the various terms in the below given expressions have usual meanings, the van’t Hoff factor (i) cannot be calculated by which one of the expressions?

Molarity and molality of a solution of ${NaOH}$ is calculated. If now temperature of the solution is increased then which of the following statement(s) is/are correct ?

(i) Molarity of solution decreases

(ii) Molality of the solution increases

Which pair will not be isotonic

Which of the following acid has the same molecular weight and equivalent weight.

Which of the following solution highest boiling point?

Vapour pressure of pure A = 100 torr, moles = 2; vapour pressure of pure B=80 torr, moles = 3. Total vapour pressure of the mixture is

$20 \,\mathrm{mL}$ of calcium hydroxide was consumed when it was reacted with $10 \,\mathrm{mL}$ of unknown solution of $\mathrm{H}_{2} \mathrm{SO}_{4}$. Also $20 \,\mathrm{mL}$ standard solution of $0.5 \,\mathrm{M} \,\mathrm{HCl}$ containing 2 drops of phenolphthalein was titrated with calcium hydroxide, the mixture showed pink colour when burette displayed the value of $35.5 \,\mathrm{mL}$ whereas the burette showed $25.5 \,\mathrm{mL}$ initially. The concentration of $\mathrm{H}_{2} \mathrm{SO}_{4}$ is _____ M. (Nearest integer)

When an ideal binary solution is in equilibrium with its vapour, molar ratio of the two components in the solution and in the vapour phase is :

When 36 grams of solute having the empirical formula $C{H_2}O$ is dissolved in 1.2 kg of water, the solution freezes at $- {0.93^0}C$ what is the molecular formula of solute? $\left( {{K_f} = {{1.86}^0}C.kg.mo{l^{ - 1}}} \right)$

Consider the following statements.

(i) On adding methyl alcohol to water, boiling point of water increases

(ii) When ${NaCl}$ is added to water, depression in freezing point is observed

(iii) Diffusion of solution occurs from a region of its high concentration to a region of its low concentration

Choose the correct options

The vapour pressure of benzene at $90^\circ C$ is 1020 torr. A solution of 5 g of a solute in 58.5 g benzene has vapour pressure 990 torr. The molecular weight of the solute is :

The plots of $\frac{1}{{{X_A}}}\;vs.\;\frac{1}{{{Y_A}}}$ (where ${X_A}\;\mathrm{and}\;{Y_A}$ are the mole fraction of liquid A in liquid and vapour phase respectively) is linear with slope and intercepts respectively:

Formation of a solution from two components can be considered as

(1) pure solvent $\to$ separated solvent molecules$\Delta {H_1}$

(2) pure solute$\to$ separated solvent molecules,$\Delta {H_2}$

(3) separated solvent and solute molecules $\to$ solution,$\Delta {H_3}$

Solution so formed will be ideal if

The exact mathematical expression of Raoult's law is ($n=$ moles of non-volatile solute, $N=$ moles of solvent, $P=$ V.P. of solution & $P^{0}=$ V.P. of pure solvent)

The degree of dissociation $(\alpha )$ of a weak electrolyte , ${A_x}{B_y}$ is related to van’t Hoff factor (i) by the expression