Solutions practice · Mixed difficulty

In cold countries, ethylene glycol is added to water in the radiators of cars during winters. It results in :

Which of the following statements is true about Henry's law?

The pair of boiling point and compound are given as,

$\begin{array}{cccccccccccccccccccc} {{C_6}{H_6}}&{C{H_3}OH}&{{C_6}{H_5}N{O_2}}&{{C_6}{H_5}N{H_2}} \\ {80^\circ C}&{65^\circ C}&{212^\circ C}&{184^\circ C} \\ {\left( {\text{I}} \right)}&{\left( {{\text{II}}} \right)}&{\left( {{\text{III}}} \right)}&{\left( {{\text{IV}}} \right)} \end{array}$

Which will show lowest vapour pressure at room temperature?

35.4 mL of HCl is required for the neutralisation of a solution containing 0.275 g of sodium hydroxide. The normality of hydrochloric acid is

$3.01 \times 10^{23}$ molecules of glucose are present in $500 \mathrm{~mL}$ of solution. The molarity of the solution is

Addition of $0.643 \mathrm{~g}$ of a compound to $50 \mathrm{~mL}$ of benzene (density $=0.879 \mathrm{~g} / \mathrm{mL})$ lowers the freezing point from $5.51^{\circ} \mathrm{C}$ to $5.03^{\circ} \mathrm{C}$. If $\mathrm{K}_{\mathrm{f}}$ for benzene is $5.12 \mathrm{~K ~kg ~mol}^{–1},$ calculate the molecular weight of the compound.

One mole of non-volatile solute is dissolved in two mole of water. The vapour pressure of the solution relative to that of water is :

Assertion (A): Aquatic species are more comfortable in cold water rather than in warm water.

Reason (R): The solubility of gas ${O}_2$, increases with decrease of temperature due to increase of ${K}_{{H}}.$

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

Negative deviation from Raoult's law is law is observed in which one of the following binary liquid mixtures?

Phenol dimerizes in benzene. If the observed molecular mass of phenol in solution is 120, then its degree of dimerization is

$0.010 \mathrm{M}$ solution an acid $H A$ freezes at $-0.0205^{\circ} \mathrm{C}$. If $\mathrm{K}_{\mathrm{f}}$ for water is $1.860 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$, the ionization constant of the conjugate base of the acid will be (assume $0.010 \mathrm{M}=0.010 \mathrm{~m}$ )

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

A solution is made by mixing 300 ml. of 1.5 M $A{{l}_{2}}{{\left( S{{O}_{4}} \right)}_{3}}$ + 300 ml. of 2 M $CaS{{O}_{4}}$ + 400 ml. of 3.5 M $CaC{{l}_{2}}.$ Find final molarity of

(a) ${SO}_4^{-2}\quad$ (b) ${Ca}^{2+}$

[Assume complete dissociation of these compounds]

The solubility of a gas in water depends on :

What is the amount of $\mathrm{CaCl}_2(\mathrm{i}=2.9)$ dissolved in 4 litre of water such that its osmotic pressure is 1 atm at $27^{\circ} \mathrm{C}$?

An unriped mango placed in a concentrated salt solution to prepare pickle, shrivels because …….. .

Which of the following statements is incorrect?

Which of the following will have the highest boiling point at $1 {~atm}$ pressure

Calculate the mole fractions of the components of the solution composed by $92 \mathrm{~g}$ glycerol and $90 \mathrm{~g}$ water$? \, \, (M$ (water$)=18 ; M($glycerol$)=92)$

Statement I: Molarity of $0.02 \mathrm{~N} \mathrm{~HNO}_3$ is $0.02 \mathrm{~M}$.

Statement II: Molarity and normality of a solution are always same.

Percent by mass of solute (molar mass $=25 \mathrm{~g} / \mathrm{mol}$ ) in its aqueous solution is 30 . The mole fraction and molality of the solute in solution are

The vapour pressure of a pure liquid A is 40 mm Hg at 310 K. The vapour pressure of this liquid in a solution with liquid B is 32 mm Hg. What is the mole fraction of A in the solution if it obeys the Raoult’s law?

Molal depression constant for a solvent is $4.0\mathrm{ }K\mathrm{ }\,\,kg\mathrm{ }\,\,mo{l^{ - 1}}$. The depression in the freezing point of the solvent for $0.03\mathrm{ }\,\,mol\,\,\mathrm{ k}{\mathrm{g}^{ - 1}}$ solution of ${K_2}S{O_4}$ is (Assume complete dissociation of the electrolyte)

For dilute solution Raoult’s law states that

When 45 gm solute is dissolved in 600 gm water freezing point lower by 2.2 K, calculate molar mass of solute $\left( {{K_f} = 1.86\,K\,kg} \right)$

The boiling point elevation constant for toluene is $3.32 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. The normal boiling point of toluene is $110.7^{\circ} \mathrm{C}$. The enthalpy of vaporisation of toluene would be nearly:

According to phase rule, if $P = 3,C = 1,$ then F must be equal to :

At $35^\circ \mathrm{C}$, the vapour pressure of $C{S_2}$ is 512 mm Hg and that of acetone is 344 mm Hg. A solution of $C{S_2}$ in acetone has a total vapour pressure of 600 mm Hg. The false statement amongst the following is

A cane sugar solution has an osmotic pressure of 2.46 atm at 300K. What is the strength of the solution.