Solutions practice · Medium

1.0 molar solution of the complex salt, $\mathrm{CrCl}_3 \cdot 6 \mathrm{H}_2 \mathrm{O}$, displays an osmotic pressure of $3 R T$. $0.5 \mathrm{~L}$ of the same solution on treatment with excess of $\mathrm{AgNO}_3$ solution will yield (assume $\alpha=1$ ) :

Calculate the amount of ice that will separate out on cooling $a$ solution containing $50 {~g}$ of ethylene glycol in $200 {~g}$ water to $-9.3^{\circ} {C}$. ( $K_f$ for water $=1.86 {~K} {~mol}^{-1} {~kg}$ )

During which of the following processes, does entropy decrease?
A) Freezing of water to ice at $0^\circ C$.
B) Freezing of water to ice at $- 10^\circ C$.
C) ${N_2}(g) + 3{H_2}(g) \to 2N{H_3}(g)$
D) Adsorption of $CO(g)$ and lead surface.
E) Dissolution of $NaCl$ in water.

A solution of urea boils at ${100.18^0}C$ at the atmospheric pressure. If ${K_f}$ and ${K_b}$ for water are 1.86 and 0.512 $K.Kg.Mo{l^{ - 1}}$ respectively, the above solution will freeze at

An aqueous solution of a weak monobasic acid containing $0.1 g$ in $21.7 g$ of water freezes at $272.813\, K$. If the value of $K_f$ for water is $1.86 {~K} / {m}$, what is the molecular mass of the monobic acid

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

Assertion (A): People taking a lot of salty food experience the puffiness or swelling, called edema.

Reason (R): There is water retention in tissue cells and intercellular spaces hecause of osmosis.

Consider the following arrangement, in which a solution containing $20 \mathrm{~g}$ of haemoglobin in $1 \mathrm{~dm}^3$ of the solution is placed in right compartment and pure water is placed in left compartment, separated by SPM. At equilibrium, the height of liquid in the right compartment is $74.5 \mathrm{~mm}$ in excess of that in the left compartment. The temperature of the system is maintained at $298 \mathrm{~K}.$ The number of millimoles in $320 \mathrm{~g}$ of haemoglobin is (Given: The density of final solution is $1.013 \mathrm{~g} / \mathrm{ml}, \mathrm{g}=10 \mathrm{~m} / \mathrm{s}^2$, $R=0.08 \mathrm{~L}-\mathrm{atm} / \mathrm{K}-\mathrm{mol}$)

If the elevation in boiling point of a solution of 10 g of solute (mol. wt. = 100 g of water is $\Delta {T_b}$, the ebullioscopic constant of water is

$2.5 {~g}$ of a substance is present in $200 {~mL}$ of solution showing the osmotic pressure of $60 {~cm} {Hg}$ at $15^{\circ} {C}$. Calculate the molar mass of substance. What will be the osmotic pressure if temperature is raised to $25^{\circ} {C}$ ?

Each of the following pair shows a positive deviation from the Raoult's law except

Consider the solution of ethanol. In it

Select correct statements :

Statement I: Mass density of a mixture of $20 \mathrm{~g}$ water and $100 \mathrm{~g}$ of ethanol is $0.86 \mathrm{~g} \mathrm{~cm}^{-3}$ at $298 \mathrm{~K}$.

Statement II: At $298 \mathrm{~K}$, molar volume of water and ethanol are respectively $18 \mathrm{~cm}^3$ and $55 \mathrm{~cm}^3$ based on density. $\left(d=1.00 \mathrm{~g} \mathrm{~cm}^{-3}\right.$ for water and $d=0.8364 \mathrm{~g} \mathrm{~cm}^{-3}$ for ethanol).

Statement I: Normality and molarity can be calculated from each other.

Statement II: Normality is equal to the product of molarity and $\mathrm{n}$.

An aqueous solution of a non-volatile and non-electrolyte solute (molecular mass = 150) boils at $373.26 \mathrm{~K}.$ The composition of solution, in terms of mass percent of the solute, is $\left(K_{\mathrm{b}}\right.$ of water $=$ $0.52)$

Which of the following has lowest freezing point

A perfectly semipermeable membrane when used to separate a solution from its solvent permits through it the passage of:

At higher altitudes the boiling point of water lowers because

Which one of the following gases has the lowest value of Henry's law constant?

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

One mole of a solute $\mathrm{A}$ is dissolved in a given volume of a solvent. The association of the solute take place as follows: $\mathrm{nA} \rightleftharpoons \mathrm{A}_{\mathrm{n}}$. If $\alpha$ is the degree of association of A, the van't Hoff factor ' $\mathrm{i}$ ' is expressed as:

Assertion (A): An azeotropic solution of two liquids has boiling point lower than either of them.
Reason (R): Solution shows +ve deviation from ideal behaviour.

Which of the following aqueous solution has osmotic pressure nearest to that of an equimolar solution of $\mathrm{K}_4\left[\mathrm{Fe}(\mathrm{CN})_6\right] ?$

The volume of $0.5 \mathrm{~M}$ Urea required to prepare $0.1 \mathrm{~M}$ of $100 \mathrm{~ml}$ Urea solution is

Which one of the following statements is false ?

Statement I: Mercuric iodide dissolves in potassium iodide solution forming $\mathrm{K}_2 \mathrm{Hgl}_4$ and the freezing point gets elevated.

Statement II: The number of particles in $\mathrm{K}_2 \mathrm{Hgl}_4$ is same as those in $\mathrm{Hgl}_2$.

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

A solution containing $8.6 \mathrm{~g}$ urea in one liter was found to be isotonic with a $5 \%(w / V)$ solution of an organic non-volatile solute at same temperature. The molecular weight of latter is

Calculate the boiling point of a one molar aqueous solution (density $1.04 \mathrm{~g} \mathrm{~mL}^{-1}$) of potassium chloride. $\left(\mathrm{K}_{\mathrm{b}}\right.$ for water $=0.52 \mathrm{~K} \mathrm{~kg} \mathrm{~mol}^{-1}$. Atomic mass of $\mathrm{K}=39, \mathrm{Cl}=35.5$)