Solutions practice · Mixed difficulty

Vapour pressure of chloroform $\left( {\mathrm{CHC}{\mathrm{l}_3}} \right)$ and dichloromethane $\left( {\mathrm{C}{\mathrm{H}_2}\mathrm{C}{\mathrm{l}_2}} \right)\;\;at\;25^\circ C$ are 200 mm Hg and 41.5 mm Hg respectively. Vapour pressure of the solution obtained by mixing 25.5 g of $\left( {\mathrm{CHC}{\mathrm{l}_3}} \right)$ and 40 g of ${\mathrm{C}{\mathrm{H}_2}\mathrm{C}{\mathrm{l}_2}}$ at the same temperature will be :
(Molecular mass of $\mathrm{CHC}{\mathrm{l}_3} = 119.5\;\;u$ and molecular mass of $\mathrm{C}{\mathrm{H}_2}\mathrm{C}{\mathrm{l}_2} = 85\;u)$

A semipermeable membrane used in the measurement of osmotic pressure of a solution allows the passage of:

Mole fraction of solute in benzene is 0.2 then find molality of solute

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

In a Victor Meyer determination of the relative molecular mass of benzene, the heating vessel was maintained at $120^{\circ} \mathrm{C}.$ A mass of $0.1528 \mathrm{~g}$ of benzene was used and the volume of displaced air collected over water at $15^{\circ} \mathrm{C},$ was $48 \mathrm{~cm}^3.$ The barometric pressure was $743 \mathrm{~mm} \mathrm{~Hg}.$ Calculate the relative molecular mass of benzene. The vapor pressure of water at $15^{\circ} \mathrm{C}$ is $13 \mathrm{~mm} \mathrm{~Hg}.$

Which of the following is not an example of a solution?

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 $\left( {{K_f} = 1.86\,K\,kg} \right)$

A non-volatile solute '$\mathrm{X}$' completely dimerizes in water, if the temperature is below $-3.72^{\circ} \mathrm{C}$ and the solute completely dissociates as $\mathrm{X} \rightarrow \mathrm{Y}+\mathrm{Z},$ if the temperature is above $100.26^{\circ} \mathrm{C}.$ In between these two temperatures (including both temperatures), the solute is neither dissociated nor associated. One mole of '$\mathrm{X}$' is dissolved in $1.0 \mathrm{~kg}$ water $\left(K_{\mathrm{b}}=0.52 \mathrm{~K}-\mathrm{kg} / \mathrm{mol}, K_{\mathrm{f}}=1.86 \mathrm{~K}-\mathrm{kg} / \mathrm{mol}\right)$. Identify the incorrect information related with the solution.

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.

How many gram of glucose must be present in $0.5 \mathrm{~L}$ of solution for its osmotic pressure to be the same as that of $9.2 \mathrm{~g}$ of glucose per litre?

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 $1.013 \mathrm{~g} / \mathrm{ml}, \mathrm{g}=10 \mathrm{~m} / \mathrm{s}^2$, $R=0.08 \mathrm{~L}-\mathrm{atm} / \mathrm{K}-\mathrm{mol}$)

Scuba divers may experience a condition called To avoids this, the tanks used by scuba divers are filled with air diluted with

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 of the following shows maximum depression in freezing point?

Assuming ideal behaviour, what mass of a non-volatile solid of molar mass $128 \mathrm{~g} \mathrm{~mole}^{-1}$ would have to be dissolved in $228 \mathrm{~g}$ octane $\left(\mathrm{C}_{\mathrm{g}} \mathrm{H}_{18}\right)$ to lower the vapour pressure of octane by $20 \%$?

An ideal solution made by mixing two volatile components A and B. If the vapour pressure of solution is 170 mm Hg, then mole fraction of A in vapour phase is $\left( {P_A^0 = 200\,mm\,Hg,\,P_B^0 = 100\,mm\,Hg\,} \right)$

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: