Solutions practice · Mixed difficulty

For a dilute solution, Raoult's law states that:

The solution having lesser value of osmotic pressure is called:

What is the molarity of $0.2\;N\;N{a_2}C{O_3}$ solution?

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?

$0.1 \mathrm{~M} \mathrm{~NaCl}$ and $0,005 \mathrm{~M} \mathrm{~BaCl}_2$ solutions are separated by a semipermeable membrane in a container. For this system, choose the correct answer.

In water saturated air, the molefraction of water vapour is 0.02. If the total pressure of the saturated air is 1.2 atm, the partial pressure of dry air is

Find final molarity of solution made by $500 \mathrm{~ml} \, 0.1 \mathrm{~M} \, {HCl}+500 \mathrm{~ml} \, 0.2 \mathrm{~M} \, {HCl}.$

Assertion (A): On increasing temperature vapour pressure of solution increases.

Reason (R): Vapour pressure of ether is higher than alcohol.

$0.1 {M}$ solution of glucose was found to be isotonic with a solution of $X$ in $100 {~g}$ water. Calculate relative lowering in vapour pressure of solution of $X$ in water.

An aqueous solution of glucose containing $12 {~g}$ in $100 {~g}$ of water was found to boil at $100.34^{\circ} {C}$. Calculate $K_b$ for water in ${K} {mol}^{-1} {~kg}$.

Lowering of vapour pressure is highest for

Which of the following will have the lowest vapour pressure

Which of the given solutions has highest osmotic pressure?

A solution of $6 \%$ (mass $/ {vol}$.) urea is isotonic with ${NaCl}_{a q}$. What is the mass/vol. $\%$ of ${NaCl}$ in solution?

The boiling point of ${CHCl}_3$ was raised by $0.323^{\circ} {C}$ when $0.5143 {~g}$ of anthracene was dissolved in $35 {~g} {CHCl}_3$. Calculate the molar mass of anthracene. $K_b^{\prime}$ for ${CHCl}_3=3.9 {~K} {~mol}^{-1} {~kg}$.

$\mathrm{H}_2 \mathrm{S},$ a toxic gas with rotten egg like smell, is used for the quantitative analysis. If the solubility of $\mathrm{H}_2 \mathrm{S}$ in water at STP is $0.2 \mathrm{~m},$ then Henry's law constant for $\mathrm{H}_2 \mathrm{S}$ in water at $273 \mathrm{~K}$ is

Determine the molarity of a $40 \%$ solution of $\mathrm{HCl}$ which has a density of $1.2 \mathrm{~g} \mathrm{~mL}^{-1}$.

Van’t Hoff factor $(i)$:

Concentration terms which are independent of temperature is/are

How much ${{\mathrm{K}_2}\mathrm{C}{\mathrm{r}_2}{\mathrm{O}_7}}$ (Mol. wt. = 294.19) is required to prepare one litre of 0.1 N solution?

Statement I: Raoult’s law is applicable for dilute solutions only.
Statement II: Henry’s law is applicable for solution of gas in liquid.

At $100^{\circ} \mathrm{C},$ the vapour pressure of a solution of $4.0 \mathrm{~g}$ of solute in $100 \mathrm{~g}$ of water is $750 \mathrm{~mm}.$ The boiling point of the solution is $\left(\mathrm{K}_{\mathrm{b}}\right.$ of water $=0.52$ $\mathrm{K}-\mathrm{kg} / \mathrm{mol})$

The osmotic pressure of $0.1 \,{M}$ aq. glucose solution at $27^{\circ} {C}$ is

An organic liquid, $A$ is immiscible with water. When boiled together with water, the boiling point is $90^{\circ} \mathrm{C}$ at which the partial pressure of water is $526 \mathrm{~mm} \mathrm{Hg}$. The atmospheric pressure is $736 \mathrm{~mm} \mathrm{Hg}$. The weight ratio of the liquid and water collected is $2.5: 1$. The molecular weight of the liquid is ...

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 :

Assertion: Van't Hoff factor for benzoic acid in benzene is one.

Reason: Benzoic acid behaves as a weaker electrolyte in benzene.

Relative lowering in vapour pressure of solution containing non-volatile solute is directly proportional to mole fraction of solute". Above statement is:

Assertion : Themolecular weight of acetic acid determined by depression in freezing point method in benzene and water was found to be different.

Reason : Water is polar and benzene is non-polar.

The boiling point of water $\left(100^{\circ} {C}\right)$ becomes $100.52^{\circ} {C}$, if $3 \,grams$ of a nonvolatile solute is dissolved in $200 \,{ml}$ of water. The molecular weight of solute is ( $K_b$ for water is $0.6 {~K}-{m}$ )

An aqueous solution of ${NaCl}$ shows the depression of freezing point of water equal to $0.372 {~K}$. The boiling point of ${BaCl}_2$ solution of same molality will be $\left(K_f\left({H}_2 {O}\right)=1.86 {~K} {~kg} {~mol}^{-1}\right.$, $\left.K_b\left({H}_2 {O}\right)=0.52 {~K} {~kg} {~mol}^{-1}\right)$