The vapour pressure of the solution of

$5\,g$ on non-electrolyte in

$100\,g$ of water at a particular temperature is

$2950\,N/{m^2}$ . The vapour pressure of water is

$3000\,N/{m^2}$ . The mocular mass of the solute is ?

0%
$54$
0%
$124$
0%
$180$
0%
$340$

The Vant Hoff factor for a dilute solution

${K_3}\left[ {Fe{{\left( {CN} \right)}_6}} \right]$

0%
10
0%
4
0%
5
0%
0.25

50 mL of 1 M oxalic acid(molar mass = 126 g) is shaken with 0.5 g of wood charcoal, the final concentration of the solution after adsorption is 0.5 M. Calculate the amount of oxalic acid adsorbed per gram of charcoal.

0%
6.1
0%
6.2
0%
6.4
0%
6.3

Benzoic undergoes dimerization in benzene solution. The van't Hoff factor is related to the degree of association 'x' of the acid is ?

0%
${\text{i}} = \left( {1 - x} \right)$
0%
${\text{i}} = \left( {1 + x} \right)$
0%
${\text{i}} = \left( {1 - \frac{x}{2}} \right)$
0%
${\text{i}} = \left( {1 + \frac{x}{2}} \right)$

Which of the following solutions will have the lowest vapour pressure?

0%
$0.1 M\ Glucose$
0%
$0.1 M\ NaCl$
0%
$0.1 M\ BaCl_2$
0%
$0.1 M Al_2 (SO_4)_3$

Vapour Pressure of methyl alcohol and ethyl alcohol solution is represented by

$P=115{ x }_{ A}+140$ . Where

${ x }_{ A }$ is the mole fraction of methyl alcohol. The value of

$\lim _{ { x }_{ A }\rightarrow 0 }{ \frac { { P }_{ B }^{ 0 } }{ { x }_{ B } } } \\$

0%
255
0%
115
0%
140
0%
135

The vapour pressure of

$1$ molal glucose solution at

$100^{o}C$ will be

0%
$760\ mmHg$
0%
$76.0\ mmHg$
0%
$1\ atm$
0%
$746.32\ mmHg$

At a certain temperature pure liquid A and liquid B have vapour pressures 10 torr and 37 torr respectively. For a certain ideal solution of A and B, the vapour in equilibrium with the liquid has the components A and B in the partial pressure ratio

$P_A : P_B=1 : 7$ . What is the mole fraction of A in the solution?

0%
0.346
0%
0.654
0%
0.5
0%
None of these

Vapour pressure increase with increase in :

0%
Concentration of solution containing non-volatile soulute
0%
Temperature up to boiling point
0%
Temperature upto triple point
0%
Altitude of the concerned place of boiling

Vapour pressure of pure 'A' is 70 mm of Hg at

$25^0C$ it forms an ideal solution is with 'B' in which mole fraction of A is 0.If the vapour pressure of the solution is 84 mm is Hg at

$25^0C$ , the vapour pressure of pure 'B' at

$25^0C$ is :

0%
56 mm Hg
0%
70 mm Hg
0%
140 mm Hg
0%
28 mm Hg

A mixture of

$H_2SO_4$ and

$H_2C_2O_4$ (oxalic acid) and some inert impurity weighing 3.185g was dissolved in water and the solution was made up to 1litre. 10mL of this solution required 3mL of 0.1N

$NaOH$ for complete neutralization. In another experiment, 100mL of the same solution in hot conditions requires 4mL of 0.02M

$KMnO_4$ solution for complete reaction.

The weight % of

$H_2SO_4$ in the mixture was:-

0%
40
0%
50
0%
60
0%
80

The mass of a non-volatile non-electrolyte solute (molar mass

$=50\ g\ mol^ {-1}$ ) needed to be dissolved in

$114\ g$ octane to reduce its vapour pressure to

$75\%$ is:

0%
$37.5\ g$
0%
$75\ g$
0%
$150\ g$
0%
$50\ g$

At a certain temperature, the vapour pressure of water is

$50\ mm.$ The relative lowering of vapour pressure of a solution containing

$36\ g$ of glucose in

$900\ g$ of water is

0%
$0.1$
0%
$0.5$
0%
$0.004$
0%
$3.75$

The possible van't Hoff factor for sodium chloride in water assuming sodium chloride is partially ionized:

0%
$0.5$
0%
$0.75$
0%
$2.5$
0%
$1.5$

Which of the following have least vapour pressure?

0%
$0.1\ M\ NaCl\ sol$
0%
$0.1\ M\ urea\ sol$
0%
$0.1\ M\ AlCl_{3}\ sol$
0%
$0.1\ M\ KCl\ sol$

$K_2HgI_4$ is

$40 \%$ ionised in aqueous solution. The value of its van't Hoff factor (i) is:

0%
$1.8$
0%
$2.2$
0%
$2.0$
0%
$1.6$

Explanation

$K_2HgI_4 \to 2K^+ + {HgI_4}^{2-}$

$i = 1+(n-1) \alpha$

$\alpha = 0.4$

$n = 3$

$i = 1+2\times 0.4 = 1.8$

Hence, the correct option is

$\text{A}$

The lowering of vapour pressure of 0.1 M aqueous solutions of

$NaCl,\ CuS{O_4}$ and

${K_2}S{O_4}$ are ;

0%
all equal
0%
in the ratio of 1 : 1 : 1.5
0%
in the ratio of 3 : 2 : 1
0%
in the ratio of 1.5 : 1 : 2.5

When a solution containing non-volatile solute is diluted with water,

0%
its vapour pressure increases
0%
its osmotic pressure increases
0%
its boiling point increases
0%
its freezing point increases

An ideal solution formed by mixing two liquids 'A' and 'B' find the pressure at which

${X_A} = {Y_B}\ ({P_A}^0 = 400\ torr,{P_B}^0 = 100\,torr)$

$({X_A}$ and

${Y_B}$ are mole fraction of A and B in liquid and vapour forms respectively at equilibrium.)

0%
250 torr
0%
200 torr
0%
150 torr
0%
125 torr

An ideal solution is formed by mixing two liquids 'A' and 'B'. Find pressure at which

${X_A} = {Y_B}\,\,({P_A}^\circ = 400\,\,torr,\,\,{P_B}^\circ = 100\,\,torr)\,\,:\,\,({X_A}\,\,and\,\,{Y_B}$ are mole fractions of A and B liquids and vapour forms, respectively, at equilibrium.)

0%
250 torr
0%
200 torr
0%
150 torr
0%
125 torr

${35}^{o}C$ , the vapour pressure of

$CS_2$ is

$512mm$

$Hg$ , and acetone is

$344mm$

$Hg$ . A solution of

$CS_2$ and acetone in, which the mol fraction of

$CS_2$ is

$0.25$ , has a total vapour pressure of

$600mm$

$Hg$ . Which of the following statements is/are correct:

0%
A mixture of $100mL$ of acetone and $100mL$ of has a volume is $200mL$
0%
When acetone and are mixed at ${35}^{o}C$ , heat must be absorbed in order to produce a solution at ${35}^{o}C$
0%
When acetone and are mixed at ${35}^{o}C$ , heat is released
0%
There is negative deviation from Raoult's law

The Van't Hoff factor of 0.1 M

${\text{Ba}}{\left( {{\text{N}}{{\text{O}}_3}} \right)_2}$ solutions is 2.The degree of dissociation will be

0%
91.3%
0%
87%
0%
100%
0%
74%

A solution is prepared by mixing

${\text{8}}{\text{.5}}\,{\text{g}}$ of

${\text{C}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{l}}_2}$ and

$11.95\,{\text{g}}$ of

${\text{CHC}}{{\text{l}}_{\text{3}}}$ . If vapour pressure of

${\text{C}}{{\text{H}}_{\text{2}}}{\text{C}}{{\text{l}}_{\text{2}}}$ and

${\text{CHC}}{{\text{l}}_3}$ at

${\text{298}}\,{\text{K}}$ are

$415$ and

$200\,{\text{mm}}$ Hg respecetively, then mole fraction of

${\text{CHC}}{{\text{l}}_{\text{3}}}$ in vapour form is:

0%
$0.162$
0%
$0.675$
0%
$0.325$
0%
$0.486$

$10\%$ solution of

$NaCl$ means that in

$100g$ of solution there is:

0%
$5.85g\ NaCl$
0%
$58.5g\ NaCl$
0%
$10g\ NaCl$
0%
$94g\ NaCl$

The value of observed and calculated molecular weight of silver nitrate are

$92.64$ and 170 respectively. The degree of dissociation of silver nitrate is :

0%
$60\%$
0%
$83.5\%$
0%
$46.7\%$
0%
$60.23\%$

Binary solute

$(AB)$

$60\%$ dissociate and

$40\%$ dimerise. Value of van't Hoff factor

$(i)$ is

0%
$1.20$
0%
$1.10$
0%
$1.40$
0%
$1.50$

Binary solute (AB) 60 % dissociate and 40 % dimerise. Value of van't Hoff factor (i) is

0%
1.20
0%
1.10
0%
1.40
0%
1.50

Which of the following pairs do not form ideal solution

0%
${{\text{C}}_6}{{\text{H}}_6}\;and\;{\text{CC}}{{\text{l}}_4}$
0%
${{\text{C}}_6}{{\text{H}}_6}\;{\text{and}}\;{{\text{C}}_6}{{\text{H}}_5}{\text{CH}}$
0%
${{\text{C}}_2}{{\text{H}}_5}Br\;and\;{{\text{C}}_2}{{\text{H}}_5}{\text{l}}$
0%
none.

The relative lowering of vapour pressure of a solution of 6 g of urea dissolved in 90 g of water is equal to

0%
0.02
0%
0.04
0%
0.60
0%
0.03

The lowering of vapour pressure of a solvent by addition of a non-volatile solute to it is directly proportional to :

0%
The strength of the solution
0%
The nature of the solute in the solution
0%
The atmospheric pressure
0%
All

Two liquids A and B form ideal solution.At 300K,the vapour pressure of solution containing 1 mol of A and 3 mol of B is 550mm Hg.At the same temperature,if one more mole of B is added to this solution,the vapour pressure of the solution increases by 10mm Hg.Determine the vapour pressures of A and B in their pure states.

0%
$563$ and $469$
0%
$500$ adn $1250$
0%
$513$ and $494$
0%
$400$ and $600$

The vapour pressure of water at T(K) is 20 mm Hg. The following solutions are prepared at T(K) :

0%
6 g of urea (mol. wt. = 60) is dissolved in 178.2 g of water
0%
0.01 mole of glucose is dissolved in 179.82 g of water
0%
5.3 g of $N{a_2}C{O_3}$ (mol. wt. =106) is dissolved in 179.1 g of water.
0%
non of these

${X_A}$ and

${X_B}$ represent mole fraction in liquid phase while

${y_A}$ and

${y_B}$ represent mole fraction in vapour phase in binary solution. Which of the following statements is/are correct?

0%
At point C liquid and vapour phase have same composition
0%
Vapour pressure of B is less than A
0%
Intermolecular forces in the solution are weaker than between like particles
0%
All of these

Solubility will be higher when the process is exothermic.

0%
True
0%
False

Molar volume of liquid A (d=0.8 gm/ml) increase by a factor of 2000 when it vapourises at 2000K. The vapour pressure of liquid A at 200K is:

[R=0.08 L-atm/mol-K] (Molar mass of A=80 g/mol)

0%
0.4 atm
0%
8 atm
0%
0.8 atm
0%
0.08 atm

In the accompanied diagram, the ideal behaviour of a solution is shown by the line/s

0%
AD
0%
CB
0%
BD
0%
AD,CB

An ideal solution contains two volatile liquids

$A (P^0=100 \ torr)$ . If the mixture contains 1 mole of A and 3 moles of B, the total vapour pressure of distillate is:

0%
150 torr
0%
188.88 torr
0%
185.72 torr
0%
198.88 torr

Which of the following mixture will be producing acidic solution at

$25^ {o}C$ ?

0%
$200ml\dfrac {M}{10}H_{2}SO_{4}+300ml\dfrac {M}{10}NaOH$
0%
$600ml\dfrac {M}{10}HNO_{3}+400ml\dfrac {M}{10}NaOH$
0%
$900ml\dfrac {M}{10}HCI+300ml\dfrac {M}{10}NaOH$
0%
$All\ of\ these$

Concentrated aqueous sulphuric acid is

$98% { H }_{ 2 }{ SO }_{ 4 }$ by mass and has a density of

$1.80{ gmL }^{ -1 }.$ Volume of acid required to make one lite of

$0.1 M{ H }_{ 2 }{ SO }_{ 4 }$ solution is:

0%
11.10 mL
0%
16.65 mL
0%
22.20 mL
0%
5.55 ml

A vessel of volume

$V = 16.62$ litres contains a mixture of hydrogen and helium at a temperature of 27

$^{0}$ C and pressure 6 atmosphere.The mass of the mixture is 10 g. Then
The ratio of mass of hydrogen to that of helium will be :

0%
1 /2
0%
2 /3
0%
3 / 2
0%
4 / 3

For binary ideal liquid solution, the total pressure of the solution is given as :

0%
${{\text{P}}_{{\text{total}}\;}} = {\text{P}}_{\text{A}}^{\text{o}}{\text{ + }}\left( {{\text{P}}_{\text{A}}^{\text{o}} - \;{\text{P}}_{\text{B}}^{\text{o}}} \right){{\text{X}}_{\text{B}}}$
0%
${{\text{P}}_{{\text{total}}\;}} = {\text{P}}_B^{\text{o}}{\text{ + }}\left( {{\text{P}}_{\text{A}}^{\text{o}} - \;{\text{P}}_{\text{B}}^{\text{o}}} \right){{\text{X}}_A}$
0%
${{\text{P}}_{{\text{total}}\;}} = {\text{P}}_B^{\text{o}}{\text{ + }}\left( {{\text{P}}_B^{\text{o}} - \;{\text{P}}_A^{\text{o}}} \right){{\text{X}}_A}$
0%
${{\text{P}}_{{\text{total}}\;}} = {\text{P}}_{\text{B}}^{\text{o}}{\text{ + }}\left( {{\text{P}}_B^{\text{o}} - \;{\text{P}}_A^{\text{o}}} \right){{\text{X}}_B}$

To an aqueous solution of

$NaI$ , increasing amounts of solid

$HgI_ { 2 }$ is added, the vapour pressure of the solution:

0%
decreases to a constant value
0%
increases to a constant value
0%
increases first and then decreases
0%
remains constant because $\mathrm { HgI} _ { 2 }$ is sparingly soluble in water

The volume of 0.0168 mol of

${ O }_{ 2 }$ obtained by decomposition of

${ KCIO }_{ 3 }$ and collected by displacement of water is 428ml at a pressure of 754 mm Hg at

${ 25 }^{ 0 }C.$ The pressure of water vapour at

${ 25 }^{ 0 }C$ is:

0%
18 mm Hg
0%
20 mm Hg
0%
22 mm Hg
0%
24 mm Hg

Colligative properties of a dilute solution depend on

0%
Nature of solute
0%
Nature of solvent
0%
Number of solute particles
0%
Number of solvent particles

Two liquids A & B form an ideal solution. What is the vapour pressure of solution containing 2 moles of A and 3 moles of B at 300 K? [Given: At 300 K, Vapour pr. of pure liquid A

$\left( P\begin{matrix} 0 \\ A \end{matrix} \right)$ =100 torr, Vapour pr. of pure liquid B

$\left( P\begin{matrix} 0 \\ B \end{matrix} \right)$ =300 torr]

0%
200 torr
0%
140 torr
0%
180 torr
0%
None of these

A mixture of

$CO$ and

$CO_2$ is found to have a density of 1.50

$g L^{-1}$ at 20

$^0C$ & 740 mm pressure. Mole

$\%$ of

$CO_2$ in the given mixture is:

0%
$64.5$ %
0%
$56.2$ %
0%
$62.8$ %
0%
$45.6\%$

Observe the following abbreviations,

$\pi _{obs}=$ observed colligative property,

$\pi_{cal} =$ theoretical colligative property, assuming normal behaviour of solute. Van't Haff factor (i) is given by:

0%
$I= \pi_{obs}\times \pi_{cal}$
0%
$I= \pi_{obs} + \pi_{cal}$
0%
$I= \pi_{obs}-\pi_{cal}$
0%
$\displaystyle I= \frac{\pi_{obs}}{\pi_{cal}}$

Which of the following electrolytes has the same van't Hoff factor

$(i)$ as that of aluminium sulphate:

0%
$N a _ { 3 } P O _ { 4 }$
0%
$\mathrm { Hg } _ { 2 } \mathrm { Cl } _ { 2 }$
0%
$K _ { 3 } \left[ F e ( \mathrm { CN } ) _ { 6 } \right]$
0%
$K _ { 4 } \left[ F e ( C N ) _ { 6 } \right]$

Which one of the following is incorrect for ideal solution ?

0%
$\Delta P=Pobs-{ P }_{ calculated} \quad by\quad Raoult's=0$
0%
$\Delta { G }_{ mix }=0$
0%
$\Delta { H }_{ mix }=0$
0%
$\Delta U_{ mix }=0$

Relative lowering in vapour pressure of a solution containing 1 mole

$K_{2}SO_{4}$ in 54 g

$H_{2}O$ is: (

$K_{2}SO_{4}$ is 100 % ionised )

0%
$\dfrac{1}{55}$
0%
$\dfrac{3}{55}$
0%
$\dfrac{3}{4}$
0%
$\dfrac{1}{2}$

CBSE Questions for Class 12 Engineering Chemistry Solutions Quiz 13 - MCQExams.com

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