EASY

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Why is it more convenient to obtain the molecular weight of an unknown solute by measuring the freezing point depression than by measuring the boiling point elevation?

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Important Questions on Solutions

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

Molal elevation constant is the elevation in boiling point produced by

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The elevation in the boiling point of an aqueous solution of

NaCl

0.01 ° C

. If its van't Hoff factor is

1.92,

the molality of

NaCl

solution is ___

(K_{b}

for water

= 0.52 K kg {mol}^{- 1})

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The boiling point (in

{}^{\circ}C

) of

0.1

molal aqueous solution of

{CuSO}_{4} . 5 H_{2} O

1

bar is closest to: [Given: Ebullioscopic (molal boiling point elevation) constant of water,

K_{b} = 0.512 K {kgmol}^{- 1}]

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The boiling point of a sugar solution when

3.42 g

of sugar is dissolved in

40 g

water is

(K_{b} = 0.52 {}^{\circ}C)

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

58.5 g of NaCl and 180 g

of glucose were separately dissolved in

1000 mL

of water. Identify the correct statement regarding the elevation of boiling point (b.pt.) of the resulting solutions.

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

An aqueous solution containing

1.0 g

of urea boils at

100.25 ° C .

The aqueous solution containing

3.0 g

of glucose in the same volume will boil at:

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The boiling point of

0.001 M

aqueous solutions of

NaCl, {Na}_{2} {SO}_{4}, K_{3} {PO}_{4}

and

{CH}_{3} COOH

should follows the order.

HARD

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The plot given below shows $P - T$ curves (where, $P$ is the pressure and $T$ is the temperature) for two solvents $X$ and $Y$ and isomolal solutions of $NaCl$ in these solvents. $NaCl$ completely dissociates in both the solvents.

Question Image

On the addition of equal number of moles of a non-volatile solute $S$ in equal amount (in $kg$ ) of these solvents, the elevation of boiling point of solvent $X$ is three times that of solvent $Y$ . The solute $S$ is known to undergo dimerization in these solvents. If the degree of dimerization is $0.7$ in the solvent $Y$ , the degree of dimerization in the solvent $X$ is _______.

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

An aqueous solution freezes at

272.4 K

, while pure water freezes at

273 K

, given

K_{f} = 1.86 K kg {mol}^{- 1}

, and

K_{b} = 0.512 K kg {mol}^{- 1};

the molality of solution and boiling point of solution respectively will be -

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

Solute

' X'

dimerises in water to the extent of

80 %

2.5 g

' X'

100 g

of water increases the boiling point by

0.3 ° C

. The molar mass of

' X'

[K_{b} = 0.52 K {kgmol}^{- 1}]

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

Acetic acid dimerises when dissolved in benzene. As a result boiling point of the solution rises by

0.36 ° C,

when

100 g

of benzene is mixed with

X g

of acetic acid. In this solution, if experimentally measured molecular weight of acetic acid is

117.8

and molar elevation constant of benzene is

2.57 K kg {mol}^{- 1},

what is the weight

%

and degree of dissociation (in

%

) of acetic acid in benzene?

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

1 m o l

N a C l

solute is dissolved in

1 k g

of water, at what temperature will water boil at

1.013

bar?

(K_{b} o f w a t e r i s 0.52 K k g m o l^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

What will be the boiling point of

30 g

benzene containing

0.75 g

of benzoic acid which undergoes

75 %

dimerization? Boiling point of pure benze

= 80.1 ° C

and

K_{b} = 2.53 {Kmol}^{- 1} kg

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

Which of the following aqueous solution will have the boiling point

102.2 ° C ?

The molal elevation constant for water is

2.2 K kg {mol}^{- 1} .

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The correct relation between the elevation in boiling point and the molar mass of a solute is: (

W_{1}

and

W_{2}

are respectively weight of solvent & solute)

HARD

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

If a compound

AB

dissociates to the extent of

75 %

in an aqueous solution, the molality of the solution which shows a

2.5 K

rise in the boiling point of the solution is ___ molal. (Rounded-off to the nearest integer)

[K_{b} = 0.52 K kg {mol}^{- 1}]

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The elevation of boiling point of

0.10 m

aqueous

{CrCl}_{3} . {xNH}_{3}

solution is two times that of

0.05 m

aqueous

{CaCl}_{2}

solution. The value of

x

\dots \dots \dots \dots . .

[Assume

100 %

ionisation of the complex and

{CaCl}_{2},

coordination number of

Cr

6,

and that all

{NH}_{3}

molecules are present inside the coordination sphere]

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

180 g

of glucose,

C_{6} H_{12} O_{6}

is dissolved in

1 kg

of water in a saucepan. At what temperature the solution will boil at

1.013

bar?

(K_{b}

for water is

0.52 K kg {mol}^{- 1})

EASY

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

1 g

of a non-volatile non-electrolyte solute is dissolved in

100 g

of two different solvents

A

and B whose ebullioscopic constants are in the ratio of

1 : 5

. The ratio of the elevation in their boiling points,

\frac{∆ T_{b} (A)}{∆ T_{b} (B)}

, is: (assuming they have the same molar mass)

MEDIUM

Chemistry>Physical Chemistry>Solutions>Elevation in Boiling Point

The boiling point of

0.2 m o l k g^{- 1}

solution of X in water is greater than equimolal solution of Y in water. Which one of the following statements is true in this case?

Why is it more convenient to obtain the molecular weight of an unknown solute by measuring the freezing point depression than by measuring the boiling point elevation?

Important Questions on Solutions

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