MEDIUM

Earn 100

Mass of ethylene glycol (antifreeze) to be added to $18.6 kg$ of water to protect the freezing point at $- 24 ° C$ is $kg$ (Molar mass in ${gmol}^{- 1}$ for ethylene glycol $62, K_{f}$ of water $= 1.86 K kg {mol}^{- 1}$ )

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Important Questions on Solutions

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

The elevation in boiling point for

1

molal solution of glucose is

2 K

. The depression in freezing point for

2

molal solution of glucose in the same solvent is

2 K .

The relation between

K_{b}

and

K_{f}

is:

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

How much amount of

N a C l

should be added to

600 g

of water

(ρ = 1.00 g / m L)

to decrease the freezing point of water to

- 0.2^{o} C

? ________. (The freezing point depression constant for water

= 2 K k g {m o l}^{- 1}

)

EASY

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

5 %

solution (by mass) of cane sugar in water has freezing point of

271 K

. Calculate the freezing point of

5 %

glucose in water if freezing point of pure water is

273.15 K

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

A solution containing

62 g

ethylene glycol in

250 g

water is cooled to

- 10^{o} C

. If

K_{f}

for water is

1.86 K kg {mol}^{- 1}

, the amount of water (in

g

) separated as ice is:

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

For

1 molal

aqueous solution of the following compounds, which one will show the highest freezing point?

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

Which of the following

0.1 M

aqueous solution will have lowest freezing point?

EASY

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

Of the following

0.10 m

aqueous solutions, which one will exhibit the largest freezing point depression?

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

When

36 g

of a non-volatile, non-electrolytic solute have the empirical formula

{CH}_{2} O

is dissolved in

1.2 kg

of water, the solution freezes at

- 0.93 ° C

. The molecular formula of the solute is (

K_{f}

of water

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

)

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

Pure water freezes at

273 K

and

1 bar

pressure. The addition of

34.5 g

of ethanol to

500 g

of water changes the freezing point of the solution. Use the freezing point depression constant of water as

2 K kg {mol}^{- 1}

. The figures shown below represent the plots of vapour pressure (

V . P .

) versus temperature (

T

). [Molecular weight of ethanol is 46 g

46 g {mol}^{- 1}

]

Among the following, the option representing a change in the freezing point is

HARD

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

On dissolving $0.5 g$ of a non-volatile non-ionic solute to $39 g$ of benzene, its vapor pressure decreases from $650 m m H g$ to $640 m m H g .$ The depression of freezing point of benzene (in $K$ ) upon addition of the solute is _______

(Given data: Molar mass and the molal freezing point depression constant of benzene are $78 g m o l^{- 1}$ and $5.12 K k g m o l^{- 1},$ respectively)

Give your answer up to three significant figures.

HARD

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

When

2.44

grams of benzoic acid

(C_{6} H_{5} COOH)

dissolved in

25

grams of benzene, it shows depression of freezing point equal to

2.2 K

. Molal depression constant of benzene is

5.0 K kg {mol}^{- 1}

. What is the percentage association of acid, if it forms dimer in solution?

HARD

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

5 g

{Na}_{2} {SO}_{4}

was dissolved in

x g

H_{2} O

. The change in freezing point was found to be

3 {.82}^{o} C

. If

{Na}_{2} {SO}_{4}

81.5 %

ionised, the value of

x

(

K_{f}

for water

= 1 {.86}^{o} C kg {mol}^{- 1}

) is approximately:

(molar mass of

S = 32 g {mol}^{- 1}

and that of

Na = 23 g {mol}^{- 1}

)

HARD

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

The freezing point depression of

0.001 M

A_{x} B_{y} [Fe {(CN)}_{6}]

5.58 \times 10^{- 3} K

. If the oxidation state of

Fe

+ 2

and

K_{f} = 1.86 K {kgmol}^{- 1}

, then the total number of possibilities for different types of

A

and

B

cations are

EASY

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

The freezing point depression constant

(K_{f})

of benzene is

5.12 K kg {mol}^{- 1}

. The freezing point depression for the solution of molality

0.078 m

containing a non-electrolyte solute in benzene is (rounded off upto two decimal places):

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

The mass of sucrose in grams (molar mass of sucrose is

(

342 g {mol}^{- 1}

)

required to be dissolved in

100 g

of water, in order to produce a solution with

104.74 ° C

as the difference between the boiling point and freezing point is

(K_{f (H_{2} O)} = 1.86 K kg {mol}^{- 1}

and

K_{b (H_{2} O)} = 0.51 K kg {mol}^{- 1})

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

Benzene freezes at

5.6 ° C

. Its

K_{f}

value is

5.1

. The value of

Δ H_{fus}

is:

EASY

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

K_{f}

(water)

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

. The temperature at which ice begins to separate from a mixture of

10

mass

%

ethylene glycol is

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

Molal depression constant for a solvent is

4.0 K k g m o l^{- 1} .

The depression in the freezing point of the solvent for

0.03 m o l k g^{- 1}

solution of

K_{2} S O_{4}

is:
(Assume complete dissociation of the electrolyte)

EASY

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

If molality of the dilute solution is doubled, the value of molal depression constant

(K_{f})

will be

MEDIUM

Chemistry>Physical Chemistry>Solutions>Depression of Freezing Point

The freezing point of benzene decreases by ${0.45}^{°} C$ on adding $0.2 g$ of acetic acid to $20 g$ of benzene. If acetic acid associates to form a dimer in benzene, then what is the percentage association of acetic acid in benzene?

$(K_{f} for benzene = 5 .12 K kg {mol}^{- 1})$

Mass of ethylene glycol (antifreeze) to be added to 18.6 kg of water to protect the freezing point at -24°C is kg (Molar mass in gmol-1 for ethylene glycol 62, Kf of water =1.86 K kg mol-1)

Important Questions on Solutions

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Mass of ethylene glycol (antifreeze) to be added to $18.6 kg$ of water to protect the freezing point at $- 24 ° C$ is $kg$ (Molar mass in ${gmol}^{- 1}$ for ethylene glycol $62, K_{f}$ of water $= 1.86 K kg {mol}^{- 1}$ )