Henry's constant (in kbar) for four gases α , β , γ and δ in water at 298 K is given below : α β γ δ K H 50 2 2 × 10 - 5 0 . 5 (density of water = 10 3 k gm - 3 at 298 K ) This table implies that :

The pressure of a 55 . 5 molal solution of δ is 250 bar

α has the highest solubility in water at a given pressure

solubility of γ at 308 K is lower than at 298 K

The pressure of 55 . 5 molal solution of γ is 1 bar .

HARD

Earn 100

A very dilute saturated solution of a sparingly soluble sali $A_{3} B_{4}$ has a vapour pressure of $20 mm$ of $Hg$ at temperature $T$ , while pure water exerts a pressure of $20.0126 mm Hg$ at the same temperature. Calculate the solubility product constant of $A_{3} B_{4}$ at the same temperature.

Important Questions on Solutions

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

The variation of solubility of four different gases

(G 1, G 2, e t c .)

in a given solvent with pressure at a constant temperature is shown in the plot.

Question Image

The gas with the highest value of Henry's law constant is

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

Which one of the following statements regarding Henry's law is not correct?

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

The solubility of pure oxygen in water at

20 ° C

and

1.0

atmosphere pressure is

1.38 \times 10^{- 3}

mol/litre. What will be the concentration of oxygen at

2 θ ° C

and partial pressure of

0.21

atmosphere?

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

${CO}_{2}$ gas is bubbled through water during a soft drink manufacturing process at $298 K$ . If ${CO}_{2}$ exerts a partial pressure of $0.835 bar$ then $x m mol$ of ${CO}_{2}$ would dissolve in $0.9 L$ of water. The value of $x$ is _______. (Nearest integer)

(Henry's law constant for ${CO}_{2}$ at $298 K$ is $1.67 \times 10^{3} bar$ )

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

10.30 m g

O_{2}

is dissolved into a liter of sea water of density

1.03 g / m L

. The concentration of

O_{2}

in ppm is _____________.

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

The Henry's law constant for

O_{2}

dissolved in water is

4.34 \times 10^{4}

atm at certain temperature. If the partial pressure of

O_{2}

in a gas mixture that is in equilibrium with water is

0.434 atm,

what is the mole fraction of

O_{2}

in the solution ?

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

The values of the Henry's law constant of

Ar, {CO}_{2}, {CH}_{4}

and

O_{2}

in water at

25 ° C

are

40.30, 1.67, 0.41

and

34.86 kbar

, respectively. The order of their solubility in water at the same temperature and pressure is

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

The

K_{H}

value

(K

bar) of argon

(I),

carbon dioxide

(II)

, formaldehyde

(III)

and methane

(IV)

are respectively

40.3, 1.67, 1.83 \times 10^{- 5}

and

0.413

298 K .

The increasing order of solubility of gas in liquid is

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

State and explain Henry's law.

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

Henry's constant (in kbar) for four gases $α, β, γ$ and $δ$ in water at $298 K$ is given below :

$\begin{matrix} α & β & γ & δ \\ K_{H} & 50 & 2 & 2 \times 10^{- 5} & 0.5 \end{matrix}$

(density of water $= 10^{3} k {gm}^{- 3}$ at $298 K$ ) This table implies that :

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

The water having more dissolved

O_{2}

is :

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

The solubility of

N_{2}

in water at

300 K

and

500 torr

partial pressure is

0 .01 g L^{- 1} .

The solubility (in

{g L}^{- 1}

) at

750 torr

partial pressure is:

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

Henry's law constant for the solubility of

N_{2}

gas in water at

298 K

1.0 \times 10^{5}

atm. The mole fraction of

N_{2}

in air is

0.8

The number of moles of

N_{2}

from air dissolved in

10

moles of water at

298 K

and

5

atm pressure is

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

The oxygen dissolved in water exerts a partial pressure of $20 kPa$ in the vapour above water. The molar solubility of oxygen in water is ______ $\times 10^{- 5} mol {dm}^{- 3} .$

(Round off to the Nearest Integer).

[Given : Henry's law constant $= K_{H} = 8.0 \times 10^{4} kPa$ for $O_{2} .$ Density of water with dissolved oxygen $= 1.0 kg {dm}^{- 3}$ ]

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

Choose the correct statement

HARD

Chemistry>Physical Chemistry>Solutions>Solubility

A company dissolves ' $x$ ' amount of ${CO}_{2}$ at $298 K$ in $1$ litre of water to prepare soda water. $x = . . . . . . . \times 10^{- 3} g$ . (nearest integer)

(Given: partial pressure of ${CO}_{2}$ at $298 K = 0.835$ bar. Henry's law constant for ${CO}_{2}$ at $298 K = 1.67 kbar$ . Atomic mass of $H, C$ and $O$ is $1, 12$ , and $6 g {mol}^{- 1}$ , respectively)

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

From the graph, the value of Henry's constant for the solubility of $HCl$ gas in cyclohexane is

Question Image

MEDIUM

Chemistry>Physical Chemistry>Solutions>Solubility

{CO}_{2}

and

{CH}_{4}

gases were bubbled through two different one litre water flasks at the same partial pressure of

P

bar at

298 K

. If the Henry's law constants of

{CO}_{2}

and

{CH}_{4}

gases at

298 K

are

1.64, 0.41 k

bar respectively, the mole ratio of

{CO}_{2}

and

{CH}_{4}

gases dissolved in one litre water is

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

For the solution of the gases

w, x, y

and

z

in water at

298 K,

the Henry's law constants

(K_{H})

are

0.5, 2, 35

and

40 k b a r,

respectively. The correct plot for the given data is:

HARD

Chemistry>Physical Chemistry>Solutions>Solubility

Solubility of which among the following solids in water changes slightly with temperature?

A very dilute saturated solution of a sparingly soluble sali A3B4 has a vapour pressure of 20 mm of Hg at temperature T, while pure water exerts a pressure of 20.0126 mm Hg at the same temperature. Calculate the solubility product constant of A3B4 at the same temperature.

Important Questions on Solutions

Learn and Prepare for any exam you want !

A very dilute saturated solution of a sparingly soluble sali $A_{3} B_{4}$ has a vapour pressure of $20 mm$ of $Hg$ at temperature $T$ , while pure water exerts a pressure of $20.0126 mm Hg$ at the same temperature. Calculate the solubility product constant of $A_{3} B_{4}$ at the same temperature.