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 .

MEDIUM

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The molar solubility (in $Mol L^{- 1}$ ) of a sparingly soluble salt ${MX}_{4}$ is ‘s’. The corresponding solubility product is $K_{s p} .$ ‘s’ is given in terms of $K_{s p}$ by the relation :

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Important Questions on Solutions

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

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

EASY

Chemistry>Physical Chemistry>Solutions>Solubility

The water having more dissolved

O_{2}

is :

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

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

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

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

If the

K_{H}

values for

{Ar}_{(g)}, {CO}_{2 (g)}, {HCHO}_{(g)}

and

{CH}_{4 (g)}

respectively are

40.39, 1.67

1.83 \times 10^{- 5}

and

0.413

, then identify the correct increasing order of their solubilities.

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

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

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 _____________.

HARD

Chemistry>Physical Chemistry>Solutions>Solubility

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

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

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

Assume that

{CO}_{2}

exerts a partial pressure of

0.9

bar on the surface of

200 mL

water contained in a cup. The number of moles of

{CO}_{2}

dissolved in water is
[Henry's law constant for

{CO}_{2}

298 K = 10^{5}

bar; density of water at

298 K = 1 g {mL}^{- 1}

;

molar

mass of

{CO}_{2} = 44 g {mol}^{- 1}

; molar mass of water

= 18 g {mol}^{- 1}

]

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

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

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:

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:

The molar solubility (in Mol L -1 ) of a sparingly soluble salt MX 4 is ‘s’. The corresponding solubility product is K sp . ‘s’ is given in terms of K sp by the relation :

Important Questions on Solutions

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The molar solubility (in $Mol L^{- 1}$ ) of a sparingly soluble salt ${MX}_{4}$ is ‘s’. The corresponding solubility product is $K_{s p} .$ ‘s’ is given in terms of $K_{s p}$ by the relation :