Degree of Dis...

Degree of Dissociation

Trending Questions

What is ionic product of water ?

When $0.004 M N a_{2} S O_{4}$ is isotonic with 0.01M solution of glucose at same temperature.the apparent degree of dissociation of sodium sulphate is

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What is the percentage strength of the $11.2 L$ volume solution of $H_{2} O_{2}$ ?

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Q. The values of

K_{P 1}

and

K_{P 2}

for the reactions,

X ⇌ Y + Z . . . (i) A ⇌ 2 B . . . (i i)

are in the ratio

9 : 1

. If the initial concentrations and the degrees of dissociation of

X

and

A

are equal, then the smallest ratio of total pressures at equilibrium

(i)

and

(i i)

x : y

. Find the value of

x + y

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Q. The unit of ionic product of water

(K_{w})

is:

$L m o l^{- 1}$
$m o l^{- 2} L^{2}$
$m o l L^{- 1}$
$m o l^{2} L^{- 2}$

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Q. The equilibrium constant

K_{p}

for the reaction

2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g)

1000 K

is 3.5. What would be the partial pressure of

O_{2}

gas with equal moles of

S O_{2}

and

S O_{3}

at equilibrium?

0.29 atm
3.50 atm
0.53 atm
1.87 atm

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An aqueous solution of $B a C l_{2}$ (1.28gm in 100gm of water)boils at ${100.0832}^{\circ}$ at 1 atm. Calculate the degree of dissociation. ( $K_{b}$ of water is 0.512 k/m)

0.5
0.75
0.85
0.6

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Q. For a given reaction

H_{2} O (l) ⇌ H_{2} O (g)

takes place in closed vessel at a constant temperature,

p_{H_{2} O}

is the vapour pressure of

H_{2} O

. The equilibrium constant,

K_{p}

is given by

$K_{P} = p_{H_{2} O (g)}$
$K_{P} = K_{C} = 1$
$K_{p} = p_{H_{2} O}^{2}$
None of the above

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Q. The equilibrium

S O_{2} (g) + 1 / 2 O_{2} (g) ⇌ S O_{3} (g)

is established in a container of

4 L

at a particular temperature. If the number of moles of

S O_{2} (g), O_{2} (g)

and

S O_{3} (g)

at equilibrium are

2, 1

and

4

respectively, then find the value of the equilibrium constant.

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Q. At

50^{o} C,

the self-ionisation constant (ionic product) of

N H_{3}

is given as,

K_{N H_{3}} = [N H_{4}^{+}] [N H_{2}^{-}] = 10^{- 30} M^{2}

.
How many

N H_{2}^{-}

ions are present per

m m^{3}

of pure liquid ammonia?

$600 i o n s / m m^{3}$
$6 \times 10^{4} i o n s / m m^{3}$
$6 \times 10^{5} i o n s / m m^{3}$
$6 \times 10^{3} i o n s / m m^{3}$

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Q. In aqueous solution the ionization constants for carbonic acid are

K_{1} = 4.2 \times 10^{- 7}

and

K_{2} = 4.8 \times 10^{- 11}

Select the correct statement for a saturated 0.04 M solution of the carbonic acid

The concentration of $C O_{3}^{2 -}$ 0.034 M.
The concentration of $C O_{3}^{2 -}$ is greater than that of $H C O_{3}^{-}$
The concentrataion of $H^{+}$ and $H C O_{3}^{-}$ are approximately equal.
The concentration of $H^{+}$ is double that of $C O_{3}^{2 -}$

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Q. For water at

100^{\circ} C

and 1 bar,

Δ H_{vap} - Δ U_{vap}

x \times 10^{2} {J mol}^{- 1}

The value of x (Round off to the Nearest Integer) is
[Use :

R = 8.31 {mol}^{- 1} K^{- 1}

]
[Assume volume of

H_{2} O (l)

is much smaller than volume of

H_{2} O (g)

. Assume

H_{2} O (g)

can be treated as an ideal gas]

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Q. Anhydrous calcium chloride is often used as a desiccant. In the presence of excess of

C a C l_{2}

, the amount of the water taken up is governed by

K_{P} = 6.4 \times 10^{85}

for the following reaction at room temperature,

C a C l_{2} (s) + 6 H_{2} O (g) ⇌ C a C l_{2} . 6 H_{2} O (s) .

What is the equilibrium vapour pressure of water in a closed vessel that contains

C a C l_{2} (s) ?

$5 \times 10^{- 13} a t m$
$5 \times 10^{- 15} a t m$
$5 \times 10^{- 14} a t m$
$5 \times 10^{- 11} a t m$

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Q. Calculate the percentage dissociation of

H_{2} S (g)

0.1

mole of

H_{2} S

is kept in

0.4

litre vessel at

1000

K for the reaction,

2 H_{2} S (g) ⇌ 2 H_{2} (g) + S_{2} (g)

The value of

K_{c}

1.0 \times 10^{- 6}

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Q. What will be the percentage degree of dissociation of

0.2 M

acetic acid

(C H_{3} C O O H)

solution with

K_{a} = 1.8 \times 10^{- 5}

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Q. An equilibrium mixture in a vessel of capacity

100

litre contain

1 m o l N_{2}, 2 m o l O_{2}

and

3 m o l N O

. Number of moles of

O_{2}

to be added so that so that at new equilibrium the concentration of

N O

is found to be

0.04 m o l / L

$\frac{101}{9}$
None of these
$\frac{101}{18}$
$\frac{202}{9}$

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Q. An unknown compound A dissociates at

500^{\circ} C

to give products as follows:

A (g) ⇌ B (g) + C (g) + D (g)

Vapour density of the equilibrium mixture is 60 when it dissociates to the extent to

20^{%}

. What will be the molecular weight (in grams) of Compound A

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Q. If the degree of dissociation of water at

70^{o} C

1.28 \times 10^{- 8}

. Then what is the ionic product of water at this temperature?

$25 \times 10^{- 16} M^{2}$
$1.52 \times 10^{- 14} M^{2}$
$5.1 \times 10^{- 13} M^{2}$
$1.28 \times 10^{- 8} M^{2}$

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Q. The percentage degree of dissociation of

0.05 M

acetic acid

(C H_{3} C O O H)

solution with

K_{a} = 1.8 \times 10^{- 5}

is :

0.55
5.5
1.9
19

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The solubility product at $298 K$ is $6 \times 10^{- 31}$ , what is the concentration of hydroxide ions in a saturated solution?

${(18 \times 10^{- 31})}^{1 / 4}$
${(18 \times 10^{- 31})}^{1 / 2}$
${(2.22 \times 10^{- 31})}^{1 / 34}$
${(4.86 \times 10^{- 29})}^{1 / 4}$

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Q. 1.50 mol each of hydrogen and iodine were placed in a sealed 10 L container maintained at 717 K. At equilibrium 1.25 mol each of hydrogen and iodine were left behind. The equilibrium constant,

K_{c}

for the reaction

H_{2} (g) + I_{2} (g) ⇌ 2 H I (g) a t 717 K

0.40
0.16
25
50

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Q. Which of the following is incorrect for degree of dissociation

(α)

The value of $α$ can be any value from 0 to 1
$α$ can be a fractional value
$α$ has no units
None of the above

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A (g) \to B (g)

For the above reaction involving gaseous reactants and gaseous products, the concentration is expressed in terms of pressure. Then the unit of rate of reaction will be:

$a t m$
$a t m . s$
$a t m^{2} . s$
$a t m s^{- 1}$

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Q. Why does the solubility of alkaline earth metal carbonates and sulphates in water decrease down the group?

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B O H

is a weak base.Molar concentration of BOH that provides a

[O H^{-}] of 1.5 \times 10^{- 3} M [K_{b} [B O H] = 1.5 \times 10^{- 5} M]

is:

$0.15 M$
$0.01515 M$
$0.0015 M$
$0.5 \times 10^{- 5} M$

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Q. Which of the following is the correct statement(s) regarding

K_{a_{1}}

for the first dissociation and

K_{a_{2}}

for the second dissociation of a polyprotic acid

H_{2} C O_{3}

$K_{a_{1}}$ has less value than $K_{a_{2}}$
$H_{i o n}^{+}$ from $H_{2} C O_{3}$ is more easier to obtain compared to $H_{i o n}^{+}$ from $H C O_{3}^{-}$
$K_{a_{1}}$ has more value than $K_{a_{2}}$
$[H^{+}]$ from $H_{2} C O_{3}$ is is more difficult to obtain as compared to $H_{i o n}^{+}$ from $H C O_{3}^{-}$

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Q. Consider the reaction

N_{2} O_{4} (g) ⇌ 2 N O_{2} (g) .

The temperature (in kelvin) at which

K_{C} = 20.4

and

K_{P} = 600.1

is (Round off to the Nearest Integer) Assume all gases are ideal and

R = 0.0831 L b a r K^{- 1} m o l^{- 1}

]

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Q. The percentage dissociation

(α)

C H_{3} C O O H

having dissociation constant

K_{a} = 1.8 \times 10^{- 5} M

is given as

5

%.
Find the inital concentration of

C H_{3} C O O H

$2.44 \times 10^{- 2} M$
$1.98 \times 10^{- 2} M$
$1.28 \times 10^{- 3} M$
$6.84 \times 10^{- 3} M$

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Q. Consider a weak base,

B O H

. Molar concentration of

B O H

that provides

[O H]^{-}

1.5 \times 10^{- 3} M

will be :
Given:

K_{b} (K O H) = 1.5 \times 10^{- 5}

$1.5 \times 10^{- 2} M$
$0.015 M$
$1.5 \times 10^{- 4} M$
$0.15 M$

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Q. What will be the

H^{+}

ion concentration of 0.01 M

H C N

solution at equilibrium, if it is 20% ionised?

$2 \times 10^{- 3} M$
$3 \times 10^{3} M$
$5 \times 10^{3} M$
$1 \times 10^{3} M$

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