Ionic Equilibrium Test

Result

Ionic Equilibrium Test - 6

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Weekly Quiz Competition

Question 1
1 / -0

The pH of a solution obtained by dissolving 5 × 10⁻⁴ moles of Ca(OH)₂ (strong electrolyte) to 100 ml solution at 298 K will be

A
11

B
12

C
9.8

D
2

Solution
Question 2
1 / -0

One litre of a saturated solution of CaCO₃ is evaporated to dryness due to which 7.0 mg of residue is left. The solubility product for CaCO₃ is

A
4.9 × 10⁻⁸

B
4.9 × 10⁻⁵

C
4.9 × 10⁻⁹

D
4.9 × 10⁻⁷

Solution

Moles of CaCO₃in residue

Moles of CaCO₃ in 1 litre solution = 7 × 10⁻⁵
Question 3
1 / -0

The hydrolysis constant for ZnCl₂ will be

Where, K_b is effective dissociation constant of base Zn⁺⁺

A

B

C

D

Solution

Zn⁺⁺+ 2H₂O ⇌ Zn(OH)₂ + 2H⁺

Zn(OH)₂ ⇌ Zn⁺⁺ + 2OH^–

K_w = [H⁺ ] [OH^– ]
Question 4
1 / -0

M(OH)_x has K_SP 4 × 10^–12 and solubility 10^–4M. Then the value of x is

A
1

B
2

C
3

D
–4

Solution

M(OH)_x will ionize in the way

M(OH)_x ⇌ M^+x + x OH^–

10^–4 x × 10^–4

∴ K_sp = [M^+x] [OH^– ]^x

∴ (10^–4) (x × 10^–4)^x = 4 × 10^–12

by inspection we get this relation will hold good when x = 2
Question 5
1 / -0

For a weak electrolyte α₁ and α₂ are in ratio of 1: 2, for a given concentration ^k_a₁ = 2 ×10⁻⁴ . What will be value of ^k_a₂ ?

A
8 × 10^–4

B
2 × 10^–4

C
4 × 10^–4

D
1 × 10^–4

Solution
Question 6
1 / -0

Consider the reaction A⁻+ H₃O⁺⇌ HA + H₂O. The K_a value for acid HA is 1.0 × 10⁻⁶ . What is the value of K for this reaction.

A
1.0 × 10⁶

B
1.0 × 10⁻⁸

C
1.0 × 10⁸

D
1.0 × 10⁻⁶

Solution

The reaction is the reverse of the ionization reaction of HA, hence the equilibrium constant is the reciprocal of K_a.
Question 7
1 / -0

The ionization constant of HCO₂H is 1.8 × 10⁻⁴ . What is the percent ionization of a 0.001 M solution?

A
66%

B
42%

C
34%

D
58%

Solution
Question 8
1 / -0

At −50°C, the self−ionization constant (ion product) is How many amide ions are present per mm³ of pure liquid ammonia?

A
600 ions/mm³

B
6 × 10⁶ ions/mm³

C
6 × 10⁴ ions/mm³

D
60 ions/mm³

Solution
Question 9
1 / -0

The degree of dissociation of anilinium acetate is

A
independent of initial concentration

B
directly proportional to initial concentration

C
inversely proportional to initial concentration

D
inversely proportional to square root of initial concentration

Solution
Question 10
1 / -0

10 ml of 0.2 M acid is added to 250 ml of a buffer solution with pH = 6.34 and the pH of the solution becomes 6.32. The buffer capacity of the solution is

A
0.1

B
0.2

C
0.3

D
0.4

Solution