Ionic Equlibrium Test

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Ionic Equlibrium Test - 4

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Weekly Quiz Competition

Question 1
1 / -0

Statement-1: pH of a buffer solution changes with change in temperature.

Statement-2: K_w of water changes with change in temperature.

A
Both Statement-1 and Statement-2 are true and Statement-2 is the correct explanation of Statement-1.

B
Both Statement-1 and Statement-2 are true and Statement-2 is not the correct explanation of Statement-1.

C
Statement-1 is true but Statement-2 is false.

D
Statement-lisfalsebutStatement-2is true.

Solution

Reason is the correct explanation of Assertion.
Question 2
1 / -0

The number of H⁺ions in 1 cc of a solution, having pH= 13, is equal to

A
6.023 × 10⁷

B
3.45 × 10¹⁶

C
3.45 × 10^–13

D
6.023 × 10¹³

Solution

Given the pH of solution = 13

[H⁺] = 10^-13 mol /litre

= 10^-13 × 6.023 × 10²³ H⁺ ions/litre

= 6.023 × 10¹⁰ H⁺ ions/litre

= 6.023 × 10¹⁰ × 10^-3 H⁺ ions/mL

= 6.023 × 10⁷ H⁺/mL
Question 3
1 / -0

The degree of dissociation of acetic acid in an aqueous solution of the acid is practically unaffected

A
by adding a drop of HCl

B
by raising the temperature

C
by adding a pinch of NaCI

D
by adding water

Solution

Na⁺ion is a weak acid and CI^- ion is a weak base. The reactions CH₃COO^-+ Na⁺→ CH₃COONa
and H⁺ + Cl^- → HCl do not occur.

By adding a drop of HCl, ilonization of CH₃COOH is suppressed due to common ion (H⁺) effect by strong acid HCl.

By adding water and raising the temperature, degree of dissociation increases.
Question 4
1 / -0

Which combinations of reactants will react less than 2% of the theoretically possible extent?

A
NH₃ + H₃O⁺→ NH₄⁺ + H₂O

B
NH₃+H₂O → NH₄⁺ + OH^-

C
CH₃COOH + H₂O → CH₃COC^- +H₃O⁺

D
CH₃COO^-+H₂O → CH₃COOH + OH^-

Solution

CH₃COOH and NH₃ are weak acid and base respectively and ionise in aqueous solution to a small extent.

For CH₃COO^-+H₂O → CH₃COOH + OH^-, hydrolysis of CH₃COO^- ion (conjugate base of weak acid CH₃COOH) occurs to a small extent.

For NH₃ + H₃O⁺→ NH₄⁺ + H₂O, this reaction is acid-base neutralization which goes almost to completion.
Question 5
1 / -0

Buffer solution can be prepared from a mixture of

A
ammonia and sodium hydroxide in water

B
ammonia and ammonium chloride in water

C
sodium acetate and HCl in water

D
sodium acetate and acetic acid in water

Solution

A buffer solution consists of a weak base or weak acid and its salt, a mixture of sodium acetate and HCl in water or ammonia and ammonium chloride in water will not prepare a buffer.

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Ionic Equlibrium Test - 4

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Ionic Equlibrium Test - 4

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Question 1

Both Statement-1 and Statement-2 are true and Statement-2 is the correct explanation of Statement-1.

Both Statement-1 and Statement-2 are true and Statement-2 is not the correct explanation of Statement-1.

Statement-1 is true but Statement-2 is false.

Statement-lisfalsebutStatement-2is true.

Solution

Question 2

6.023 × 107

3.45 × 1016

3.45 × 10–13

6.023 × 1013

Solution

Question 3

by adding a drop of HCl

by raising the temperature

by adding a pinch of NaCI

by adding water

Solution

Question 4

NH3 + H3O+ → NH4+ + H2O

NH3+H2O → NH4+ + OH-

CH3COOH + H2O → CH3COC- +H3O+

CH3COO-+H2O → CH3COOH + OH-

Solution

Question 5

ammonia and sodium hydroxide in water

ammonia and ammonium chloride in water

sodium acetate and HCl in water

sodium acetate and acetic acid in water

Solution

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6.023 × 10⁷

3.45 × 10¹⁶

3.45 × 10^–13

6.023 × 10¹³

NH₃ + H₃O⁺→ NH₄⁺ + H₂O

NH₃+H₂O → NH₄⁺ + OH^-

CH₃COOH + H₂O → CH₃COC^- +H₃O⁺

CH₃COO^-+H₂O → CH₃COOH + OH^-