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12th Chemistry Monthly Test -1 (Ionic Equilibrium)

St. Britto Hr. Sec. School - Madurai

12th Chemistry Monthly Test -1 (Ionic Equilibrium) -Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

Which of the following relation is correct for degree of hydrolysis of ammonium acetate?

\(h=\sqrt { \frac { { K }_{ h } }{ C } } \)
h = \(\sqrt { \frac { { K }_{ a } }{ { K }_{ b } } } \)
h = \(\sqrt { \frac { { K }_{ h } }{ { { K }_{ a }.K }_{ b } } } \)
h = \(\sqrt { \frac { { { K }_{ a }.K }_{ b } }{ { K }_{ h } } } \)

According to Lowry - Bronsted theory, an acid is a_______

electron donor
electron acceptor
proton donor
profon acceptor

___ can acts as both bronsted acid and Bronsted base.

\({ NH }_{ 4 }^{ + }\)
Cl^-
\({ HCO }_{ 3 }^{ - }\)
H₃O⁺

Pick out the incorrect statement regarding Lewis acids and bases.

A Lewis acid is a electron deficient molecule
Lewis bases is one which donates an electron pair
Lewis base is a cation
Both (a) and (c)

A drop of hydrochloric acid is added to pure water, its pH______

increases
decreases
increases and then decreases
resist the change in pH and so remains unaltered

An acid is a substance that dissociates to give hydrogen ions in water. The above concept of acids was proposed by______

Lewis
Arrhenius
Bronsted
Lowry

HCI is a strong acid since

It can be easily oxidised
It can be easily ionised
It dissociates completely to give H⁺ ions in solution
Both (a) and (b)

Which of the following is not a Lewis acid?

SiCl₄
AlCl₃
SO₃
CO

What is the decreasing order of strength of bases?
OH^-, \({ NH }_{ 2 }^{ - }\) H - C ≡ C and CH₃ - \({ NH }_{ 2 }^{ - }\)

OH^-> \({ NH }_{ 2 }^{ - }\) > H - C ≡ C^-> CH₃- \({ CH }_{ 2 }^{ - }\)
\({ NH }_{ 2 }^{ - }\) > OH^- > CH₃ - \({ CH }_{ 2 }^{ - }\) > H - C ≡ C
CH₃ - CH₂ > \({ NH }_{ 2 }^{ - }\) > H - C ≡ C^- > OH^-
OH^- > H - C ≡ C^- > CH - \({ CH }_{ 2 }^{ - }\) > \({ NH }_{ 2 }^{ - }\)

The hydrogen ion concentration of a buffer acids and bases solution consisting of a weak acid and its salts is given by

[H⁺] = \(\frac { { K }_{ a }\left[ acid \right] }{ [salt] } \)
[H⁺] = K_a [salt]
[H⁺] = K_a [acid]
[H⁺]\(\frac { { K }_{ a }\left[ salt \right] }{ [acid] } \)

The conjugate base of \({ NH }_{ 2 }^{ - }\) is

NH^-
NH₃
\({ NH }_{ \ 3 }^{ \ + }\)
NH^2-

Degree of dissociation \(\alpha \) is

\(\alpha =\frac { { { K }_{ a } } }{ C } \)
\(\alpha =\frac { { { C }^{ 2 } } }{ { K }_{ a } } \)
\(\alpha =\sqrt { \frac { { K }_{ a } } { { C } }} \)
\(\alpha =\sqrt { \frac { { C } }{ { K }_{ a } } } \)

Pick the strongest conjugate base among the following

Cl^-
\({ NO }_{ 2 }^{ - }\)
\({ SO }_{ 4 }^{ 2- }\)
CH₃COO^-

According to ___ concept, BF₃ acts as a acid.

Bronsted.
Arrhenius
Lewis
None of the above

The pH of a solution containing 0.1 N NaOH solution is

1
10^-1
13
10^-13

Part - B

Generic 2 - Answer All Question

Write down the conjugate acid and base of the following

(i) NH3 (Iii) \({ HSO }_{ 4 }^{ - }\)

Define Buffer solution.

Write the expression for the solubility product of Hg₂Cl₂.

Why is aqueous solution of FeCl₃ acidic?

Give the Limitations of Arrhenius concept theory of acids and bases.

Will a precipitate be formed when 0.150 L of 0.1 M Pb(NO₃)₂ and 0.100 L of 0.2 M NaCl
are mixed? K_sp (PbCl₂) = 1.2 X 10^-5

Calculate the extent of hydrolysis and the pH of 0.1 M ammonium acetate Given that K_a = K_b = 1.8 x 10^-5.

Indentify the conjugate acid base pair for the following reaction in aqueous solution.
i) \({ HS }^ -_{ aq }\) + HF\(\rightleftharpoons \) \({ F }^ -_{ aq }\) + H₂S(aq)
ii) HP\({ O }_{ 3 }^{ 2- }\)- + \({ SO }_{ 3 }^{ 2- }\)\(\rightleftharpoons \) \({ PO }_{ 4 }^{ 3- }\) + \({ HSO }_{ 3 }^{ - }\)
iii) \({ NH }_{ 4 }^{ + }\) +\({ CO }_{ 3 }^{ 2- }\) \(\rightleftharpoons \) NH₃ + \({ HCO }_{ 3 }^{ - }\)

Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.

What are the limitations of Ostwald's dilutionlaw?

K_sp of AgCl is 1.8 x 10^-10. Calculate molar solubility in 1 M AgNO₃

Ksp of Ag2Cr04 is 1.1 X 10^-12. what is solubility of Ag₂CrO₄ in 0.1M K₂CrO₄.

When aqueous ammonia is added to CuSO₄ solution, the solution turns deep blue due to the formation of tetramminecopper (II) complex, [Cu(H₂O)₄]_(aq)²⁺ + 4NH₃(aq) \(\rightleftharpoons \) [Cu(NH₃)₄] _(aq)²⁺, among H₂O and NH₃ Which is stronger Lewis base.

Define solubility product.

The concentration of hydroxide ion in a water sample is found to be 2.5 x 10^-6 M. Identify the nature of the solution.

50 ml of 0.05 M HNO₃ is added to 50 ml of 0.025 M KOH. Calculate the pH of the resultant solution.

Calculate the pH of 1.5 x 10^-3 M solution of Ba(OH)₂.

Part - C

Generic 3 - Answer All Question

What do you mean by buffer action?

What is Henderson equation?

Define buffer Index.

For an aqueous solution of NH₄Cl, prove that \(\left[ H^{ + } \right] =\sqrt { { K }_{ a }.C } \)

What do you mean by auto ionisation of water?

How will you calculate solubility product from molar solubility?

Based on Arrhenius concept, define acid and bases and give an example for each.

Part - D

Generic 5 - Answer All Question

Derive Henderson - Hasselbalch equation.

Derive the hydrolysis constant for the hydrolysis of salt of strong base and weak acid. Deduce its pH.

Derive the relationship between pH and pOH.

Explain buffer action in an acidic buffer.

On hydrolysis of salts of strong acid and strong base, the solution obtained is neutral. Justify your answer with a suitable example.

Derive an expression for the hydrolysis constant for the hydrolysis of salt of weak acid and weak base.

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