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12th Chemistry weekly Test - 1 ( Ionic Equilibrium )

St. Britto Hr. Sec. School - Madurai

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

Time : 1.30 Hours

Part - A

Multiple Choice Question - Answer All Question

If ionic product < solubility product then the solution is_______

saturated
super saturated
unsaturated
none of the above

Pick the odd one out

Cl^-
CaO
SO₂
\({ CH }_{ 3 }^{ - }\)

The degree of hydrolysis of 0.1 M solution of ammonium acetate is 8.48 x 10^-5 The dissociation constant of the weak base is

1.39 X 10^-4·
1.39 X 10^-5
1.45 x 10^-10
1.45 x 10^-9

Addition of sodium chloride to a saturated solution of silver chloride

dissociation of AgCl increases
concentration of Cl^- decreases
dissociation of AgCl^- decreases
concentration of Ag⁺ increases

For two acids A and B, K_a values at 25°C are 2 x 10⁶ and 1.8 x 10^-4 respectively. which among the following is true with respect to the above data.
A and B are equally acidic

A is stronger than B

B is stronger than A

K_a value is not a measure of acid strength
Which one among the following in the strongest Bronsted base
\(Cl{ O }_{ 4 }^{ - }\)

\(Cl{ O }_{ 3 }^{ - }\)

\(Cl{ O }_{2 }^{ - }\)

\(Cl{ O }^{ - }\)

Degree of dissociation \(\alpha \) is

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

A solution which is resistant to changes of pH on addition of small amounts of an acid or a base is known as

buffer solution
true solution
isohydric solution
ideal solution

H₂\({ PO }_{ 4 }^{ - }\) the conjugate base of

\({ PO }_{ 4 }^{ 3- }\)
P₂O₅
H₃PO₄
H\({ PO }_{ 4 }^{ 3- }\)

According to ___ concept, BF₃ acts as a acid.

Bronsted.
Arrhenius
Lewis
None of the above

Dissociation constant ofNH40H is 1.8 x 10^-5 the hydrolysis constant of NH₄Cl would be

1.8 x 10^-19
5.55 x 10^-10
5.55 x 10^-5
1.80 x 10^-5

Part - B

Generic 2 - Answer All Question

Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.
Calculate the pH of 1.5 x 10^-3 M solution of Ba(OH)₂.

How is common ion effect related to the solubility of the electrolyte?

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.

Calculate the ionisation constant for the conjugate base of HF. Ionisation constant of HF at 298 K is 6.8 x I0^-4

The K_w of a neutral solution is 10^-12 at a particular temperature. What are its pH and
pOHvalues?

Part - C

Generic 3 - Answer All Question

What do you mean by auto ionisation of water?
What is Henderson equation?

Define buffer Index.

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

How will you calculate solubility product from molar solubility?

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

Part - D

Generic 5 - Answer All Question

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

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.

Derive Henderson - Hasselbalch equation.

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