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12th Chemistry weekly Test - 2 ( Ionic Equilibrium )

St. Britto Hr. Sec. School - Madurai

12th Chemistry weekly Test - 2 ( Ionic Equilibrium )-Aug 2020

Time : 1.30 Hours

Part - A

Multiple Choice Question - Answer All Question

The Lewis base among the following is______

BF₃
NH₃
AlCl₃
\({ NH }_{ 4 }^{ + }\)

Ionic product of water increases when

Pressure decreases
H⁺ ions are added
OH^- ions are added
temperature increases

pH of0.05 M H₂SO₄ is

1
2.6990
1.3010
1.6990

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

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

pH of buffer depends upon concentration of

acid (H⁺)
Conjugate base (OH^-)
Salt
Both (a) and (b)

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅NH) in a 0.10M aqueous pyridine solution (K_b for C₅H₅N =1.7 x l0^-9) is

0.006%
0.013%
0.77%
1.6%

If ionic product < solubility product then the solution is_______

saturated
super saturated
unsaturated
none of the above

The pH of a solution containing 0.1 N NaOH solution is

1
10^-1
13
10^-13

___ can acts as both bronsted acid and Bronsted base.

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

The pH of 10^-5 M KOH solution will be

9
5
19
none of these

Which will make basic buffer?

50 mL of 0.1M NaOH +25mL of 0.1M ch₃cooh
100 mL of 0.1M CH₃COOH + 100 mL of 0.1m NH₄OH
100 mL of 0.1M HCl + 200 mL of 0.1M NH₄OH
100 mL of 0.1M HC1 + 100 mL of 0.1M NaOH

Buffer index is

\(\beta =\frac { dB }{ { pK }_{ a } } \)
\(\beta =\frac { dB }{ { d(pH) } } \)
\(\beta =\frac { dB }{ { pH } } \)
\(\beta =\frac { dB }{ { pOH } } \)

MY and NY₃, are insoluble salts and have the same K_sp values of 6.2 x l0^-13 at room sp temperature. Which statement would be true with regard to MY and NY₃?

The salts MY and NY₃ are more soluble in O.5 M KY than in pure water
The addition of the salt of KY to the suspension of MY and NY₃ will have no effect on their solubility's
The molar solubilities of MY and NY₃ in water are identical
The molar solubility of MY in water is less than that of NY₃

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

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

Which one of the following is correct?

pH = H⁺
pH= -log₁₀ H⁺
pH = log₁₀ H⁺
pH = 2log₁₀ H⁺

Analyses the equilibrium

HClO₄ + H₂O \(\rightleftharpoons \) H₃O⁺ + \({ ClO }_{ 4 }^{ - }\)

and choose the correct statement.

H₃O⁺ is the conjugate base of H₂O
\({ ClO }_{ 4 }^{ - }\)is the conjugate base of HClO₄
H₂O is the conjugate acid of H₃O⁺
HClO₄ is the conjugate acid of H₃O⁺

An example of basic buffer is

NH₄OH and NH₄Cl
NH₄OH and NaOH
NaOH and NH₄Cl
NaOH and KOH

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)

K_wrepresents

ionic product constant of water
Solubility product of water
Equilibrium constant of water
Buffer index

Part - B

Generic 5 - Answer All Question

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 Henderson - Hasselbalch equation.

Derive the relationship between pH and pOH.

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

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

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