# Ionic Equilibrium Test 7

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:An aqueous solution of ammonia consists of

$${H^ + }$$

$$O{H^ - }$$

$$NH_4^ +$$

$$NH_4^ +$$ and $$O{H^ - }$$

## Questions 2 of 50

Question:$$N{H_4}OH$$ is weak base because

It has low vapour pressure

It is only slightly ionized

It is not a hydroxide of metal

It has low density

## Questions 3 of 50

Question:Correct statement is

$$N{H_4}Cl$$gives alkaline solution in water

$$C{H_3}COONa$$ gives acidic solution in water

$$C{H_3}COOH$$ is a weak acid

$$N{H_4}OH$$ is a strong base

## Questions 4 of 50

Question:$$C{l^ - }$$is the conjugate base of

$$HCl{O_4}$$

$$1 \times {10^{ - 5}},$$

$$C{H_3}COONa$$

$$HCl{O_3}$$

## Questions 5 of 50

Question:The strongest base from the following species is

$$N{H^{2 - }}$$

$$O{H^ - }$$

$${O^{2 - }}$$

$${S^{2 - }}$$

## Questions 6 of 50

Question:The compound HCl behaves as …. in the reaction, $$HCl + HF \to H_2^ + Cl + {F^ - }$$

Weak base

Weak acid

Strong base

Strong acid

## Questions 7 of 50

Question:The conjugate base of a strong acid is a

Strong base

Strong acid

Weak acid

Weak base

## Questions 8 of 50

Question:The conjugate base of sulphuric acid is

Sodium hydroxide

Hydrochloric acid

Bisulphate ion

Barium hydroxide

## Questions 9 of 50

Question:Which is strongest Lewis base

$$Sb{H_3}$$

$$As{H_3}$$

$$P{H_3}$$

$$N{H_3}$$

## Questions 10 of 50

Question:Phenolphthalein does not act as an indicator for the titration between

$$NaOH$$ and $$C{H_3}COOH$$

$${H_2}{C_2}{O_4}$$ and $$KMn{O_4}$$

$$Ba{(OH)_2}$$ and $$HCl$$

$$KOH$$and $${H_2}S{O_4}$$

## Questions 11 of 50

Question:Which is not example of Bronsted Lowry theory

$$AlC{l_3}$$

$${H_2}S{O_4}$$

$$S{O_2}$$

$$HN{O_3}$$

## Questions 12 of 50

Question:When $$FeC{l_3}$$ gets soluble in water, then its solution represents which of the characteristics

Amphoteric

Acidic

Basic

Neutral

## Questions 13 of 50

Question:Lewis acid are those substances

Which accept electron pair

Which provide $${H^ + }$$ion in the solution

Which give electron pair

Which accept $$O{H^ - }$$ion

## Questions 14 of 50

Question:For an aqueous solution, the characteristic species of acid is

$${H^ + }$$ion

$${H_3}{O^ + }$$ion

$${H_2}^ +$$ion

$${H_4}{O^ + }$$ion

## Questions 15 of 50

Question:Which is a Lewis base

$${B_2}{H_6}$$

$$LiAl{H_4}$$

$$Al{H_3}$$

$$N{H_3}$$

## Questions 16 of 50

Question:Let the solubility of an aqueous solution of $$Mg{(OH)_2}$$ be x then its $${k_{sp}}$$ is

$$4{x^3}$$

$$108{x^5}$$

$$27{x^4}$$

$$9x$$

## Questions 17 of 50

Question:The solubility product of $$BaS{O_4}$$ at $$25^\circ C$$ is $$1.0 \times {10^{ - 9}}$$. What would be the concentration of $${H_2}S{O_4}$$ necessary to precipitate $$BaS{O_4}$$ from a solution of $$0.01\,M\,B{a^{2 + }}$$ions

$${10^{ - 9}}$$

$${10^{ - 8}}$$

$${10^{ - 7}}$$

$${10^{ - 6}}$$

## Questions 18 of 50

Question:Which is the correct alternate for hydrolysis constant of $$N{H_4}CN$$

$$\sqrt {\frac{{{K_w}}}{{{K_a}}}}$$

$$\frac{{{K_w}}}{{{K_a} \times {K_b}}}$$

$$\sqrt {\frac{{{K_b}}}{c}}$$

$$\frac{{{K_a}}}{{{K_b}}}$$

## Questions 19 of 50

Question:Which of the following salts undergoes hydrolysis

$$C{H_3}COONa$$

$$KN{O_3}$$

$$NaCl$$

$${K_2}S{O_4}$$

## Questions 20 of 50

Question:At 298 K, the solubility product of $$PbC{l_2}$$ is $$1.0 \times {10^{ - 6}}$$. What will be the solubility of $$PbC{l_2}$$in moles/litre

$$6.3 \times {10^{ - 3}}$$

$$1.0 \times {10^{ - 3}}$$

$$3.0 \times {10^{ - 3}}$$

$$4.6 \times {10^{ - 14}}$$

## Questions 21 of 50

Question:Solubility product is

The ionic product of an electrolyte in its saturated solution

The product of the solubilities of the ions of the electrolyte

The product of solubilities of the salts

The product of the concentration of the ions

## Questions 22 of 50

Question:The solubility product of a sparingly soluble salt $$AB$$ at room temperature is $$1.21 \times {10^{ - 6}}$$. Its molar solubility is

$$1.21 \times {10^{ - 6}}$$

$$1.21 \times {10^{ - 3}}$$

$$1.1 \times {10^{ - 4}}$$

$$1.1 \times {10^{ - 4}}$$

## Questions 23 of 50

Question:The precipitation occurs if ionic concentration is

Less than solubility product

More than solubility product

Equal to solubility product

None of these

## Questions 24 of 50

Question:Which of the following cannot be hydrolysed

A salt of weak acid and strong base

A salt of strong acid and weak base

A salt of weak acid and weak base

A salt of strong acid and strong base

## Questions 25 of 50

Question:$$pH$$of water is 7. When a substance $$Y$$is dissolved in water, the $$pH$$becomes 13. The substance $$Y$$is a salt of

Strong acid and strong base

Weak acid and weak base

Strong acid and weak base

Weak acid and strong base

## Questions 26 of 50

Question:In which of the following salt hydrolysis takes place

$$KCl$$

$$NaN{O_3}$$

$$C{H_3}COOK$$

$${K_2}S{O_4}$$

## Questions 27 of 50

Question:At $${90^o}C$$ pure water has $$[{H_3}{O^ + }] = {10^{ - 6}}\,M,$$ the value of $${K_w}$$ at this temperature will be

$${10^{ - 6}}$$

$${10^{ - 12}}$$

$${10^{ - 14}}$$

$${10^{ - 8}}$$

## Questions 28 of 50

Question:Which salt will give basic solution on hydrolysis

$$KCN$$

$$KCl$$

$$N{H_4}Cl$$

$$C{H_3}COON{H_4}$$

## Questions 29 of 50

Question:Which of the following sulphides has the lowest solubility product

$$FeS$$

$$MnS$$

$$PbS$$

$$ZnS$$

## Questions 30 of 50

Question:Electrolytes when dissolved in water dissociate into their constituent ions. The degree of dissociation of an electrolyte increases with

Increasing concentration of the electrolyte

Decreasing concentration of the electrolyte

Decreasing temperature

Presence of a substance yielding a common ion

## Questions 31 of 50

Question:An electrolyte

Gives complex ions in solution

Dissolves in water to give ions

Is ionized in the solid state

Generates ions on passing electric current

## Questions 32 of 50

Question:Vant hoff factor of $$BaC{l_2}$$ of conc. $$0.01M$$ is 1.98. Percentage dissociation of $$BaC{l_2}$$ on this conc. Will be

49

69

89

98

100

## Questions 33 of 50

Question:In which of the following solutions, ions are present

Sucrose in water

Sulphur in $$C{S_2}$$

Caesium nitrate in water

Ethanol in water

## Questions 34 of 50

Question:The $$pH$$ of blood does not appreciably change by a small addition of an acid or a base because blood

Contains serum protein which acts as buffer

Contains iron as a part of the molecule

Can be easily coagulated

It is body fluid

## Questions 35 of 50

Question:The $$pH$$ of a $$0.001\,M\,NaOH$$ will be

3

2

11

12

## Questions 36 of 50

Question:The $$pH$$ of a $${10^{ - 10}}M\,NaOH$$ solution is nearest to

10

7

4

$$- 10$$

## Questions 37 of 50

Question:Which will have maximum $$pH$$

Distilled water

$$1\,M\,\,N{H_3}$$

$$1\,M\,\,NaOH$$

Water saturated by chlorine

## Questions 38 of 50

Question:When rain is accompained by a thunderstorm, the collected rain water will have a pH value

Slightly lower than that of rain water without thunderstorm

Slightly higher than that when the thunderstorm is not there

Uninfluenced by occurrence of thunderstorm

Which depends on the amount of dust in air

## Questions 39 of 50

Question:Which of the following is the buffer solution of strong acidic nature

$$HCOOH + HCO{O^ - }$$

$$C{H_3}COOH + C{H_3}CO{O^ - }$$

$${H_2}{C_2}{O_4} + {C_2}O_4^{2 - }$$

$${H_3}B{O_3} + BO_3^{3 - }$$

## Questions 40 of 50

Question:The pH of $$0.1\,M\,NaOH$$ is

11

12

13

14

## Questions 41 of 50

Question:pH of human blood is 7.4. Then $${H^ + }$$ concentration will be

$$4 \times {10^{ - 8}}$$

$$2 \times {10^{ - 8}}$$

$$4 \times {10^{ - 4}}$$

$$2 \times {10^{ - 4}}$$

## Questions 42 of 50

Question:The $$pH$$ of $${10^{ - 5}}$$M aqueous solution of $$NaOH$$is

5

7

9

11

## Questions 43 of 50

Question:The $$pH$$ of $${10^{ - 7}}N\,HCl$$ is

6

6.97

8

10

## Questions 44 of 50

Question:When $$100\,\,ml$$ of $$M/10\,\,NaOH$$ solution and $$50\,\,ml$$ of $$M/5\,\,HCl$$ solution are mixed, the $$pH$$ of resulting solution would be

0

7

Less than 7

More than 7

## Questions 45 of 50

Question:What is the $$pH$$of $$Ba{(OH)_2}$$if normality is 10

4

10

7

9

## Questions 46 of 50

Question:Pure water is kept in a vessel and it remains exposed to atmospheric $$C{O_2}$$which is absorbed, then its pH will be

Greater than 7

Less than 7

7

Depends on ionic product of water

## Questions 47 of 50

Question:The $$pH$$ of 0.001 molar solution of $$HCl$$ will be

0.001

3

2

6

## Questions 48 of 50

Question:The condition for minimum change in $$pH$$ for a buffer solution is

Conjugate acid or base is added

$$pH = p{K_a}$$

None of these

## Questions 49 of 50

Question:What will be hydrogen ion concentration in moles $$litr{e^{ - 1}}$$ of a solution, whose $$pH$$ is 4.58

$$2.63 \times {10^{ - 5}}$$

$$3.0 \times {10^{ - 5}}$$

$$4.68$$

None of these

## Questions 50 of 50

Question:Which of the following is a Lewis base

$$N{H_3}$$
$$BC{l_3}$$