# Ionic Equilibrium Test 1

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:A white substance having alkaline nature in solution is

$$NaN{O_3}$$

$$N{H_4}Cl$$

$$N{a_2}C{O_3}$$

$$F{e_2}{O_3}$$

## Questions 2 of 50

Question:Which of the following can act both as Bronsted acid and Bronsted base

$$C{l^ - }$$

$$HCO_3^ -$$

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

$$O{H^ - }$$

## Questions 3 of 50

Question:In the equilibrium $$C{H_3}COOH + HF$$$$\leftrightarrow$$ $$C{H_3}COO{H_2}^ + + {F^ - }$$

$${F^ - }$$is the conjugate acid of $$C{H_3}COOH$$

$${F^ - }$$is the conjugate base of $$HF$$

$$C{H_3}COOH$$ is the conjugate acid of $$C{H_3}COO{H_2}^ +$$

$$C{H_3}COO{H_2}^ +$$ is the conjugate base of $$C{H_3}COOH$$

## Questions 4 of 50

Question:The compound that is not a Lewis acid is

$$HSO_4^ -$$

$$AlC{l_3}$$

$$BeC{l_2}$$

$$N{H_3}$$

## Questions 5 of 50

Question:$${H^ + }$$ is a

Lewis acid

Lewis base

Bronsted-Lowry base

None of the above

## Questions 6 of 50

Question:Dissociation of $${H_3}P{O_4}$$takes place in following steps

1

2

3

4

## Questions 7 of 50

Question:$$100\,\,ml$$of $$0.2\,\,M\,\,{H_2}S{O_4}$$ is added to $$100\,\,ml$$ of $$0.2\,\,M\,\,NaOH.$$ The resulting solution will be

Acidic

Basic

Neutral

Slightly basic

## Questions 8 of 50

Question:$${H_3}B{O_3}$$ is

Monobasic and weak Lewis acid

Monobasic and weak Bronsted acid

Monobasic and strong Lewis acid

Tribasic and weak Bronsted acid

## Questions 9 of 50

Question:(i) A strong acid has a weak conjugate base (ii) An acid is an electron pair acceptor. The above statements (i) and (ii)

Correct

Wrong

(i) Correct and (ii) Wrong

(i) Wrong and (ii) Correct

## Questions 10 of 50

Question:The pH is less than 7, of the solution of

$$FeC{l_3}$$

$$NaCN$$

$$NaOH$$

$$NaCl$$

## Questions 11 of 50

Question:What is the conjugate base of $$O{H^ - }$$

$${O_2}$$

$${H_2}O$$

$${O^ - }$$

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

## Questions 12 of 50

Question:Which of the following is a Lewis base

$$C{H_4}$$

$${C_2}{H_5}OH$$

Acetone

Secondary amine

## Questions 13 of 50

Question:Conjugate base of $$N{H_3}$$ is

$$NH_4^ \oplus$$

$$NH_2^ \oplus$$

$$NH_2^\Theta$$

$${N_2}$$

## Questions 14 of 50

Question:Which of the following species is an acid and also a conjugate base of another acid

$$HSO_4^ -$$

$${H_2}S{O_4}$$

$$O{H^ - }$$

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

## Questions 15 of 50

Question:Among the following, the weakest base is

$${H^ - }$$

$$CH_3^ -$$

$$C{H_3}{O^ - }$$

$$C{l^ - }$$

## Questions 16 of 50

Question:Which of the following is not lewis base

$$N{H_3}$$

$$P{H_3}$$

$${(C{H_3})_3}N$$

$$H{N_3}$$

## Questions 17 of 50

Question:Neutralization of an acid with a base invariably results in the production of

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

$$O{H^ - }$$

$${H_2}O$$

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

## Questions 18 of 50

Question:The conjugate acid of $$HPO_4^{2 - }$$is

$${H_2}PO_4^ -$$

$$PO_4^{3 - }$$

$${H_3}P{O_4}$$

$${H_3}P{O_3}$$

## Questions 19 of 50

Question:The indicator used in the titration of sodium carbonate with sulphuric acid is

Phenolphthalein

Methyl orange

Potassium ferrocynide

Potassium ferricynide

## Questions 20 of 50

Question:According to Bronsted law, water is a/an

Base

Acid

Acid and base both

Salt

## Questions 21 of 50

Question:The conjugate base of $${H_2}PO_4^ -$$ is

$${H_3}P{O_4}$$

$${P_2}{O_5}$$

$$PO_4^{3 - }$$

$$HPO_4^{2 - }$$

## Questions 22 of 50

Question:Conjugate base of $$HSO_4^ -$$ is

$$SO_4^{2 - }$$

$${H_2}S{O_4}$$

$${H_3}SO_4^ +$$

None of these

## Questions 23 of 50

Question:Solubility product of a sulphide MS is $$3 \times {10^{ - 25}}$$and that of another sulphide NS is $$4 \times {10^{ - 40}}$$. In ammoniacal solution

Only NS gets precipitated

Only MS gets precipitated

No sulphide precipitates

Both sulphides precipitate

## Questions 24 of 50

Question:Which of the following salts when dissolved in water will get hydrolysed

$$NaCl$$

$$N{H_4}Cl$$

$$KCl$$

$$N{a_2}S{O_4}$$

## Questions 25 of 50

Question:Solubility product of $$BaC{l_2}$$ is $$4 \times {10^{ - 9}}$$. Its solubility in moles/litre would be

$$1 \times {10^{ - 3}}$$

$$1 \times {10^{ - 9}}$$

$$4 \times {10^{ - 27}}$$

$$1 \times {10^{ - 27}}$$

## Questions 26 of 50

Question:Which hydroxide will have lowest value of solubility product at normal temperature $$({25^o}C)$$

$$Mg\,{(OH)_2}$$

$$Ca\,{(OH)_2}$$

$$Ba\,{(OH)_2}$$

$$Be\,{(OH)_2}$$

## Questions 27 of 50

Question:The solubility of $$AgI$$ in $$NaI$$ solution is less than that in pure water because

AgI forms complex with NaI

Of common ion effect

Solubility product of AgI is less than that of NaI

The temperature of the solution decreases

## Questions 28 of 50

Question:The solubility product of $$BaS{O_4}$$ is $$1.5 \times {10^{ - 9}}.$$ The precipitation in a 0.01 $$M\,\,B{a^{2 + }}$$solution will start, on adding $${H_2}S{O_4}$$ of concentration

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

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

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

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

## Questions 29 of 50

Question:On passing $${H_2}S$$ gas through a highly acidic solution containing $$C{d^{2 + }}$$ions, $$CdS$$is not precipitated because

Of common ion effect

The solubility of $$CdS$$is low

$$C{d^{2 + }}$$ions do not form complex with $${H_2}S$$

The solubility product of $$CdS$$ is low

## Questions 30 of 50

Question:Which of the following will occur if a 0.1 M solution of a weak acid is diluted to $$0.01\,M$$ at constant temperature

$$[{H^ + }]$$ will decrease to 0.01 M

$$pH$$ will decrease

Percentage ionization will increase

$${K_a}$$ will increase

## Questions 31 of 50

Question:The precipitate of $$Ca{F_2}$$$$({K_{sp}} = 1.7 \times {10^{ - 10}})$$ is obtained when equal volumes of the following are mixed

$${10^{ - 4}}M\,C{a^{2 + }} + {10^{ - 4}}M\,{F^ - }$$

$${10^{ - 2}}M\,C{a^{2 + }} + {10^{ - 3}}M\,{F^ - }$$

Both 1,2

None of these

## Questions 32 of 50

Question:In the reaction: $${H_2}S$$ $$\leftrightarrow$$ $$2{H^ + } + {S^{ - - }}$$, when $$N{H_4}OH$$ is added, then

$${S^{ - - }}$$ is precipitate

No action takes places

Concentration of $${S^{ - - }}$$ decreases

Concentration of $${S^{ - - }}$$ increases

## Questions 33 of 50

Question:What is the solubility of calcium fluoride in a saturated solution, if its solubility product is $$3.2 \times {10^{ - 11}}$$

$$2.0 \times {10^{ - 4}}\,mole/litre$$

$$12.0 \times {10^{ - 3}}\,mole/litre$$

$$0.2 \times {10^{ - 4}}\,mole/litre$$

$$2 \times {10^{ - 3}}\,mole/litre$$

## Questions 34 of 50

Question:The following equilibrium exists in an aqueous solution of hydrogen sulphide : $${H_2}S$$ $$\leftrightarrow$$ $${H^ + } + H{S^ - }$$If dilute $$HCl$$ is added to an aqueous solution of $${H_2}S$$ without any change in temperature

The equilibrium constant will change

The concentration of $$H{S^ - }$$will increase

The concentration of undissociated $${H_2}S$$ will decrease

The concentration of $$H{S^ - }$$will decrease

## Questions 35 of 50

Question:The concentration of KI and KCl in certain solution containing both is 0.001M each. If 20 ml of this solution is added to 20 ml of a saturated solution of AgI in water? What will happen

AgCl will be precipitated

AgI will be precipitated

Both AgCl and AgI will be precipitated

There will be no precipitated

## Questions 36 of 50

Question:Theory of ionization was given by

Rutherford

Graham

Arrhenius

## Questions 37 of 50

Question:Degree of dissociation of $$0.1\,N\,\,C{H_3}COOH$$ is (Dissociation constant $$= 1 \times {10^{ - 5}}$$)

$${10^{ - 5}}$$

$${10^{ - 4}}$$

$${10^{ - 3}}$$

$${10^{ - 2}}$$

## Questions 38 of 50

Question:pH of a $${10^{ - 3}}M$$ solution of hydrochloric acid will be

1.3

2

3

4.5

## Questions 39 of 50

Question:What is the correct relationship between the $$pHs$$ of isomolar solutions of sodium oxide $$(p{H_1})$$, sodium sulphide $$(p{H_2}),$$ sodium selenide $$(p{H_3})$$ and sodium telluride $$(p{H_4})$$?

$$p{H_1} > p{H_2} = p{H_3} > p{H_4}$$

$$p{H_1} < p{H_2} < p{H_3} < p{H_4}$$

$$p{H_1} < p{H_2} < p{H_3} = p{H_4}$$

$$p{H_1} > p{H_2} > p{H_3} > p{H_4}$$

## Questions 40 of 50

Question:0.02 M monobasic acid dissociates 2% hence, $$pH$$ of the solution is

0.3979

1.3979

1.699

3.3979

## Questions 41 of 50

Question:A solution of $$MgC{l_2}$$ in water has pH

< 7

> 7

7

14.2

## Questions 42 of 50

Question:An acidic buffer solution can be prepared by mixing solution of

Ammonium acetate and acetic acid

Ammonium chloride and hydrochloric acid

Sulphuric acid and sodium sulphate

Acetic acid and sulphuric acid

$$NaCl$$ and $$NaOH$$

## Questions 43 of 50

Question:A certain buffer solution contains equal concentration of $$3.9 \times {10^{ - 5}}$$ and $$HX.$$ The $${K_b}$$ for $${H^ - }$$ is $${10^{ - 10}}.$$ The $$pH$$of the buffer is

4

7

10

14

## Questions 44 of 50

Question:When an acid or alkali is mixed with buffer solution, then $$pH$$of buffer solution

Not changes

Changes slightly

Increases

Decreases

## Questions 45 of 50

Question:When $$pH$$ of a solution decreases, its hydrogen ion concentration

Decreases

Increases

Rapidly increases

Remains always constant

## Questions 46 of 50

Question:The hydrogen ion concentration in a given solution is $$6 \times {10^{ - 4}}.$$ Its $$pH$$ will be

6

4

3.22

2

## Questions 47 of 50

Question:If $$pH$$of $$A,\,\,B,\,\,C$$and $$D$$are 9.5, 2.5, 3.5 and 5.5 respectively, then strongest acid is

A

C

D

B

## Questions 48 of 50

Question:The concentration of hydrogen ion in water is

8

$$1 \times {10^{ - 7}}$$

7

$$1/7$$

## Questions 49 of 50

Question:$$pH$$ of blood is maintained constant by mechanism of

Common ion effect

Buffer

Solubility

All of these

## Questions 50 of 50

Question:Assuming complete dissociation, which of the following aqueous solutions will have the same $$pH$$value

$$N{H_3}$$ of $$0.01\,\,M\,\,HCl$$
$$_{10}\frac{1}{{{K_a}}}$$ of $$0.01\,\,M\,\,{H_2}S{O_4}$$
$$50\,\,ml$$ of $$_{10}\frac{1}{{{K_a}}}$$
Mixture of 50 $$ml$$ of $$0.02\,\,M\,\,{H_2}S{O_4}$$ and $$50\,\,ml$$ of $$0.02\,\,M\,\,NaOH$$