# Ionic Equilibrium Test 8

Total Questions:50 Total Time: 75 Min

Remaining:

## Questions 1 of 50

Question:Which of the following is not a Lewis acid

$$B{F_3}$$

$$FeC{l_3}$$

$$Si{F_4}$$

$${C_2}{H_4}$$

## Questions 2 of 50

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

$$N{H_3}$$

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

$$NH_4^ +$$

$${N_3}^ -$$

## Questions 3 of 50

Question:$$HN{O_3}$$in liquid hydrogen fluoride behaves

As an acid

As a base

Neither as a base nor as an acid

As a base and as an acid

## Questions 4 of 50

Question:Aqueous solution of $$CuS{O_4}.5{H_2}O$$ changes blue litmus paper to red due to

Presence of $$C{u^{ + + }}$$ ions

Presence of $$S{O_4}^{ - - }$$ ions

Hydrolysis taking place

Reduction taking place

## Questions 5 of 50

Question:$$p{K_a}$$ of a weak acid is defined as

log$$_{10}{K_a}$$

$$\frac{1}{{lo{g_{10}}{K_a}}}$$

log $$_{10}\frac{1}{{{K_a}}}$$

log $$_{10}\frac{1}{{{K_a}}}$$

## Questions 6 of 50

Question:A salt $$'X'$$ is dissolved in water $$(pH = 7),$$ the resulting solution becomes alkaline in nature. The salt is made of

A strong acid and strong base

A strong acid and weak base

A weak acid and weak base

A weak acid and strong base

## Questions 7 of 50

Question:Which of the following behaves as both Lewis and Bronsted base

$$B{F_3}$$

$$C{l^ - }$$

$$CO$$

None of these

## Questions 8 of 50

Question:The conjugate acid of a strong base is a

Strong acid

Weak acid

Strong base

Weak base

## Questions 9 of 50

Question:Which one is Lewis acid

$$C{l^ - }$$

$$A{g^ + }$$

$${C_2}{H_5}OH$$

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

## Questions 10 of 50

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

$${H_3}P{O_4}$$

$${H_2}PO_4^ -$$

$$PO_4^{3 - }$$

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

## Questions 11 of 50

Question:Which among the following is strongest acid

H(ClO)O$$_{\rm{2}}$$

H(ClO)O$$_{\rm{3}}$$

H(ClO)O

H(ClO)

## Questions 12 of 50

Question:In the reaction $$2{H_2}O$$$$\leftrightarrow$$$${H_3}{O^ + } + O{H^ - }$$, water is

A weak base

A weak acid

Both a weak acid and a weak base

Neither an acid nor a base

## Questions 13 of 50

Question:According to Bronsted principle, an aqueous solution of $$HN{O_3}$$ will contain

$$NO_2^ -$$

$$NO_3^ -$$

$$NO_2^ +$$

$$N{O^ + }$$

## Questions 14 of 50

Question:Aqueous solution of an acid is characterised by the presence of

$${H^ + }$$ions

$$H_2^ +$$ions

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

$${H_4}{O^ + }$$ions

## Questions 15 of 50

Question:An aqueous solution of sodium carbonate is alkaline because sodium carbonate is a salt of

Weak acid and weak base

Strong acid and weak base

Weak acid and strong base

Strong acid and strong base

## Questions 16 of 50

Question:The acid that results when a base accepts a proton is called

Conjugate base of the acid

Conjugate protonated base

Lewis base

Conjugate acid of the base

None of these

## Questions 17 of 50

Question:The conjugate base of $$HCO_3^ -$$ is

$${H_2}C{O_3}$$

$$CO_3^{2 - }$$

$$C{O_2}$$

$${H_2}O$$

## Questions 18 of 50

Question:In the reaction $$N{H_3} + B{F_3}$$ $$\leftrightarrow$$ $$N{H_3} \to B{F_3},\,\,B{F_3}$$ is

Lewis acid

Lewis base

Neither Lewis acid nor Lewis base

Lewis acid and Lewis base both

## Questions 19 of 50

Question:For a weak acid, the incorrect statement is

Its dissociation constant is low

Its $$p{K_a}$$ is very low

It is partially dissociated

Solution of its sodium salt is alkaline in water

## Questions 20 of 50

Question:The solubility in water of a sparingly soluble salt $$A{B_2}$$ is $$1.0 \times {10^{ - 5}}mol\,{l^{ - 1}}$$. Its solubility product number will be

$$4 \times {10^{ - 15}}$$

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

$$1 \times {10^{ - 15}}$$

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

## Questions 21 of 50

Question:What will happen if $$CC{l_4}$$ is treated with $$AgN{O_3}$$

A white ppt. of $$AgCl$$ will form

$$N{O_2}$$ will be evolved

$$CC{l_4}$$ will dissolve in $$AgN{O_3}$$

Nothing will happen

## Questions 22 of 50

Question:Ionic product of water increases, if

Pressure is reduced

$${H^ + }$$is added

$$O{H^ - }$$is added

Temperature increases

## Questions 23 of 50

Question:If $$S$$ and $${K_{sp}}$$ are respectively solubility and solubility product of a sparingly soluble binary electrolyte, then

$$S = {K_{sp}}$$

$$S = K_{sp}^2$$

$$S = \sqrt {{K_{sp}}}$$

$$S = \frac{1}{2}{K_{sp}}$$

## Questions 24 of 50

Question:Which is a basic salt

$$PbS$$

$$PbC{O_3}$$

$$PbS{O_4}$$

$$2PbC{O_3}.Pb{(OH)_2}$$

## Questions 25 of 50

Question:Solubility of $$M{X_2}$$ type electrolyte is $$0.5 \times {10^{ - 4}}mole/litre$$. The value of $${K_{sp}}$$ of the electrolyte is

$$5 \times {10^{ - 13}}$$

$$25 \times {10^{ - 10}}$$

$$1.25 \times {10^{ - 13}}$$

$$5 \times {10^{12}}$$

## Questions 26 of 50

Question:The concentration of which ion is to be decreased, when $$N{H_3}$$ solution is added

$$O{H^ - }$$

$$NH_4^ +$$

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

$$O_2^ -$$

## Questions 27 of 50

Question:A monoprotic acid in 1.00 M solution is 0.01% ionised. The dissociation constant of this acid is

$$1 \times {10^{ - 8}}$$

$$1 \times {10^{ - 4}}$$

$$1 \times {10^{ - 6}}$$

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

## Questions 28 of 50

Question:The following equilibrium exists inaqueous solution, $$C{H_3}COOH$$$$\leftrightarrow$$$$C{H_3}CO{O^ - } + {H^ + }$$ if dil HCl is added, without change in temperature, the

Concentration of $$C{H_3}CO{O^ - }$$ will increase

Concentration of $$C{H_3}CO{O^ - }$$ will decrease

The equilibrium constant will increase

The equilibrium constant will decrease

## Questions 29 of 50

Question:pH value of a solution, whose hydronium ion concentration is $$6.2 \times {10^{ - 9}}mol/\,l,$$ is

6.21

7.21

7.75

8.21

## Questions 30 of 50

Question:pH of a solution is 9.5. The solution is

Neutral

Acidic

Basic

Amphoteric

## Questions 31 of 50

Question:The dissociation constant of an acid HA is $$1 \times {10^{ - 5}}$$. The $$pH$$ of 0.1 molar solution of the acid will be

Five

Four

Three

One

## Questions 32 of 50

Question:Assuming complete ionisation, the pH of $$0.1\,M\,HCl,$$ is 1. The molarity of $${H_2}S{O_4}$$ with the same pH is

0.1

0.2

0.05

2

## Questions 33 of 50

Question:The $$pH$$ of 0.05 M solution of dibasic acid is

$$+ 1$$

$$- 1$$

$$+ 2$$

$$- 2$$

## Questions 34 of 50

Question:A buffer solution contains $$6.4 \times {10^{ - 5}}$$ of acetic acid and $$0.1\,\,M$$ of sodium acetate. What will be its $$pH$$, if $$p{K_a}$$of acetic acid is 4.75

4

4.75

5

5.25

## Questions 35 of 50

Question:If the $$pH$$ of a solution is 2, its normality will be

2N

$${\textstyle{1 \over 2}}N$$

0.01 N

None of these

## Questions 36 of 50

Question:The buffer solution of 100 $$ml$$ having a $$pH$$ value 4 when added to 1 $$ml$$ dilute $$HCl$$, then the $$pH$$ of buffer solution

Converts to 7

Does not change

Converts to 2

Changes to 10

## Questions 37 of 50

Question:How many millilitres of $$6.0\,\,M$$hydrochloric acid should be used to prepare $$150\,\,ml$$ of a solution which is $$0.30\,\,M$$ in hydrogen ion

3

7.5

9.3

30

## Questions 38 of 50

Question:The pH of 0.1 M acetic acid is 3, the dissociation constant of acid will be

$$1.0 \times {10^{ - 4}}$$

$$1.0 \times {10^{ - 5}}$$

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

$$1.0 \times {10^{ - 8}}$$

## Questions 39 of 50

Question:What will be the $$pH$$ of a solution formed by mixing $$40\,\,ml$$ of $$0.10\,\,M\,\,HCl$$ with $$10\,\,ml$$ of $$0.45\,\,M\,\,NaOH$$

12

10

8

6

## Questions 40 of 50

Question:The $$pH$$ of a solution having $$[{H^ + }] = 10 \times {10^{ - 4}}\,\,moles/litre$$ will be

1

2

3

4

## Questions 41 of 50

Question:The $$pH$$of a solution is 2. If its $$pH$$ is to be raised to 4, then the $$[{H^ + }]$$ of the original solution has to be

Doubled

Halved

Increased hundred times

Decreased hundred times

## Questions 42 of 50

Question:Which of the following solutions cannot act as a buffer

$$Na{H_2}P{O_4} + {H_3}P{O_4}$$

$$C{H_3}COOH + C{H_3}COONa$$

$$HCl + N{H_4}Cl$$

$${H_3}P{O_4} + N{a_2}HP{O_4}$$

## Questions 43 of 50

Question:Which salt can be classified as an acid salt

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

$$BiOCl$$

$$Pb(OH)Cl$$

$$N{a_2}HP{O_4}$$

## Questions 44 of 50

Question:Given a 0.1M solution of each of the following. Which solution has the lowest $$pH$$

$$NaHS{O_4}$$

$$N{H_4}Cl$$

$$HCl$$

$$N{H_3}$$

## Questions 45 of 50

Question:A buffer solution with $$pH$$9 is to be prepared by mixing $$N{H_4}Cl$$ and $$N{H_4}OH$$. Calculate the number of moles of $$N{H_4}Cl$$ that should be added to one litre of $$1.0\,M\;N{H_4}OH.\,$$ $$[{K_b} = 1.8 \times {10^{ - 5}}]$$

3.4

2.6

1.5

1.8

## Questions 46 of 50

Question:The ionization constant of a certain weak acid is $${10^{ - 4}}$$. What should be the [salt] to [acid] ratio if we have to prepare a buffer with pH = 5 using this acid and one of the salts

$$1:10$$

$$10:1$$

$$5:4$$

$$4:5$$

## Questions 47 of 50

Question:Assuming complete dissociation, the $$pH$$ of a 0.01 M $$NaOH$$solution is equal to

2

14

12

0.01

## Questions 48 of 50

Question:50 $$ml$$ of $$2\,N$$acetic acid mixed with $$10\,ml$$ of $$1\,\,N$$sodium acetate solution will have an approximate $$pH$$ of

4

5

6

7

## Questions 49 of 50

Question:What will be the $$pH$$value of 0.05 M $$Ba{(OH)_2}$$solution

12

13

1

12.96

## Questions 50 of 50

Question:In a mixing of acetic acid and sodium acetate the ratio of concentration of the salts to the acid is increased ten times. Then the pH of the solution