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

Answers Choices:

\(B{F_3}\)

\(FeC{l_3}\)

\(Si{F_4}\)

\({C_2}{H_4}\)

Questions 2 of 50

Question:The conjugate base of \(N{H_2}^ - \)is

Answers Choices:

\(N{H_3}\)

\(N{H^{2 - }}\)

\(NH_4^ + \)

\({N_3}^ - \)

Questions 3 of 50

Question:\(HN{O_3}\)in liquid hydrogen fluoride behaves

Answers Choices:

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

Answers Choices:

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

Answers Choices:

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

Answers Choices:

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

Answers Choices:

\(B{F_3}\)

\(C{l^ - }\)

\(CO\)

None of these

Questions 8 of 50

Question:The conjugate acid of a strong base is a

Answers Choices:

Strong acid

Weak acid

Strong base

Weak base

Questions 9 of 50

Question:Which one is Lewis acid

Answers Choices:

\(C{l^ - }\)

\(A{g^ + }\)

\({C_2}{H_5}OH\)

\({S^{2 - }}\)

Questions 10 of 50

Question:The conjugate acid of \({H_2}PO_4^ - \) is

Answers Choices:

\({H_3}P{O_4}\)

\({H_2}PO_4^ - \)

\(PO_4^{3 - }\)

\({H_3}{O^ + }\)

Questions 11 of 50

Question:Which among the following is strongest acid

Answers Choices:

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

Answers Choices:

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

Answers Choices:

\(NO_2^ - \)

\(NO_3^ - \)

\(NO_2^ + \)

\(N{O^ + }\)

Questions 14 of 50

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

Answers Choices:

\({H^ + }\)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

Answers Choices:

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

Answers Choices:

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

Answers Choices:

\({H_2}C{O_3}\)

\(CO_3^{2 - }\)

\(C{O_2}\)

\({H_2}O\)

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

Answers Choices:

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

Answers Choices:

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

Answers Choices:

\(4 \times {10^{ - 15}}\)

\(4 \times {10^{ - 10}}\)

\(1 \times {10^{ - 15}}\)

\(1 \times {10^{ - 10}}\)

Questions 21 of 50

Question:What will happen if \(CC{l_4}\) is treated with \(AgN{O_3}\)

Answers Choices:

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

Answers Choices:

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

Answers Choices:

\(S = {K_{sp}}\)

\(S = K_{sp}^2\)

\(S = \sqrt {{K_{sp}}} \)

\(S = \frac{1}{2}{K_{sp}}\)

Questions 24 of 50

Question:Which is a basic salt

Answers Choices:

\(PbS\)

\(PbC{O_3}\)

\(PbS{O_4}\)

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

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

Answers Choices:

\(5 \times {10^{ - 13}}\)

\(25 \times {10^{ - 10}}\)

\(1.25 \times {10^{ - 13}}\)

\(5 \times {10^{12}}\)

Questions 26 of 50

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

Answers Choices:

\(O{H^ - }\)

\(NH_4^ + \)

\({H_3}{O^ + }\)

\(O_2^ - \)

Questions 27 of 50

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

Answers Choices:

\(1 \times {10^{ - 8}}\)

\(1 \times {10^{ - 4}}\)

\(1 \times {10^{ - 6}}\)

\({10^{ - 5}}\)

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

Answers Choices:

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

Answers Choices:

6.21

7.21

7.75

8.21

Questions 30 of 50

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

Answers Choices:

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

Answers Choices:

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

Answers Choices:

0.1

0.2

0.05

2

Questions 33 of 50

Question:The \(pH\) of 0.05 M solution of dibasic acid is

Answers Choices:

\( + 1\)

\( - 1\)

\( + 2\)

\( - 2\)

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

Answers Choices:

4

4.75

5

5.25

Questions 35 of 50

Question:If the \(pH\) of a solution is 2, its normality will be

Answers Choices:

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

Answers Choices:

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

Answers Choices:

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

Answers Choices:

\(1.0 \times {10^{ - 4}}\)

\(1.0 \times {10^{ - 5}}\)

\(1.0 \times {10^{ - 3}}\)

\(1.0 \times {10^{ - 8}}\)

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 \(0.45\,\,M\,\,NaOH\)

Answers Choices:

12

10

8

6

Questions 40 of 50

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

Answers Choices:

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

Answers Choices:

Doubled

Halved

Increased hundred times

Decreased hundred times

Questions 42 of 50

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

Answers Choices:

\(Na{H_2}P{O_4} + {H_3}P{O_4}\)

\(C{H_3}COOH + C{H_3}COONa\)

\(HCl + N{H_4}Cl\)

\({H_3}P{O_4} + N{a_2}HP{O_4}\)

Questions 43 of 50

Question:Which salt can be classified as an acid salt

Answers Choices:

\(N{a_2}S{O_4}\)

\(BiOCl\)

\(Pb(OH)Cl\)

\(N{a_2}HP{O_4}\)

Questions 44 of 50

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

Answers Choices:

\(NaHS{O_4}\)

\(N{H_4}Cl\)

\(HCl\)

\(N{H_3}\)

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 \(1.0\,M\;N{H_4}OH.\,\) \([{K_b} = 1.8 \times {10^{ - 5}}]\)

Answers Choices:

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

Answers Choices:

\(1:10\)

\(10:1\)

\(5:4\)

\(4:5\)

Questions 47 of 50

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

Answers Choices:

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

Answers Choices:

4

5

6

7

Questions 49 of 50

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

Answers Choices:

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

Answers Choices:

Increase by one

Decreases by one

Decrease ten fold

Increases ten fold