Question Bank for JEE Main & Advanced Chemistry Equilibrium / साम्यावस्था Topic Test - Ionic Equilibrium

1)

Silver ions are added to solution with \[[B{{r}^{-}}]=[C{{l}^{-}}]=[CO_{3}^{2-}]=[AsO_{4}^{3-}]=0.1\,M\]. Which compound will precipitate at lowest \[[A{{g}^{+}}]\]?

A)

\[AgBr({{K}_{sp}}=5\times {{10}^{-13}})\]

B)

\[AgCl({{K}_{sp}}=1.8\times {{10}^{-10}})\]

C)

\[A{{g}_{2}}C{{O}_{3}}({{K}_{sp}}=8\times {{10}^{-12}})\]

D)

\[A{{g}_{3}}As{{O}_{4}}({{K}_{sp}}={{10}^{-22}})\]

View Solution

2)

pH of 2M HCl solution at \[25{}^\circ \]

A)

Ph < 0

B)

0 < pH > 1

C)

0

D)

1

View Solution

3)

Taking \[Ba{{(OH)}_{2}}\] to be completely ionised. The pH of its 0.001 M solution is

A)

11.3

B)

2.7

C)

11

D)

3

View Solution

4)

The ionization constant of \[HCOOH\] is \[1.8\times {{10}^{-4}}\]. What is the percent ionization of a 0.001 M solution?

A)

66%

B)

42%

C)

34%

D)

58%

View Solution

5)

Which of the following statements is not correct?

A)

\[{{I}^{-}}\] is a weaker base than \[{{F}^{-}}\]

B)

\[H{{O}^{-}}\] is a stronger base than \[{{H}_{2}}{{N}^{-}}\]

C)

\[HON{{H}_{2}}\] is a weaker base than \[N{{H}_{3}}\]

D)

\[{{F}_{3}}{{C}^{-}}\] is a stronger base than \[C{{l}_{3}}{{C}^{-}}\]

View Solution

6)

The pH of solution, containing 0.1 N HCI and \[0.1\,N\,C{{H}_{3}}COOH\,({{K}_{a}}=2\times {{10}^{-5}})\] is

A)

1

B)

0.7

C)

3

D)

1.3

View Solution

7)

Equal volumes of two HCl solutions of \[pH=3\] and were mixed. What is the pH of the resulting solution?

A)

3.5

B)

4.0

C)

4.5

D)

3.3

View Solution

8)

Select the best indicator from the given table for titration of 20 mL of \[0.02\,M\,\,C{{H}_{3}}COOH\] with 0.02 M NaOH. Given \[p{{K}_{a}}\,(C{{H}_{3}}COOH)=4.74\]

	Indicator	pH Range
(I)	Bromothy mol blue	6.0-7.6
(II)	Thymolphthalein	9.3-11.05
(III)	Malachite green	11.4-13
(IV)	M-Cresol purple	7.4-9.0

A)

I

B)

II

C)

III

D)

IV

View Solution

9)

Of the following acids

I. Hypophosphorous acid

II. Orthophosphorous acid

III. Caro's acid

IV. Glycine

A)

I, II monobasic; III dibasic acid and IV amphoteric

B)

II monobasic; I, III dibasic acid and IV amphoteric

C)

I monobasic; II, III dibasic acid and IV amphoteric

D)

I, II, III dibasic acids and IV amphoteric

View Solution

10)

\[N{{H}_{4}}Cl\] is acidic, because:

A)

on hydrolysis, \[N{{H}_{4}}Cl\] gives weak base \[N{{H}_{4}}OH\] and strong acid \[HCl\]

B)

nitrogen donates a pair of electron

C)

it is a salt of weak acid and strong base

D)

on hydrolysis, \[N{{H}_{4}}Cl\] gives strong base and weak acid

View Solution

11)

pH of an aqueous solution of HCl is 5. if 1 c.c. of this solution is diluted to 1000 times. The pH will become

A)

8

B)

5

C)

6.9

D)

None

View Solution

12)

In which case change in pH is maximum?

A)

1 mL of pH = 2 is diluted to 100 mL

B)

0.01 mol of \[NaOH\] is added to 100 mL of 0.01 M \[NaOH\] solution

C)

100 mL of \[{{H}_{2}}O\] is added to 900 mL of \[{{10}^{-6}}\] M \[HCl\]

D)

100 mL of pH = 2 solution is mixed with 100 mL of pH = 12

View Solution

13)

Which relation is wrong

A)

\[{{10}^{-pH}}+{{10}^{-pOH}}={{10}^{-14}}\]

B)

\[pH\alpha \frac{1}{[{{H}^{+}}]}\]

C)

\[{{K}_{w}}\alpha \,T\]

D)

dissociation constant of water \[K=1.8\times {{10}^{-16}}\]

View Solution

14)

If acetic acid is 1.0% ionised in its decinormal solution, then pH of its seminormal solution will be

A)

3.4

B)

4.8

C)

1.6

D)

2.6

View Solution

15)

Which of the following species would be least likely to act as Lewis base?

A)

\[PC{{l}_{3}}\]

B)

\[C{{N}^{-}}\]

C)

\[SC{{l}_{2}}\]

D)

\[{{I}^{+}}\]

View Solution

16)

Which of the following cannot have a conjugate base?

A)

\[{{H}_{2}}PO_{2}^{-}\]

B)

\[HCO_{3}^{-}\]

C)

\[{{H}_{2}}{{O}_{2}}\]

D)

\[HSO_{4}^{-}\]

View Solution

17)

Choose the correct order of strength of following acids.

(i) \[C{{H}_{3}}C{{H}_{2}}C{{H}_{2}}COOH\]

(ii) \[~C{{H}_{3}}C{{H}_{2}}CH(Br)COOH\]

(iii) \[C{{H}_{3}}CH(Br)C{{H}_{2}}COOH\]

(IV) \[{{(C{{H}_{3}})}_{2}}CHCOOH\]

A)

I < II < III < IV

B)

IV < I < III < II

C)

IV < III < I < II

D)

II < I < III < IV

View Solution

18)

Match List I with List II and select the correct answer using the code given below the lists

List I	List II
[A] pH of 0.1 M HA \[(p{{K}_{a}}=5)\] and 0.01 M NaA	(p) 4
[B] pH of 0.1 M BOH \[(p{{K}_{b}}=6)\] and 0.1 M BCI	(q) 7
[C] pH of 0.1 M salt of HA \[(p{{K}_{a}}=5)\] and BOH \[(p{{K}_{b}}=7)\]	(r) 6
[D] pH of 500 litre of 0.2 M \[HN{{O}_{3}}\] and 500 litre 0.2 M NaOH	(s) 8

Codes:

A)

A\[\to \]p, B\[\to \]s, C\[\to \]r, D\[\to \]q

B)

A\[\to \]s, B\[\to \]p, C\[\to \]r, D\[\to \]q

C)

A\[\to \]p, B\[\to \]r, C\[\to \]s, D\[\to \]q

D)

A\[\to \]p, B\[\to \]s, C\[\to \]q, D\[\to \]r

View Solution

19)

A solution saturated in lime water has a pH of 12.4. Then the Ksp for \[Ca{{(OH)}_{2}}\] is:

A)

\[3.2\times {{10}^{-3}}\]

B)

\[7.8\times {{10}^{-6}}\]

C)

\[7.8\times {{10}^{-28}}\]

D)

\[3.2\times {{10}^{-4}}\]

View Solution

20)

Which will act as a buffer solution

A)

\[200\text{ }ml\text{ }N/10\text{ }NaOH\]\[+100\text{ }ml\text{ }N/20\text{ }HCl\]

B)

\[100\text{ }ml\text{ }0.1\text{ }N\text{ }NaOH\]\[+100\text{ }ml\text{ }0.1\text{ }N\text{ }HCl\]

C)

\[100\,\,ml\,\,0.1\,\,N\,NaOH\]\[+50\,\,ml\,\,0.2N\,C{{H}_{3}}OOH\]

D)

\[100\text{ }ml\text{ }0.1\text{ }N\text{ }NaOH\]\[+150\text{ }ml\text{ }0.1\text{ }N\text{ }HCN\]

View Solution

21)

100 mL of 1 M \[HCl\] is mixed with 50 mL of 2 M \[HCl\]. Hence, \[\left[ {{H}_{3}}{{O}^{+}} \right]\] is:

A)

1.00 M

B)

1.50 M

C)

1.33 M

D)

3.00 M

View Solution

22)

The solubility product of \[Mg{{(OH)}_{2}}\] is \[{{10}^{-14}}\]. The solubility of \[Mg{{(OH)}_{2}}\] in a buffer solution of \[pH=8\] is

A)

\[{{10}^{-8}}\]

B)

\[{{10}^{-6}}\]

C)

\[{{10}^{-2}}\]

D)

\[{{10}^{-4}}\]

View Solution

23)

At \[30{}^\circ C\] the solubility of \[A{{g}_{2}}C{{O}_{3}}\] \[({{K}_{SP}}=8\times {{10}^{-12}})\] would be greatest in one litre of:

A)

\[0.05M\,\,N{{a}_{2}}C{{O}_{3}}\]

B)

\[0.05M\,AgN{{O}_{3}}\]

C)

Pure water

D)

\[0.05M\,{{K}_{2}}C{{O}_{3}}\]

View Solution

24)

A mixture of weak acid is \[0.1\text{ }M\] in \[HCOOH\] \[({{K}_{a}}=1.8\times {{10}^{-4}})\] and \[0.1\text{ }M\] in \[HOCN\,\,({{K}_{a}}=3.1\times {{10}^{-4}})\] Hence, \[[{{H}_{3}}{{O}^{\oplus }}]\] is

A)

\[7.0\times {{10}^{-3}}M\]

B)

\[4.1\times {{10}^{-4}}M\]

C)

\[0.20M\]

D)

\[4.1\times {{10}^{-3}}M\]

View Solution

25)

The solubility of \[AgCl\] in water at \[25{}^\circ C\] is \[1.79\times {{10}^{-3}}g/L\]. The \[{{K}_{sp}}\] of \[AgCl\] at \[25{}^\circ C\] is

A)

\[1.68\times {{10}^{-12}}\]

B)

\[1.55\times {{10}^{-10}}\]

C)

\[12.4\times {{10}^{-8}}\]

D)

\[1.73\times {{10}^{-14}}\]

View Solution

26)

Solubility of \[PbC{{l}_{2}}\] in 0.5 M NaCl is \[{{S}_{1}}\] and that in 0.5 M \[Pb{{(N{{O}_{3}})}_{2}}\] is \[{{S}_{2}}\] then which of 5 the following is correct:

A)

\[\frac{{{S}_{1}}}{{{S}_{2}}}=1\]

B)

\[{{S}_{1}}-{{S}_{2}}>0\]

C)

\[{{S}_{1}}-{{S}_{2}}<0\]

D)

\[\frac{{{S}_{1}}}{{{S}_{2}}}>1\]

View Solution

27)

Arrange the following in increasing order of \[pH\,\,KN{{O}_{3}}(aq),\,C{{H}_{3}}COON(aq),\]\[N{{H}_{4}}Cl(aq),\,{{C}_{6}}{{H}_{5}}COON{{H}_{4}}(aq)\]

A)

\[C{{H}_{3}}COONa<{{C}_{6}}{{H}_{5}}COON{{H}_{4}}\]\[<N{{H}_{4}}Cl<KN{{O}_{3}}\]

B)

\[KN{{O}_{3}}<N{{H}_{4}}C<C{{H}_{3}}COONa\]\[<{{C}_{6}}{{H}_{5}}COONa\]

C)

\[N{{H}_{4}}Cl<KN{{O}_{3}}<C{{H}_{3}}COONa\]\[<{{C}_{6}}{{H}_{5}}COON{{H}_{4}}\]

D)

\[N{{H}_{4}}Cl<KN{{O}_{3}}<{{C}_{6}}{{H}_{5}}COON{{H}_{4}}\]\[<C{{H}_{3}}COONa\]

View Solution

28)

Blue litmus turns red in which of the following mixture of acid and base?

A)

\[100\,mL\] of \[1\times {{10}^{-2}}M\,{{H}_{2}}S{{O}_{4}}\]\[+\,100\,mL\] of \[1\times {{10}^{-2}}M\,Ca{{\left( OH \right)}_{2}}\]

B)

\[100\,mL\] of \[1\times {{10}^{-2}}M\,HCl\]+ \[100\,mL\] of \[1\times {{10}^{-2}}M\,Ba{{\left( OH \right)}_{2}}\]

C)

\[100\,mL\] of \[1\times {{10}^{-2}}M\,{{H}_{2}}S{{O}_{4}}\]\[+\,10\,mL\] of \[1\times {{10}^{-2}}M\,NaOH\]

D)

\[100\,mL\] of \[1\times {{10}^{-2}}M\,HCl\]\[+\,100\,mL\] of \[1\times {{10}^{-2}}M\,NaOH\]

View Solution

29)

The degree of ionization of a compound depends on

A)

size of solute

B)

nature of solute

C)

nature of vessel

D)

quantity of electricity passed

View Solution

30)

What is the minimum pH when \[Fe{{(OH)}_{3}},\] starts precipitating from a solution containing \[0.1M\text{ }FeC{{l}_{3}}\]? \[{{k}_{sp}}\] of \[Fe{{(OH)}_{3}}=8\times {{10}^{-13}}{{M}^{3}}(\log \text{ }2\text{ }=\text{ }0.3)\]

A)

3.7

B)

5.7

C)

10.3

D)

8.3

View Solution

31)

The number of moles of \[N{{H}_{3}}\] that must be added to 1 L of 0.1 M \[AgN{{O}_{3}}\] to reduce \[A{{g}^{+}}\] concentration to \[2\times {{10}^{-7}}M\] are Given, \[{{K}_{dis}}{{[Ag{{(N{{H}_{3}})}_{2}}]}^{+}}=6.8\times {{10}^{-8}}\]

A)

0.184 M

B)

0.384 M

C)

0.293 M

D)

0.0539 M

View Solution

32)

10 mL, of a strong acid solution of \[pH=2.000\] are mixed with 990 mL of another strong acid solution of \[pH=4.000\]. The pH of the resulting solution will be:

A)

4.002

B)

4.000

C)

4.200

D)

3.7

View Solution

33)

Conjugate base of \[NH_{4}^{+}\] is

A)

\[N{{H}_{3}}\]

B)

\[NH_{2}^{-}\]

C)

\[N{{H}_{4}}OH\]

D)

\[C{{l}^{-}}\]

View Solution

34)

The correct order of acidic strength is:

A)

\[C{{l}_{2}}{{O}_{7}}>S{{O}_{2}}>{{P}_{4}}{{O}_{10}}\]

B)

\[C{{O}_{2}}>{{N}_{2}}{{O}_{5}}>S{{O}_{3}}\]

C)

\[N{{a}_{2}}O>MgO>A{{l}_{2}}{{O}_{3}}\]

D)

\[{{K}_{2}}O>CaO>MgO\]

View Solution

35)

Match list I (Solutions of salts of...) with list II (pH of the solution is given by) and select the correct answer using the codes given below the lists:

List I	List II
Weak acid and strong base	(p) \[\frac{1}{2}p{{K}_{w}}\]
Strong acid and weak base	(q) \[\frac{1}{2}(p{{K}_{w}}-p{{K}_{b}}+p{{K}_{a}})\]
Weak acid and weak base	(r) \[\frac{1}{2}(p{{K}_{w}}-p{{K}_{b}}-\log \,\,C)\]
Strong acid and strong base	(s) \[\frac{1}{2}(p{{K}_{w}}+p{{K}_{a}}+\log \,\,C)\]

Codes:

A)

A\[\to \]p, B\[\to \]q, C\[\to \]r, D\[\to \]s

B)

A\[\to \]s, B\[\to \]r, C\[\to \]q, D\[\to \]p

C)

A\[\to \]s, B\[\to \]r, C\[\to \]p, D\[\to \]q

D)

A\[\to \]r, B\[\to \]s, C\[\to \]q, D\[\to \]p

View Solution

JEE Main & Advanced Chemistry Equilibrium / साम्यावस्था Question Bank

done Topic Test - Ionic Equilibrium Total Questions - 35

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Topic Test - Ionic Equilibrium Total Questions - 35