JEE Main Ionic Equilibrium Practice Questions With Solutions

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JEE Main Chemistry Ionic Equilibrium Practice Questions

Question 1.

For a sparingly soluble salt ${AB}_{2}$ , the equilibrium concentrations of $A^{2 +}$ ions and $B^{-}$ ions are $1.2 \times 10^{- 4} M$ and $0.24 \times 10^{- 3} M$ , respectively. The solubility product of ${AB}_{2}$ is :

0.069 \times 10^{- 12}

0.276 \times 10^{- 12}

6.91 \times 10^{- 12}

27.65 \times 10^{- 12}

Question 2.

Given below are two statements :

Statement (I) : A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities

Statement (II) : Blood is naturally occurring buffer solution whose $pH$ is maintained by $H_{2} {CO}_{3} / {HCO}_{3}^{⊖}$ concentrations.

In the light of the above statements, choose the correct answer from the options given below :

Both Statement I and Statement II are false

Both Statement I and Statement II are true

Statement I is false but Statement II is true

Statement I is true but Statement II is false

Question 3.

The equilibrium ${Cr}_{2} O_{7}^{2 -} ⇌ 2 {CrO}_{4}^{2 -}$ is shifted to the right in :

a weakly acidic medium

a basic medium

a neutral medium

an acidic medium

Question 4.

Solubility of calcium phosphate (molecular mass, M) in water is

W_{g}

per

100 mL

25^{\circ} C

. Its solubility product at

25^{\circ} C

will be approximately.

10^{7} {(\frac{W}{M})}^{3}

10^{3} {(\frac{W}{M})}^{5}

10^{7} {(\frac{W}{M})}^{5}

10^{5} {(\frac{W}{M})}^{5}

Question 5.

Given below are two statements :

Statement (I) : Aqueous solution of ammonium carbonate is basic.

Statement (II) : Acidic/basic nature of salt solution of a salt of weak acid and weak base depends on $K_{a}$ and $K_{b}$ value of acid and the base forming it.

In the light of the above statements, choose the most appropriate answer from the options given below :

Both Statement I and Statement II are correct

Statement I is correct but Statement II is incorrect

Both Statement I and Statement II are incorrect

Statement I is incorrect but Statement II is correct

Question 6.

Which of the following statement(s) is/are correct?

(A) The

pH

1 \times 10^{- 8} M HCl

solution is 8 .

(B) The conjugate base of

H_{2} {PO}_{4}^{-}

{HPO}_{4}^{2 -}

.

(C)

K_{w}

increases with increase in temperature.

(D) When a solution of a weak monoprotic acid is titrated against a strong base at half neutralisation point,

pH = \frac{1}{2} {pK}_{a}

Choose the correct answer from the options given below:

(A), (B), (C)

(B), (C)

(B), (C), (D)

(A), (D)

Question 7.

$25 mL$ of silver nitrate solution (1M) is added dropwise to $25 mL$ of potassium iodide $(1.05 M)$ solution. The ion(s) present in very small quantity in the solution is/are :

I^{-}

only

K^{+}

only

{Ag}^{+}

and

I^{-}

both

{NO}_{3}^{-}

only

Question 8.

The incorrect statement for the use of indicators in acid-base titration is :

Phenolphthalein is a suitable indicator for a weak acid vs strong base titration.

Methyl orange may be used for a weak acid vs weak base titration.

Methyl orange is a suitable indicator for a strong acid vs weak base titration.

Phenolphthalein may be used for a strong acid vs strong base titration.

Question 9.

When the hydrogen ion concentration [H $^{+}$ ] changes by a factor of 1000, the value of pH of the solution __________

decreases by 2 units

increases by 2 units

decreases by 3 units

increases by 1000 units

Question 10.

$200 mL$ of $0.01 M HCl$ is mixed with $400 mL$ of $0.01 M H_{2} {SO}_{4}$ . The $pH$ of the mixture is _________.

Given: $\log 2 = 0.30, \log 3 = 0.48, \log 5 = 0.70, \log 7 = 0.84, \log 11 = 1.04$

1.14

1.78

2.34

3.02

Question 1.

Given below are two statements : One is labelled as Assertion A and the other is labelled as Reason R

Assertion A : Permanganate titrations are not performed in presence of hydrochloric acid.

Reason R : Chlorine is formed as a consequence of oxidation of hydrochloric acid.

In the light of the above statements, choose the correct answer from the options given below

Both

A

and

R

are true and

R

is the correct explanation of

A

Both

A

and

R

are true but

R

is NOT the correct explanation of

A

A

is true but

R

is false

A

is false but

R

is true

Question 2.

The plot of $pH$ -metric titration of weak base ${NH}_{4} OH$ vs strong acid HCl looks like :

JEE Main 2022 (Online) 27th July Evening Shift Chemistry - Ionic Equilibrium Question 29 English Option 1

JEE Main 2022 (Online) 27th July Evening Shift Chemistry - Ionic Equilibrium Question 29 English Option 2

JEE Main 2022 (Online) 27th July Evening Shift Chemistry - Ionic Equilibrium Question 29 English Option 3

JEE Main 2022 (Online) 27th July Evening Shift Chemistry - Ionic Equilibrium Question 29 English Option 4

Question 3.

Class XII students were asked to prepare one litre of buffer solution of $pH 8.26$ by their Chemistry teacher: The amount of ammonium chloride to be dissolved by the student in $0.2 M$ ammonia solution to make one litre of the buffer is :

(Given: ${pK}_{b} ({NH}_{3}) = 4.74$

Molar mass of ${NH}_{3} = 17 g {mol}^{- 1}$

Molar mass of ${NH}_{4} Cl = 53.5 g {mol}^{- 1}$ )

53.5 g

72.3 g

107.0 g

126.0 g

Question 4.

$K_{a_{1}}$ , $K_{a_{2}}$ and $K_{a_{3}}$ are the respective ionization constants for the following reactions (a), (b) and (c).

(a) $H_{2} C_{2} O_{4} \vec{\leftarrow} H^{+} + H C_{2} O_{4}^{-}$

(b) $H C_{2} O_{4}^{-} \vec{\leftarrow} H^{+} + C_{2} O_{4}^{2 -}$

The relationship between $K_{a_{1}}$ , $K_{a_{2}}$ and $K_{a_{3}}$ is given as :

K_{a_{3}}

=

K_{a_{1}}

+

K_{a_{2}}

K_{a_{3}}

=

K_{a_{1}}

-

K_{a_{2}}

K_{a_{3}}

=

K_{a_{1}}

/

K_{a_{2}}

K_{a_{3}}

=

K_{a_{1}}

\times

K_{a_{2}}

Question 5.

$20 mL$ of $0.1 M {NH}_{4} OH$ is mixed with $40 mL$ of $0.05 M HCl$ . The $pH$ of the mixture is nearest to :

(Given : $K_{b} ({NH}_{4} OH) = 1 \times 10^{- 5}, \log 2 = 0.30, \log 3 = 0.48, \log 5 = 0.69, \log 7 = 0.84, \log 11 = 1.04)$

3.2

4.2

5.2

6.2

Question 6.

The solubility of AgCl will be maximum in which of the following?

0.01 M KCl

0.01 M HCl

0.01 M AgNO₃

Deionised water

Question 7.

A student needs to prepare a buffer solution of propanoic acid and its sodium salt with pH 4. The ratio of $\frac{[C H_{3} C H_{2} C O O^{-}]}{[C H_{3} C H_{2} C O O H]}$ required to make buffer is ___________.

Given : $K_{a} (C H_{3} C H_{2} C O O H) = 1.3 \times 10^{- 5}$

0.03

0.13

0.23

0.33

Question 8.

The K_sp for bismuth sulphide (Bi₂S₃) is 1.08 $\times$ 10^{$-$ 73}. The solubility of Bi₂S₃ in mol L^{$-$ 1} at 298 K is :

1.0

\times

10^{$-$ 15}

2.7

\times

10^{$-$ 12}

3.2

\times

10^{$-$ 10}

4.2

\times

10^{$-$ 8}

Question 9.

Given below are two statements one is labelled as Assertion A and the other is labelled as Reason R :

Assertion A : The amphoteric nature of water is explained by using Lewis acid/base concept.

Reason R : Water acts as an acid with NH₃ and as a base with H₂S.

In the light of the above statements choose the correct answer from the options given below :

Both A and R are true and R is the correct explanation of A.

Both A and R are true but R is NOT the correct explanation of A.

A is true but R is false.

A is false but R is true.

Question 10.

Given below are two statements.

Statement I : In the titration between strong acid and weak base methyl orange is suitable as an indicator.

Statement II : For titration of acetic acid with NaOH phenolphthalein is not a suitable indicator.

In the light of the above statements, choose the most appropriate answer from the options given below :

Statement I is false but Statement II is true

Statement I is true but Statement II is false

Both Statement I and Statement II are true

Both Statement I and Statement II are false

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JEE Main Ionic Equilibrium Practice Questions With Solutions

JEE Main Chemistry Ionic Equilibrium Practice Questions

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

Question 10.

Question 1.

Question 2.

Question 3.

Question 4.

Question 5.

Question 6.

Question 7.

Question 8.

Question 9.

Question 10.

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