QBManager

Ionic Equilibrium

229663 ${NH}_{4} Cl$ is acidic due to

1 Cationic hydrolysis

2 Anionic hydrolysis

3 Its ionic nature

4

pH > 7

Explanation:

: ${NH}_{4} Cl$ is a salt of strong acid $HCl$ and weak base ${NH}_{4} OH$ .
Hydrolysis:-
$\begin{aligned} {NH}_{4} Cl + H_{2} O ◻ {NH}_{4} OH + HCl \\ {NH}_{4}^{+} + {Cl}^{-} + H_{2} O ◻ {NH}_{4} OH + H^{+} + {Cl}^{-} \\ {NH}_{4}^{+} (aq) + H_{2} O (l) ◻ {NH}_{4} OH (aq) + H^{+} (aq) \end{aligned}$
Only the cation will undergo hydrolysis and the solution will be acidic in nature due to $H^{+}$ formation. So here the cation is responsible for the acidic nature of the solution.

MHT CET-2010

Ionic Equilibrium

229666 If $20 mL$ of an acidic solution of $pH = 3$ is diluted to $100 mL$ , the $H^{+}$ ion concentration will be

1

1 \times 10^{- 3} M

2

2 \times 10^{- 3} M

3

2 \times 10^{- 4} M

4

0.02 \times 10^{- 4} M

Explanation:

: Given that -
$\begin{aligned} pH = 3 \\ V_{1} = 20 ml V_{2} = 100 ml \\ H^{+} = ? \\ H^{+} = 1 \times 10^{- 3} m = 1 \times 10^{- 3} N \\ N_{1} V_{1} = N_{2} V_{2} \\ 1 \times 10^{- 3} \times 20 = N_{2} \times 100 \\ N_{2} = 2 \times 10^{- 4} \\ [H^{+}] = 2 \times 10^{- 4} M \end{aligned}$

MHT CET-2009

Ionic Equilibrium

229668 Which one of the following species acts as both Bronsted acid and base?

1

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

2

{HPO}_{3}^{2 -}

3

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

4 All of these

Explanation:

: ${HPO}_{4}^{2 -}$ act as both Bronsted acid and bronsted base.
$\begin{array}{ll} {HPO}_{4}^{2 -} + H_{2} O ◻ & H_{2} {PO}_{4}^{-} + {OH}^{-} \\ {HPO}_{4}^{2 -} + H_{2} O ◻ & {PO}_{4}^{3 -} + H_{3} O^{+} \end{array}$
$H_{2} {PO}_{2}^{-}$ is conjugate base of $H_{3} {PO}_{2}$ (a monobasic acid) and does not give $H^{+}$ .
${HPO}_{3}^{2 -}$ is a conjugate base of $H_{2} {PO}_{3}^{-}$ and does not ionize further.
$H_{3} {PO}_{3}$ is a dibasic acid.

UPTU/UPSEE-2015

Ionic Equilibrium

229670 Which of the following is an amphoteric oxide?

1

{SO}_{3}

2

Mg

3

{Al}_{2} O_{3}

4

P_{4} O_{10}

МНТ СЕТ -2007

Explanation:

:
Amphoteric
- These are the oxides that can react with both acids and as well as bases to form salt and water.
- These possess both acidic and basic properties.
- ${Al}_{2} O_{3}, {SiO}_{2}$ is an example of Amphoteric oxide
- ${Al}_{2} O_{3} + 2 NaOH$ (Base) $\to 2 {NaAlO}_{2} + H_{2} O$
- ${Al}_{2} O_{3} + 6 HCl$ (acid) $\to 2 {AlCl}_{3} + 3 H_{2} O$

Ionic Equilibrium

229663 ${NH}_{4} Cl$ is acidic due to

1 Cationic hydrolysis

2 Anionic hydrolysis

3 Its ionic nature

4

pH > 7

Explanation:

: ${NH}_{4} Cl$ is a salt of strong acid $HCl$ and weak base ${NH}_{4} OH$ .
Hydrolysis:-
$\begin{aligned} {NH}_{4} Cl + H_{2} O ◻ {NH}_{4} OH + HCl \\ {NH}_{4}^{+} + {Cl}^{-} + H_{2} O ◻ {NH}_{4} OH + H^{+} + {Cl}^{-} \\ {NH}_{4}^{+} (aq) + H_{2} O (l) ◻ {NH}_{4} OH (aq) + H^{+} (aq) \end{aligned}$
Only the cation will undergo hydrolysis and the solution will be acidic in nature due to $H^{+}$ formation. So here the cation is responsible for the acidic nature of the solution.

MHT CET-2010

Ionic Equilibrium

229666 If $20 mL$ of an acidic solution of $pH = 3$ is diluted to $100 mL$ , the $H^{+}$ ion concentration will be

1

1 \times 10^{- 3} M

2

2 \times 10^{- 3} M

3

2 \times 10^{- 4} M

4

0.02 \times 10^{- 4} M

Explanation:

: Given that -
$\begin{aligned} pH = 3 \\ V_{1} = 20 ml V_{2} = 100 ml \\ H^{+} = ? \\ H^{+} = 1 \times 10^{- 3} m = 1 \times 10^{- 3} N \\ N_{1} V_{1} = N_{2} V_{2} \\ 1 \times 10^{- 3} \times 20 = N_{2} \times 100 \\ N_{2} = 2 \times 10^{- 4} \\ [H^{+}] = 2 \times 10^{- 4} M \end{aligned}$

MHT CET-2009

Ionic Equilibrium

229668 Which one of the following species acts as both Bronsted acid and base?

1

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

2

{HPO}_{3}^{2 -}

3

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

4 All of these

Explanation:

: ${HPO}_{4}^{2 -}$ act as both Bronsted acid and bronsted base.
$\begin{array}{ll} {HPO}_{4}^{2 -} + H_{2} O ◻ & H_{2} {PO}_{4}^{-} + {OH}^{-} \\ {HPO}_{4}^{2 -} + H_{2} O ◻ & {PO}_{4}^{3 -} + H_{3} O^{+} \end{array}$
$H_{2} {PO}_{2}^{-}$ is conjugate base of $H_{3} {PO}_{2}$ (a monobasic acid) and does not give $H^{+}$ .
${HPO}_{3}^{2 -}$ is a conjugate base of $H_{2} {PO}_{3}^{-}$ and does not ionize further.
$H_{3} {PO}_{3}$ is a dibasic acid.

UPTU/UPSEE-2015

Ionic Equilibrium

229670 Which of the following is an amphoteric oxide?

1

{SO}_{3}

2

Mg

3

{Al}_{2} O_{3}

4

P_{4} O_{10}

МНТ СЕТ -2007

Explanation:

:
Amphoteric
- These are the oxides that can react with both acids and as well as bases to form salt and water.
- These possess both acidic and basic properties.
- ${Al}_{2} O_{3}, {SiO}_{2}$ is an example of Amphoteric oxide
- ${Al}_{2} O_{3} + 2 NaOH$ (Base) $\to 2 {NaAlO}_{2} + H_{2} O$
- ${Al}_{2} O_{3} + 6 HCl$ (acid) $\to 2 {AlCl}_{3} + 3 H_{2} O$

Ionic Equilibrium

229663 ${NH}_{4} Cl$ is acidic due to

1 Cationic hydrolysis

2 Anionic hydrolysis

3 Its ionic nature

4

pH > 7

Explanation:

: ${NH}_{4} Cl$ is a salt of strong acid $HCl$ and weak base ${NH}_{4} OH$ .
Hydrolysis:-
$\begin{aligned} {NH}_{4} Cl + H_{2} O ◻ {NH}_{4} OH + HCl \\ {NH}_{4}^{+} + {Cl}^{-} + H_{2} O ◻ {NH}_{4} OH + H^{+} + {Cl}^{-} \\ {NH}_{4}^{+} (aq) + H_{2} O (l) ◻ {NH}_{4} OH (aq) + H^{+} (aq) \end{aligned}$
Only the cation will undergo hydrolysis and the solution will be acidic in nature due to $H^{+}$ formation. So here the cation is responsible for the acidic nature of the solution.

MHT CET-2010

Ionic Equilibrium

229666 If $20 mL$ of an acidic solution of $pH = 3$ is diluted to $100 mL$ , the $H^{+}$ ion concentration will be

1

1 \times 10^{- 3} M

2

2 \times 10^{- 3} M

3

2 \times 10^{- 4} M

4

0.02 \times 10^{- 4} M

Explanation:

: Given that -
$\begin{aligned} pH = 3 \\ V_{1} = 20 ml V_{2} = 100 ml \\ H^{+} = ? \\ H^{+} = 1 \times 10^{- 3} m = 1 \times 10^{- 3} N \\ N_{1} V_{1} = N_{2} V_{2} \\ 1 \times 10^{- 3} \times 20 = N_{2} \times 100 \\ N_{2} = 2 \times 10^{- 4} \\ [H^{+}] = 2 \times 10^{- 4} M \end{aligned}$

MHT CET-2009

Ionic Equilibrium

229668 Which one of the following species acts as both Bronsted acid and base?

1

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

2

{HPO}_{3}^{2 -}

3

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

4 All of these

Explanation:

: ${HPO}_{4}^{2 -}$ act as both Bronsted acid and bronsted base.
$\begin{array}{ll} {HPO}_{4}^{2 -} + H_{2} O ◻ & H_{2} {PO}_{4}^{-} + {OH}^{-} \\ {HPO}_{4}^{2 -} + H_{2} O ◻ & {PO}_{4}^{3 -} + H_{3} O^{+} \end{array}$
$H_{2} {PO}_{2}^{-}$ is conjugate base of $H_{3} {PO}_{2}$ (a monobasic acid) and does not give $H^{+}$ .
${HPO}_{3}^{2 -}$ is a conjugate base of $H_{2} {PO}_{3}^{-}$ and does not ionize further.
$H_{3} {PO}_{3}$ is a dibasic acid.

UPTU/UPSEE-2015

Ionic Equilibrium

229670 Which of the following is an amphoteric oxide?

1

{SO}_{3}

2

Mg

3

{Al}_{2} O_{3}

4

P_{4} O_{10}

МНТ СЕТ -2007

Explanation:

:
Amphoteric
- These are the oxides that can react with both acids and as well as bases to form salt and water.
- These possess both acidic and basic properties.
- ${Al}_{2} O_{3}, {SiO}_{2}$ is an example of Amphoteric oxide
- ${Al}_{2} O_{3} + 2 NaOH$ (Base) $\to 2 {NaAlO}_{2} + H_{2} O$
- ${Al}_{2} O_{3} + 6 HCl$ (acid) $\to 2 {AlCl}_{3} + 3 H_{2} O$

Ionic Equilibrium

229663 ${NH}_{4} Cl$ is acidic due to

1 Cationic hydrolysis

2 Anionic hydrolysis

3 Its ionic nature

4

pH > 7

Explanation:

: ${NH}_{4} Cl$ is a salt of strong acid $HCl$ and weak base ${NH}_{4} OH$ .
Hydrolysis:-
$\begin{aligned} {NH}_{4} Cl + H_{2} O ◻ {NH}_{4} OH + HCl \\ {NH}_{4}^{+} + {Cl}^{-} + H_{2} O ◻ {NH}_{4} OH + H^{+} + {Cl}^{-} \\ {NH}_{4}^{+} (aq) + H_{2} O (l) ◻ {NH}_{4} OH (aq) + H^{+} (aq) \end{aligned}$
Only the cation will undergo hydrolysis and the solution will be acidic in nature due to $H^{+}$ formation. So here the cation is responsible for the acidic nature of the solution.

MHT CET-2010

Ionic Equilibrium

229666 If $20 mL$ of an acidic solution of $pH = 3$ is diluted to $100 mL$ , the $H^{+}$ ion concentration will be

1

1 \times 10^{- 3} M

2

2 \times 10^{- 3} M

3

2 \times 10^{- 4} M

4

0.02 \times 10^{- 4} M

Explanation:

: Given that -
$\begin{aligned} pH = 3 \\ V_{1} = 20 ml V_{2} = 100 ml \\ H^{+} = ? \\ H^{+} = 1 \times 10^{- 3} m = 1 \times 10^{- 3} N \\ N_{1} V_{1} = N_{2} V_{2} \\ 1 \times 10^{- 3} \times 20 = N_{2} \times 100 \\ N_{2} = 2 \times 10^{- 4} \\ [H^{+}] = 2 \times 10^{- 4} M \end{aligned}$

MHT CET-2009

Ionic Equilibrium

229668 Which one of the following species acts as both Bronsted acid and base?

1

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

2

{HPO}_{3}^{2 -}

3

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

4 All of these

Explanation:

: ${HPO}_{4}^{2 -}$ act as both Bronsted acid and bronsted base.
$\begin{array}{ll} {HPO}_{4}^{2 -} + H_{2} O ◻ & H_{2} {PO}_{4}^{-} + {OH}^{-} \\ {HPO}_{4}^{2 -} + H_{2} O ◻ & {PO}_{4}^{3 -} + H_{3} O^{+} \end{array}$
$H_{2} {PO}_{2}^{-}$ is conjugate base of $H_{3} {PO}_{2}$ (a monobasic acid) and does not give $H^{+}$ .
${HPO}_{3}^{2 -}$ is a conjugate base of $H_{2} {PO}_{3}^{-}$ and does not ionize further.
$H_{3} {PO}_{3}$ is a dibasic acid.

UPTU/UPSEE-2015

Ionic Equilibrium

229670 Which of the following is an amphoteric oxide?

1

{SO}_{3}

2

Mg

3

{Al}_{2} O_{3}

4

P_{4} O_{10}

МНТ СЕТ -2007

Explanation:

:
Amphoteric
- These are the oxides that can react with both acids and as well as bases to form salt and water.
- These possess both acidic and basic properties.
- ${Al}_{2} O_{3}, {SiO}_{2}$ is an example of Amphoteric oxide
- ${Al}_{2} O_{3} + 2 NaOH$ (Base) $\to 2 {NaAlO}_{2} + H_{2} O$
- ${Al}_{2} O_{3} + 6 HCl$ (acid) $\to 2 {AlCl}_{3} + 3 H_{2} O$

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