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Ionic Equilibrium

229530 Which one of the following salts gives an acidic solution in water?

1

{CH}_{3} COONa

2

{NH}_{4} Cl

3

NaCl

4

{CH}_{3} {COONH}_{4}

Explanation:

Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $HCl$ is a strong acid.
${NH}_{4} Cl$ ? ${NH}_{4}^{+} + {Cl}^{-}$
$2 H_{2} OG$ ? ${OH}^{-} + H_{3} O^{+}$
${NH}_{4}^{+} + {OH}^{-}$ ?? ${NH}_{4} OH$

AP-EAMCET-2007

Ionic Equilibrium

229534 When a particular aqueous solution is diluted by a factor of ten with $K_{2} O$ , the $pH$ increases by one unit. the solution most likely contains a

1 Weak acid

2 Strong base

3 Strong acid

4 Buffer

Explanation:

The increasing of $pH$ by one unit, that means the solution is more acidic because the $pH$ scale show the acidic character from 1 to 7 . Less the value in $pH$ scale, higher acidity of the solution will be.
Weak acid $\to$ Acid that don't completely dissociated in solution.
Strong acid $\to$ Completely dissociated in solution ExaChloric acid hydrobromic acid.
Buffer $\to$ A buffer Solution are resist a change in $pH$ when small acid or alkali are added.

**SCRA-2014**

Ionic Equilibrium

229535 Consider the following regarding potash alum:
1.It has 24 water molecules.
2.It swells on heating.
3.Its aqueous solution is basic.
4.It is white in colour.
Which of the above statements are correct?

1 1 and 2 only

2 1,3 and 4

3 2,3 and 4

4 1,2 and 4

Explanation:

The formula of potash alum is $K_{2} {SO}_{4} {Al}_{2} {({SO}_{4})}_{3} .24 H_{2} O$ .
It is white in colour.
It has 24 water molecules and it swells on heating.

SCRA 2010

Ionic Equilibrium

229537 In the reaction $H_{2} O + HCl \to H_{3} O^{+} + {Cl}^{-}$ , the species that acts as Bronsted base is :

1

H_{2} O

2

HCl

3

H_{3} O^{+}

4

{Cl}^{-}

Explanation:

A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $H^{+}$ . Ex. $H_{2} O$ .
$\underset{Acid}{HCl} + \underset{Base}{H_{2} O} \to \underset{\begin{matrix} Conjugate \\ base \end{matrix}}{{Cl}^{-}} + \underset{\begin{matrix} Conjugate \\ acid \end{matrix}}{H_{3} O^{+}}$
- Bronsted-Lowry acids are proton/ $/ H^{+}$ doners (Lose $H^{+})$

MPPET-2013

Ionic Equilibrium

229530 Which one of the following salts gives an acidic solution in water?

1

{CH}_{3} COONa

2

{NH}_{4} Cl

3

NaCl

4

{CH}_{3} {COONH}_{4}

Explanation:

Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $HCl$ is a strong acid.
${NH}_{4} Cl$ ? ${NH}_{4}^{+} + {Cl}^{-}$
$2 H_{2} OG$ ? ${OH}^{-} + H_{3} O^{+}$
${NH}_{4}^{+} + {OH}^{-}$ ?? ${NH}_{4} OH$

AP-EAMCET-2007

Ionic Equilibrium

229534 When a particular aqueous solution is diluted by a factor of ten with $K_{2} O$ , the $pH$ increases by one unit. the solution most likely contains a

1 Weak acid

2 Strong base

3 Strong acid

4 Buffer

Explanation:

The increasing of $pH$ by one unit, that means the solution is more acidic because the $pH$ scale show the acidic character from 1 to 7 . Less the value in $pH$ scale, higher acidity of the solution will be.
Weak acid $\to$ Acid that don't completely dissociated in solution.
Strong acid $\to$ Completely dissociated in solution ExaChloric acid hydrobromic acid.
Buffer $\to$ A buffer Solution are resist a change in $pH$ when small acid or alkali are added.

**SCRA-2014**

Ionic Equilibrium

229535 Consider the following regarding potash alum:
1.It has 24 water molecules.
2.It swells on heating.
3.Its aqueous solution is basic.
4.It is white in colour.
Which of the above statements are correct?

1 1 and 2 only

2 1,3 and 4

3 2,3 and 4

4 1,2 and 4

Explanation:

The formula of potash alum is $K_{2} {SO}_{4} {Al}_{2} {({SO}_{4})}_{3} .24 H_{2} O$ .
It is white in colour.
It has 24 water molecules and it swells on heating.

SCRA 2010

Ionic Equilibrium

229537 In the reaction $H_{2} O + HCl \to H_{3} O^{+} + {Cl}^{-}$ , the species that acts as Bronsted base is :

1

H_{2} O

2

HCl

3

H_{3} O^{+}

4

{Cl}^{-}

Explanation:

A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $H^{+}$ . Ex. $H_{2} O$ .
$\underset{Acid}{HCl} + \underset{Base}{H_{2} O} \to \underset{\begin{matrix} Conjugate \\ base \end{matrix}}{{Cl}^{-}} + \underset{\begin{matrix} Conjugate \\ acid \end{matrix}}{H_{3} O^{+}}$
- Bronsted-Lowry acids are proton/ $/ H^{+}$ doners (Lose $H^{+})$

MPPET-2013

Ionic Equilibrium

229530 Which one of the following salts gives an acidic solution in water?

1

{CH}_{3} COONa

2

{NH}_{4} Cl

3

NaCl

4

{CH}_{3} {COONH}_{4}

Explanation:

Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $HCl$ is a strong acid.
${NH}_{4} Cl$ ? ${NH}_{4}^{+} + {Cl}^{-}$
$2 H_{2} OG$ ? ${OH}^{-} + H_{3} O^{+}$
${NH}_{4}^{+} + {OH}^{-}$ ?? ${NH}_{4} OH$

AP-EAMCET-2007

Ionic Equilibrium

229534 When a particular aqueous solution is diluted by a factor of ten with $K_{2} O$ , the $pH$ increases by one unit. the solution most likely contains a

1 Weak acid

2 Strong base

3 Strong acid

4 Buffer

Explanation:

The increasing of $pH$ by one unit, that means the solution is more acidic because the $pH$ scale show the acidic character from 1 to 7 . Less the value in $pH$ scale, higher acidity of the solution will be.
Weak acid $\to$ Acid that don't completely dissociated in solution.
Strong acid $\to$ Completely dissociated in solution ExaChloric acid hydrobromic acid.
Buffer $\to$ A buffer Solution are resist a change in $pH$ when small acid or alkali are added.

**SCRA-2014**

Ionic Equilibrium

229535 Consider the following regarding potash alum:
1.It has 24 water molecules.
2.It swells on heating.
3.Its aqueous solution is basic.
4.It is white in colour.
Which of the above statements are correct?

1 1 and 2 only

2 1,3 and 4

3 2,3 and 4

4 1,2 and 4

Explanation:

The formula of potash alum is $K_{2} {SO}_{4} {Al}_{2} {({SO}_{4})}_{3} .24 H_{2} O$ .
It is white in colour.
It has 24 water molecules and it swells on heating.

SCRA 2010

Ionic Equilibrium

229537 In the reaction $H_{2} O + HCl \to H_{3} O^{+} + {Cl}^{-}$ , the species that acts as Bronsted base is :

1

H_{2} O

2

HCl

3

H_{3} O^{+}

4

{Cl}^{-}

Explanation:

A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $H^{+}$ . Ex. $H_{2} O$ .
$\underset{Acid}{HCl} + \underset{Base}{H_{2} O} \to \underset{\begin{matrix} Conjugate \\ base \end{matrix}}{{Cl}^{-}} + \underset{\begin{matrix} Conjugate \\ acid \end{matrix}}{H_{3} O^{+}}$
- Bronsted-Lowry acids are proton/ $/ H^{+}$ doners (Lose $H^{+})$

MPPET-2013

Ionic Equilibrium

229530 Which one of the following salts gives an acidic solution in water?

1

{CH}_{3} COONa

2

{NH}_{4} Cl

3

NaCl

4

{CH}_{3} {COONH}_{4}

Explanation:

Ammonium chloride when dissolved in water gives hydrochloric acid which makes the solution acidic in nature as $HCl$ is a strong acid.
${NH}_{4} Cl$ ? ${NH}_{4}^{+} + {Cl}^{-}$
$2 H_{2} OG$ ? ${OH}^{-} + H_{3} O^{+}$
${NH}_{4}^{+} + {OH}^{-}$ ?? ${NH}_{4} OH$

AP-EAMCET-2007

Ionic Equilibrium

229534 When a particular aqueous solution is diluted by a factor of ten with $K_{2} O$ , the $pH$ increases by one unit. the solution most likely contains a

1 Weak acid

2 Strong base

3 Strong acid

4 Buffer

Explanation:

The increasing of $pH$ by one unit, that means the solution is more acidic because the $pH$ scale show the acidic character from 1 to 7 . Less the value in $pH$ scale, higher acidity of the solution will be.
Weak acid $\to$ Acid that don't completely dissociated in solution.
Strong acid $\to$ Completely dissociated in solution ExaChloric acid hydrobromic acid.
Buffer $\to$ A buffer Solution are resist a change in $pH$ when small acid or alkali are added.

**SCRA-2014**

Ionic Equilibrium

229535 Consider the following regarding potash alum:
1.It has 24 water molecules.
2.It swells on heating.
3.Its aqueous solution is basic.
4.It is white in colour.
Which of the above statements are correct?

1 1 and 2 only

2 1,3 and 4

3 2,3 and 4

4 1,2 and 4

Explanation:

The formula of potash alum is $K_{2} {SO}_{4} {Al}_{2} {({SO}_{4})}_{3} .24 H_{2} O$ .
It is white in colour.
It has 24 water molecules and it swells on heating.

SCRA 2010

Ionic Equilibrium

229537 In the reaction $H_{2} O + HCl \to H_{3} O^{+} + {Cl}^{-}$ , the species that acts as Bronsted base is :

1

H_{2} O

2

HCl

3

H_{3} O^{+}

4

{Cl}^{-}

Explanation:

A Bronsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the $H^{+}$ . Ex. $H_{2} O$ .
$\underset{Acid}{HCl} + \underset{Base}{H_{2} O} \to \underset{\begin{matrix} Conjugate \\ base \end{matrix}}{{Cl}^{-}} + \underset{\begin{matrix} Conjugate \\ acid \end{matrix}}{H_{3} O^{+}}$
- Bronsted-Lowry acids are proton/ $/ H^{+}$ doners (Lose $H^{+})$

MPPET-2013

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