QBManager

Ionic Equilibrium

229578 In the reaction $I_{2} + I^{-} \to I_{3}^{-}$ , the Lewis base is:

1

I_{3}^{-}

2

I_{2}

3

I^{-}

4 non of these

Explanation:

$F$ ion can act as Lewis base i.e. It can denote electron pair to some species.
Here, $F^{-}$ is giving electron pair to $I_{2}$ molecule. Therefore $I_{2}$ is a lewis acid and $Γ^{-}$ is a lewis base.

BCECE-2005

Ionic Equilibrium

229583 Which one of the following compounds is Lewis acid?

1

{PCl}_{3}

2

{BCl}_{3}

3

{NCl}_{3}

4

{CHCl}_{3}

Explanation:

In ${BCl}_{3}$ , Boron has 6 electrons in it outermost orbital and has a vacant p-orbital. Thus, it is an electron-deficient compound.
Hence, it acts as Lewis acid and accepts a loan pair of electrons.

AP - EAMCET - (Medical)-1997

Ionic Equilibrium

229584 The conjugate acid of ${NH}_{2}^{-}$ ion is:

1

{NH}_{3}

2

{NH}_{4}^{+}

3

N_{2} H_{4}

4

{NH}_{2} OH

Explanation:

According to Bronsted-Lowery theory of acid and base, the species which accepting a proton is called conjugate acid of the base.
$\underset{Base}{{NH}_{2}^{-}} + H^{+} ⟶ \underset{Conjugate acid}{{NH}_{3}}$

COMEDK 2012]**

Ionic Equilibrium

229586 The strongest conjugate base results from':

1 Formic acid

2 Benzoic acid

3 Acetic acid

4 Acetylene

Explanation:

The compounds which donates a proton are called acid and compounds which accept proton are called base. When an acid donate a proton is called conjugate base of that acid.
The strongest conjugate base results from acetylene since it is the weakest acid among formic acid, benzoic acid, acetic acid and acetylene.
The order of strength of acids is given below-
Acetylene $<$ Acetic acid $<$ Formic acid $<$ Benzoic acid Weaker an acid, stronger will be its conjugate base. Hence, the order of strength of conjugate bases will be as follows-
Acetylene $>$ Acetic acid $>$ Formic acid $>$ Benzoic acid

AP-EAMCET-1998]**

Ionic Equilibrium

229587 Which of the following oxide is amphoteric?

1

{SnO}_{2}

2

CaO

3

{SiO}_{2}

4

{CO}_{2}

Explanation:

Amphoteric oxides reacts with both acids and alkalis to form salts and water. Examples of amphoteric oxides are zinc oxide aluminium oxide and tin oxide. Generally in group $14 {SiO}_{2}$ and ${CO}_{2}$ are acidic where as in second group due to alkali nature of elements it oxide are basic.
Amphoteric $\to$ Acidic/Basic
Metals $\to$ Basic, Amphoteric
Amphoteric Metals $\to Be, Sc, Ti, V, Cr, Fe, Co, Cu, Zn$ , $Al, Ge, Sn, Zn, Ag, Ga, Au, In, T 1, Pb, Sb, Bi$

VITEEE-2012

Ionic Equilibrium

229578 In the reaction $I_{2} + I^{-} \to I_{3}^{-}$ , the Lewis base is:

1

I_{3}^{-}

2

I_{2}

3

I^{-}

4 non of these

Explanation:

$F$ ion can act as Lewis base i.e. It can denote electron pair to some species.
Here, $F^{-}$ is giving electron pair to $I_{2}$ molecule. Therefore $I_{2}$ is a lewis acid and $Γ^{-}$ is a lewis base.

BCECE-2005

Ionic Equilibrium

229583 Which one of the following compounds is Lewis acid?

1

{PCl}_{3}

2

{BCl}_{3}

3

{NCl}_{3}

4

{CHCl}_{3}

Explanation:

In ${BCl}_{3}$ , Boron has 6 electrons in it outermost orbital and has a vacant p-orbital. Thus, it is an electron-deficient compound.
Hence, it acts as Lewis acid and accepts a loan pair of electrons.

AP - EAMCET - (Medical)-1997

Ionic Equilibrium

229584 The conjugate acid of ${NH}_{2}^{-}$ ion is:

1

{NH}_{3}

2

{NH}_{4}^{+}

3

N_{2} H_{4}

4

{NH}_{2} OH

Explanation:

According to Bronsted-Lowery theory of acid and base, the species which accepting a proton is called conjugate acid of the base.
$\underset{Base}{{NH}_{2}^{-}} + H^{+} ⟶ \underset{Conjugate acid}{{NH}_{3}}$

COMEDK 2012]**

Ionic Equilibrium

229586 The strongest conjugate base results from':

1 Formic acid

2 Benzoic acid

3 Acetic acid

4 Acetylene

Explanation:

The compounds which donates a proton are called acid and compounds which accept proton are called base. When an acid donate a proton is called conjugate base of that acid.
The strongest conjugate base results from acetylene since it is the weakest acid among formic acid, benzoic acid, acetic acid and acetylene.
The order of strength of acids is given below-
Acetylene $<$ Acetic acid $<$ Formic acid $<$ Benzoic acid Weaker an acid, stronger will be its conjugate base. Hence, the order of strength of conjugate bases will be as follows-
Acetylene $>$ Acetic acid $>$ Formic acid $>$ Benzoic acid

AP-EAMCET-1998]**

Ionic Equilibrium

229587 Which of the following oxide is amphoteric?

1

{SnO}_{2}

2

CaO

3

{SiO}_{2}

4

{CO}_{2}

Explanation:

Amphoteric oxides reacts with both acids and alkalis to form salts and water. Examples of amphoteric oxides are zinc oxide aluminium oxide and tin oxide. Generally in group $14 {SiO}_{2}$ and ${CO}_{2}$ are acidic where as in second group due to alkali nature of elements it oxide are basic.
Amphoteric $\to$ Acidic/Basic
Metals $\to$ Basic, Amphoteric
Amphoteric Metals $\to Be, Sc, Ti, V, Cr, Fe, Co, Cu, Zn$ , $Al, Ge, Sn, Zn, Ag, Ga, Au, In, T 1, Pb, Sb, Bi$

VITEEE-2012

Ionic Equilibrium

229578 In the reaction $I_{2} + I^{-} \to I_{3}^{-}$ , the Lewis base is:

1

I_{3}^{-}

2

I_{2}

3

I^{-}

4 non of these

Explanation:

$F$ ion can act as Lewis base i.e. It can denote electron pair to some species.
Here, $F^{-}$ is giving electron pair to $I_{2}$ molecule. Therefore $I_{2}$ is a lewis acid and $Γ^{-}$ is a lewis base.

BCECE-2005

Ionic Equilibrium

229583 Which one of the following compounds is Lewis acid?

1

{PCl}_{3}

2

{BCl}_{3}

3

{NCl}_{3}

4

{CHCl}_{3}

Explanation:

In ${BCl}_{3}$ , Boron has 6 electrons in it outermost orbital and has a vacant p-orbital. Thus, it is an electron-deficient compound.
Hence, it acts as Lewis acid and accepts a loan pair of electrons.

AP - EAMCET - (Medical)-1997

Ionic Equilibrium

229584 The conjugate acid of ${NH}_{2}^{-}$ ion is:

1

{NH}_{3}

2

{NH}_{4}^{+}

3

N_{2} H_{4}

4

{NH}_{2} OH

Explanation:

According to Bronsted-Lowery theory of acid and base, the species which accepting a proton is called conjugate acid of the base.
$\underset{Base}{{NH}_{2}^{-}} + H^{+} ⟶ \underset{Conjugate acid}{{NH}_{3}}$

COMEDK 2012]**

Ionic Equilibrium

229586 The strongest conjugate base results from':

1 Formic acid

2 Benzoic acid

3 Acetic acid

4 Acetylene

Explanation:

The compounds which donates a proton are called acid and compounds which accept proton are called base. When an acid donate a proton is called conjugate base of that acid.
The strongest conjugate base results from acetylene since it is the weakest acid among formic acid, benzoic acid, acetic acid and acetylene.
The order of strength of acids is given below-
Acetylene $<$ Acetic acid $<$ Formic acid $<$ Benzoic acid Weaker an acid, stronger will be its conjugate base. Hence, the order of strength of conjugate bases will be as follows-
Acetylene $>$ Acetic acid $>$ Formic acid $>$ Benzoic acid

AP-EAMCET-1998]**

Ionic Equilibrium

229587 Which of the following oxide is amphoteric?

1

{SnO}_{2}

2

CaO

3

{SiO}_{2}

4

{CO}_{2}

Explanation:

Amphoteric oxides reacts with both acids and alkalis to form salts and water. Examples of amphoteric oxides are zinc oxide aluminium oxide and tin oxide. Generally in group $14 {SiO}_{2}$ and ${CO}_{2}$ are acidic where as in second group due to alkali nature of elements it oxide are basic.
Amphoteric $\to$ Acidic/Basic
Metals $\to$ Basic, Amphoteric
Amphoteric Metals $\to Be, Sc, Ti, V, Cr, Fe, Co, Cu, Zn$ , $Al, Ge, Sn, Zn, Ag, Ga, Au, In, T 1, Pb, Sb, Bi$

VITEEE-2012

Ionic Equilibrium

229578 In the reaction $I_{2} + I^{-} \to I_{3}^{-}$ , the Lewis base is:

1

I_{3}^{-}

2

I_{2}

3

I^{-}

4 non of these

Explanation:

$F$ ion can act as Lewis base i.e. It can denote electron pair to some species.
Here, $F^{-}$ is giving electron pair to $I_{2}$ molecule. Therefore $I_{2}$ is a lewis acid and $Γ^{-}$ is a lewis base.

BCECE-2005

Ionic Equilibrium

229583 Which one of the following compounds is Lewis acid?

1

{PCl}_{3}

2

{BCl}_{3}

3

{NCl}_{3}

4

{CHCl}_{3}

Explanation:

In ${BCl}_{3}$ , Boron has 6 electrons in it outermost orbital and has a vacant p-orbital. Thus, it is an electron-deficient compound.
Hence, it acts as Lewis acid and accepts a loan pair of electrons.

AP - EAMCET - (Medical)-1997

Ionic Equilibrium

229584 The conjugate acid of ${NH}_{2}^{-}$ ion is:

1

{NH}_{3}

2

{NH}_{4}^{+}

3

N_{2} H_{4}

4

{NH}_{2} OH

Explanation:

According to Bronsted-Lowery theory of acid and base, the species which accepting a proton is called conjugate acid of the base.
$\underset{Base}{{NH}_{2}^{-}} + H^{+} ⟶ \underset{Conjugate acid}{{NH}_{3}}$

COMEDK 2012]**

Ionic Equilibrium

229586 The strongest conjugate base results from':

1 Formic acid

2 Benzoic acid

3 Acetic acid

4 Acetylene

Explanation:

The compounds which donates a proton are called acid and compounds which accept proton are called base. When an acid donate a proton is called conjugate base of that acid.
The strongest conjugate base results from acetylene since it is the weakest acid among formic acid, benzoic acid, acetic acid and acetylene.
The order of strength of acids is given below-
Acetylene $<$ Acetic acid $<$ Formic acid $<$ Benzoic acid Weaker an acid, stronger will be its conjugate base. Hence, the order of strength of conjugate bases will be as follows-
Acetylene $>$ Acetic acid $>$ Formic acid $>$ Benzoic acid

AP-EAMCET-1998]**

Ionic Equilibrium

229587 Which of the following oxide is amphoteric?

1

{SnO}_{2}

2

CaO

3

{SiO}_{2}

4

{CO}_{2}

Explanation:

Amphoteric oxides reacts with both acids and alkalis to form salts and water. Examples of amphoteric oxides are zinc oxide aluminium oxide and tin oxide. Generally in group $14 {SiO}_{2}$ and ${CO}_{2}$ are acidic where as in second group due to alkali nature of elements it oxide are basic.
Amphoteric $\to$ Acidic/Basic
Metals $\to$ Basic, Amphoteric
Amphoteric Metals $\to Be, Sc, Ti, V, Cr, Fe, Co, Cu, Zn$ , $Al, Ge, Sn, Zn, Ag, Ga, Au, In, T 1, Pb, Sb, Bi$

VITEEE-2012

Ionic Equilibrium

229578 In the reaction $I_{2} + I^{-} \to I_{3}^{-}$ , the Lewis base is:

1

I_{3}^{-}

2

I_{2}

3

I^{-}

4 non of these

Explanation:

$F$ ion can act as Lewis base i.e. It can denote electron pair to some species.
Here, $F^{-}$ is giving electron pair to $I_{2}$ molecule. Therefore $I_{2}$ is a lewis acid and $Γ^{-}$ is a lewis base.

BCECE-2005

Ionic Equilibrium

229583 Which one of the following compounds is Lewis acid?

1

{PCl}_{3}

2

{BCl}_{3}

3

{NCl}_{3}

4

{CHCl}_{3}

Explanation:

In ${BCl}_{3}$ , Boron has 6 electrons in it outermost orbital and has a vacant p-orbital. Thus, it is an electron-deficient compound.
Hence, it acts as Lewis acid and accepts a loan pair of electrons.

AP - EAMCET - (Medical)-1997

Ionic Equilibrium

229584 The conjugate acid of ${NH}_{2}^{-}$ ion is:

1

{NH}_{3}

2

{NH}_{4}^{+}

3

N_{2} H_{4}

4

{NH}_{2} OH

Explanation:

According to Bronsted-Lowery theory of acid and base, the species which accepting a proton is called conjugate acid of the base.
$\underset{Base}{{NH}_{2}^{-}} + H^{+} ⟶ \underset{Conjugate acid}{{NH}_{3}}$

COMEDK 2012]**

Ionic Equilibrium

229586 The strongest conjugate base results from':

1 Formic acid

2 Benzoic acid

3 Acetic acid

4 Acetylene

Explanation:

The compounds which donates a proton are called acid and compounds which accept proton are called base. When an acid donate a proton is called conjugate base of that acid.
The strongest conjugate base results from acetylene since it is the weakest acid among formic acid, benzoic acid, acetic acid and acetylene.
The order of strength of acids is given below-
Acetylene $<$ Acetic acid $<$ Formic acid $<$ Benzoic acid Weaker an acid, stronger will be its conjugate base. Hence, the order of strength of conjugate bases will be as follows-
Acetylene $>$ Acetic acid $>$ Formic acid $>$ Benzoic acid

AP-EAMCET-1998]**

Ionic Equilibrium

229587 Which of the following oxide is amphoteric?

1

{SnO}_{2}

2

CaO

3

{SiO}_{2}

4

{CO}_{2}

Explanation:

Amphoteric oxides reacts with both acids and alkalis to form salts and water. Examples of amphoteric oxides are zinc oxide aluminium oxide and tin oxide. Generally in group $14 {SiO}_{2}$ and ${CO}_{2}$ are acidic where as in second group due to alkali nature of elements it oxide are basic.
Amphoteric $\to$ Acidic/Basic
Metals $\to$ Basic, Amphoteric
Amphoteric Metals $\to Be, Sc, Ti, V, Cr, Fe, Co, Cu, Zn$ , $Al, Ge, Sn, Zn, Ag, Ga, Au, In, T 1, Pb, Sb, Bi$

VITEEE-2012

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Question Bank Series

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation:

Explanation: