According to the Lewis theory an acid is a electron pair acceptor. lewis acids accept an electron pair. Lewis acids are electrophilic meaning that they are electron attracting when bonding with a base the acid uses its lowest unoccupied molecular orbital.
COMEDK-2011
Ionic Equilibrium
229523
The conjugate base of $\mathrm{HSO}_4^{-}$ion is ....
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{H}_3 \mathrm{SO}_4^{+}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{O}^{2-}$
Explanation:
Although it has a negative charge, it will never accept a $\mathrm{H}^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$ (sulfuric acid). That is because sulfuric acid is a strong acid and completely disassociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{2-}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$ $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}} \xrightarrow{-\mathrm{H}^{+}} \underset{\substack{\text { Conjugate base }}}{\mathrm{SO}_4^{2-}}$
AP-EAMCET-1991
Ionic Equilibrium
229521
The conjugate acid of $\mathrm{N}_3^{-}$(azide ion) is:
1 $\mathrm{NH}_3$
2 $\mathrm{HN}_3$
3 $\mathrm{NH}_2^{-}$
4 $\mathrm{N}_2^{-}$
Explanation:
The species formed by the addition of proton in a base is called conjugate acid. $\underset{\text { Base }}{\mathrm{N}_3^{-}}+\underset{\text { Proton }}{\mathrm{H}^{+}} \rightarrow \underset{\substack{\text { Conjugate acid }}}{\mathrm{HN}_3}$
AP-EAMCET (Med.)-1999
Ionic Equilibrium
229529
The conjugate base of $\mathrm{NH}_2^{-}$is
1 $\mathrm{NH}_3$
2 $\mathrm{NH}^{2-}$
3 $\mathrm{NH}_4^{+}$
4 $\mathrm{N}_3^{-}$
Explanation:
Conjugate base is defined by a substance formed when an acid losses a hydrogen ion. The conjugate base of $\mathrm{NH}_2^{-}$. $\mathrm{NH}_2^{-} \xrightarrow{-\mathrm{H}^{+}} \mathrm{NH}^{2-}$
According to the Lewis theory an acid is a electron pair acceptor. lewis acids accept an electron pair. Lewis acids are electrophilic meaning that they are electron attracting when bonding with a base the acid uses its lowest unoccupied molecular orbital.
COMEDK-2011
Ionic Equilibrium
229523
The conjugate base of $\mathrm{HSO}_4^{-}$ion is ....
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{H}_3 \mathrm{SO}_4^{+}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{O}^{2-}$
Explanation:
Although it has a negative charge, it will never accept a $\mathrm{H}^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$ (sulfuric acid). That is because sulfuric acid is a strong acid and completely disassociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{2-}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$ $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}} \xrightarrow{-\mathrm{H}^{+}} \underset{\substack{\text { Conjugate base }}}{\mathrm{SO}_4^{2-}}$
AP-EAMCET-1991
Ionic Equilibrium
229521
The conjugate acid of $\mathrm{N}_3^{-}$(azide ion) is:
1 $\mathrm{NH}_3$
2 $\mathrm{HN}_3$
3 $\mathrm{NH}_2^{-}$
4 $\mathrm{N}_2^{-}$
Explanation:
The species formed by the addition of proton in a base is called conjugate acid. $\underset{\text { Base }}{\mathrm{N}_3^{-}}+\underset{\text { Proton }}{\mathrm{H}^{+}} \rightarrow \underset{\substack{\text { Conjugate acid }}}{\mathrm{HN}_3}$
AP-EAMCET (Med.)-1999
Ionic Equilibrium
229529
The conjugate base of $\mathrm{NH}_2^{-}$is
1 $\mathrm{NH}_3$
2 $\mathrm{NH}^{2-}$
3 $\mathrm{NH}_4^{+}$
4 $\mathrm{N}_3^{-}$
Explanation:
Conjugate base is defined by a substance formed when an acid losses a hydrogen ion. The conjugate base of $\mathrm{NH}_2^{-}$. $\mathrm{NH}_2^{-} \xrightarrow{-\mathrm{H}^{+}} \mathrm{NH}^{2-}$
According to the Lewis theory an acid is a electron pair acceptor. lewis acids accept an electron pair. Lewis acids are electrophilic meaning that they are electron attracting when bonding with a base the acid uses its lowest unoccupied molecular orbital.
COMEDK-2011
Ionic Equilibrium
229523
The conjugate base of $\mathrm{HSO}_4^{-}$ion is ....
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{H}_3 \mathrm{SO}_4^{+}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{O}^{2-}$
Explanation:
Although it has a negative charge, it will never accept a $\mathrm{H}^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$ (sulfuric acid). That is because sulfuric acid is a strong acid and completely disassociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{2-}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$ $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}} \xrightarrow{-\mathrm{H}^{+}} \underset{\substack{\text { Conjugate base }}}{\mathrm{SO}_4^{2-}}$
AP-EAMCET-1991
Ionic Equilibrium
229521
The conjugate acid of $\mathrm{N}_3^{-}$(azide ion) is:
1 $\mathrm{NH}_3$
2 $\mathrm{HN}_3$
3 $\mathrm{NH}_2^{-}$
4 $\mathrm{N}_2^{-}$
Explanation:
The species formed by the addition of proton in a base is called conjugate acid. $\underset{\text { Base }}{\mathrm{N}_3^{-}}+\underset{\text { Proton }}{\mathrm{H}^{+}} \rightarrow \underset{\substack{\text { Conjugate acid }}}{\mathrm{HN}_3}$
AP-EAMCET (Med.)-1999
Ionic Equilibrium
229529
The conjugate base of $\mathrm{NH}_2^{-}$is
1 $\mathrm{NH}_3$
2 $\mathrm{NH}^{2-}$
3 $\mathrm{NH}_4^{+}$
4 $\mathrm{N}_3^{-}$
Explanation:
Conjugate base is defined by a substance formed when an acid losses a hydrogen ion. The conjugate base of $\mathrm{NH}_2^{-}$. $\mathrm{NH}_2^{-} \xrightarrow{-\mathrm{H}^{+}} \mathrm{NH}^{2-}$
According to the Lewis theory an acid is a electron pair acceptor. lewis acids accept an electron pair. Lewis acids are electrophilic meaning that they are electron attracting when bonding with a base the acid uses its lowest unoccupied molecular orbital.
COMEDK-2011
Ionic Equilibrium
229523
The conjugate base of $\mathrm{HSO}_4^{-}$ion is ....
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{H}_3 \mathrm{SO}_4^{+}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{O}^{2-}$
Explanation:
Although it has a negative charge, it will never accept a $\mathrm{H}^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$ (sulfuric acid). That is because sulfuric acid is a strong acid and completely disassociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{2-}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$ $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}} \xrightarrow{-\mathrm{H}^{+}} \underset{\substack{\text { Conjugate base }}}{\mathrm{SO}_4^{2-}}$
AP-EAMCET-1991
Ionic Equilibrium
229521
The conjugate acid of $\mathrm{N}_3^{-}$(azide ion) is:
1 $\mathrm{NH}_3$
2 $\mathrm{HN}_3$
3 $\mathrm{NH}_2^{-}$
4 $\mathrm{N}_2^{-}$
Explanation:
The species formed by the addition of proton in a base is called conjugate acid. $\underset{\text { Base }}{\mathrm{N}_3^{-}}+\underset{\text { Proton }}{\mathrm{H}^{+}} \rightarrow \underset{\substack{\text { Conjugate acid }}}{\mathrm{HN}_3}$
AP-EAMCET (Med.)-1999
Ionic Equilibrium
229529
The conjugate base of $\mathrm{NH}_2^{-}$is
1 $\mathrm{NH}_3$
2 $\mathrm{NH}^{2-}$
3 $\mathrm{NH}_4^{+}$
4 $\mathrm{N}_3^{-}$
Explanation:
Conjugate base is defined by a substance formed when an acid losses a hydrogen ion. The conjugate base of $\mathrm{NH}_2^{-}$. $\mathrm{NH}_2^{-} \xrightarrow{-\mathrm{H}^{+}} \mathrm{NH}^{2-}$
