229557
What is the conjugate base of $\mathrm{HSO}_4^{-}$?
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{HSO}_4^{2-}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{H}^{+}$
Explanation:
The acid base reaction can be written as:- $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { acidof } \mathrm{H}_2 \mathrm{O}}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\substack{\text { Conseofugate } \\ \mathrm{SO}_2 \mathrm{SO}_4}}{\mathrm{SO}_4^{2-}}$ Although it has a negative charge, it will never accept ah ${ }^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$. That is because $\mathrm{H}_2 \mathrm{SO}_4$ is a strong acid and completely dissociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{-2}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$.
AP-EAMCET (Medical)
Ionic Equilibrium
229561
Which one of the following statements is not correct.
1 $\mathrm{Cl}^{-}$is a Lewis acid
2 The $\mathrm{pH}$ of $10^{-8}$ molar $\mathrm{HCl}$ solution is less than 7
3 the ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$ $\mathrm{mol}^2 \mathrm{~L}^{-2}$
4 Bronsted-Lowry theory could not explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
$\mathrm{Cl}^{-}$is not a Lewis acid. It is a Lewis base. Lewis acid is a chemical species that reacts with a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that donates a pair of electrons to a Lewis acid to form a Lewis adduct. Therefore, $\mathrm{Cl}^{-}$is a Lewis acid statement is not correct.
AP-EAMCET (Medical)
Ionic Equilibrium
229565
The set of amphoteric oxides among the given oxides are $\mathrm{Ga}_2 \mathrm{O}_3, \mathrm{As}_4 \mathrm{O}_{10}, \mathrm{Sb}_4 \mathrm{O}_{10}, \mathrm{~B}_2 \mathrm{O}_3, \mathrm{Tl}_2 \mathrm{O}$
Amphoteric oxides-Metaloxide which react with both basic and acidic oxides to produces salt and water. Ex- $\mathrm{Ga}_2 \mathrm{O}_3, \quad \mathrm{As}_4 \mathrm{O}_{10}, \quad \mathrm{Sb}_4 \mathrm{O}_{10}$ and $\mathrm{Al}_2 \mathrm{O}_3$, all are amphoteric oxides because they react as acid with base and vice-versa.
229557
What is the conjugate base of $\mathrm{HSO}_4^{-}$?
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{HSO}_4^{2-}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{H}^{+}$
Explanation:
The acid base reaction can be written as:- $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { acidof } \mathrm{H}_2 \mathrm{O}}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\substack{\text { Conseofugate } \\ \mathrm{SO}_2 \mathrm{SO}_4}}{\mathrm{SO}_4^{2-}}$ Although it has a negative charge, it will never accept ah ${ }^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$. That is because $\mathrm{H}_2 \mathrm{SO}_4$ is a strong acid and completely dissociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{-2}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$.
AP-EAMCET (Medical)
Ionic Equilibrium
229561
Which one of the following statements is not correct.
1 $\mathrm{Cl}^{-}$is a Lewis acid
2 The $\mathrm{pH}$ of $10^{-8}$ molar $\mathrm{HCl}$ solution is less than 7
3 the ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$ $\mathrm{mol}^2 \mathrm{~L}^{-2}$
4 Bronsted-Lowry theory could not explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
$\mathrm{Cl}^{-}$is not a Lewis acid. It is a Lewis base. Lewis acid is a chemical species that reacts with a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that donates a pair of electrons to a Lewis acid to form a Lewis adduct. Therefore, $\mathrm{Cl}^{-}$is a Lewis acid statement is not correct.
AP-EAMCET (Medical)
Ionic Equilibrium
229565
The set of amphoteric oxides among the given oxides are $\mathrm{Ga}_2 \mathrm{O}_3, \mathrm{As}_4 \mathrm{O}_{10}, \mathrm{Sb}_4 \mathrm{O}_{10}, \mathrm{~B}_2 \mathrm{O}_3, \mathrm{Tl}_2 \mathrm{O}$
Amphoteric oxides-Metaloxide which react with both basic and acidic oxides to produces salt and water. Ex- $\mathrm{Ga}_2 \mathrm{O}_3, \quad \mathrm{As}_4 \mathrm{O}_{10}, \quad \mathrm{Sb}_4 \mathrm{O}_{10}$ and $\mathrm{Al}_2 \mathrm{O}_3$, all are amphoteric oxides because they react as acid with base and vice-versa.
229557
What is the conjugate base of $\mathrm{HSO}_4^{-}$?
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{HSO}_4^{2-}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{H}^{+}$
Explanation:
The acid base reaction can be written as:- $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { acidof } \mathrm{H}_2 \mathrm{O}}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\substack{\text { Conseofugate } \\ \mathrm{SO}_2 \mathrm{SO}_4}}{\mathrm{SO}_4^{2-}}$ Although it has a negative charge, it will never accept ah ${ }^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$. That is because $\mathrm{H}_2 \mathrm{SO}_4$ is a strong acid and completely dissociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{-2}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$.
AP-EAMCET (Medical)
Ionic Equilibrium
229561
Which one of the following statements is not correct.
1 $\mathrm{Cl}^{-}$is a Lewis acid
2 The $\mathrm{pH}$ of $10^{-8}$ molar $\mathrm{HCl}$ solution is less than 7
3 the ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$ $\mathrm{mol}^2 \mathrm{~L}^{-2}$
4 Bronsted-Lowry theory could not explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
$\mathrm{Cl}^{-}$is not a Lewis acid. It is a Lewis base. Lewis acid is a chemical species that reacts with a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that donates a pair of electrons to a Lewis acid to form a Lewis adduct. Therefore, $\mathrm{Cl}^{-}$is a Lewis acid statement is not correct.
AP-EAMCET (Medical)
Ionic Equilibrium
229565
The set of amphoteric oxides among the given oxides are $\mathrm{Ga}_2 \mathrm{O}_3, \mathrm{As}_4 \mathrm{O}_{10}, \mathrm{Sb}_4 \mathrm{O}_{10}, \mathrm{~B}_2 \mathrm{O}_3, \mathrm{Tl}_2 \mathrm{O}$
Amphoteric oxides-Metaloxide which react with both basic and acidic oxides to produces salt and water. Ex- $\mathrm{Ga}_2 \mathrm{O}_3, \quad \mathrm{As}_4 \mathrm{O}_{10}, \quad \mathrm{Sb}_4 \mathrm{O}_{10}$ and $\mathrm{Al}_2 \mathrm{O}_3$, all are amphoteric oxides because they react as acid with base and vice-versa.
229557
What is the conjugate base of $\mathrm{HSO}_4^{-}$?
1 $\mathrm{H}_2 \mathrm{SO}_4$
2 $\mathrm{HSO}_4^{2-}$
3 $\mathrm{SO}_4^{2-}$
4 $\mathrm{H}^{+}$
Explanation:
The acid base reaction can be written as:- $\underset{\text { Acid }}{\mathrm{HSO}_4^{-}}+\underset{\text { Base }}{\mathrm{H}_2 \mathrm{O}} \rightarrow \underset{\substack{\text { Conjugate } \\ \text { acidof } \mathrm{H}_2 \mathrm{O}}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\substack{\text { Conseofugate } \\ \mathrm{SO}_2 \mathrm{SO}_4}}{\mathrm{SO}_4^{2-}}$ Although it has a negative charge, it will never accept ah ${ }^{+}$to form $\mathrm{H}_2 \mathrm{SO}_4$. That is because $\mathrm{H}_2 \mathrm{SO}_4$ is a strong acid and completely dissociates in water. Therefore, the sulfate ion $\left(\mathrm{SO}_4^{-2}\right)$ is the conjugate base of $\mathrm{HSO}_4^{-}$.
AP-EAMCET (Medical)
Ionic Equilibrium
229561
Which one of the following statements is not correct.
1 $\mathrm{Cl}^{-}$is a Lewis acid
2 The $\mathrm{pH}$ of $10^{-8}$ molar $\mathrm{HCl}$ solution is less than 7
3 the ionic product of water at $25^{\circ} \mathrm{C}$ is $10^{-14}$ $\mathrm{mol}^2 \mathrm{~L}^{-2}$
4 Bronsted-Lowry theory could not explain the acidic character of $\mathrm{AlCl}_3$
Explanation:
$\mathrm{Cl}^{-}$is not a Lewis acid. It is a Lewis base. Lewis acid is a chemical species that reacts with a Lewis base to form a Lewis adduct. A Lewis base, then, is any species that donates a pair of electrons to a Lewis acid to form a Lewis adduct. Therefore, $\mathrm{Cl}^{-}$is a Lewis acid statement is not correct.
AP-EAMCET (Medical)
Ionic Equilibrium
229565
The set of amphoteric oxides among the given oxides are $\mathrm{Ga}_2 \mathrm{O}_3, \mathrm{As}_4 \mathrm{O}_{10}, \mathrm{Sb}_4 \mathrm{O}_{10}, \mathrm{~B}_2 \mathrm{O}_3, \mathrm{Tl}_2 \mathrm{O}$
Amphoteric oxides-Metaloxide which react with both basic and acidic oxides to produces salt and water. Ex- $\mathrm{Ga}_2 \mathrm{O}_3, \quad \mathrm{As}_4 \mathrm{O}_{10}, \quad \mathrm{Sb}_4 \mathrm{O}_{10}$ and $\mathrm{Al}_2 \mathrm{O}_3$, all are amphoteric oxides because they react as acid with base and vice-versa.
