: According to Bronsted Lowry concept bases are the substance which have tendency to accept a proton. $\underset{\text { (acid) }}{\mathrm{H}_2 \mathrm{SO}_4}+\underset{\text { (base) }}{\mathrm{H}_2 \mathrm{O}} \longrightarrow \underset{\begin{array}{c} \text { (Conjugated } \\ \text { acid) } \end{array}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\begin{array}{c} \text { (Conjugated } \\ \text { base) } \end{array}}{\mathrm{HSO}_4^{-}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229703
Which of the following behaves as Lewis acid and not as Bronsted acid?
1 \(\mathrm{HCl}\)
2 \(\mathrm{H}_2 \mathrm{SO}_4\)
3 \(\mathrm{HSO}_3^{-}\)
4 \(\mathrm{SO}_3\)
Explanation:
: Lewis acids have a tendency to accept electron while Bronsted acid have a tendency to donate proton. (a) \(\mathrm{HCl} \rightarrow \mathrm{H}^{+}+\mathrm{Cl}^{-}\) Bronsted acid (c) \(\mathrm{HSO}_3^{-} \rightarrow \mathrm{H}^{+}+\mathrm{SO}_3^{2-}\) Bronsted acid (b) \(\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{H}^{+}+\mathrm{HSO}_4^{-}\) Bronsted acid (d) \(\mathrm{SO}_3+\mathrm{O}^{2-} \rightarrow \mathrm{SO}_4^{2-}\) Lewis acid
UPTU/UPSEE-2009
Ionic Equilibrium
229706
Of the following compounds, which one is the strongest Bronsted acid in a aqueous solution?
1 \(\mathrm{HCIO}_3\)
2 \(\mathrm{HCIO}_2\)
3 \(\mathrm{HOCI}\)
4 \(\mathrm{HOBr}\)
Explanation:
: The central atom in oxoacids, higher oxidation number more strongly it behave bronsted acid. \(\mathrm{HCIO}_3\) \(\begin{aligned} & +1 x+(-2) \times 3=0 \\ & =1+x-6=0 \\ & x-5=0 \\ & x=+5 \end{aligned}\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO}_2 \rightarrow+3\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO} \rightarrow+1\) Oxidation no. for \(\mathrm{Br}\) in \(\mathrm{HBrO} \rightarrow+1\) Hence, \(\mathrm{HClO} 3\) is the strongest Bronsted acid in aqueous solution
WB-JEE-2017
Ionic Equilibrium
229608
Which element from group 15 gives most basic compound with hydrogen?
1 Nitrogen
2 Bismuth
3 Arsenic
4 Phosphorus
Explanation:
Basic character of group 15 hydrides decreases down the group. Thus, $\mathrm{NH}_3$ is most basic and Bismuth is least basic. order of basic strength is$\mathrm{NH}_3>\mathrm{PH}_3>\mathrm{As}>\mathrm{Bi}$
: According to Bronsted Lowry concept bases are the substance which have tendency to accept a proton. $\underset{\text { (acid) }}{\mathrm{H}_2 \mathrm{SO}_4}+\underset{\text { (base) }}{\mathrm{H}_2 \mathrm{O}} \longrightarrow \underset{\begin{array}{c} \text { (Conjugated } \\ \text { acid) } \end{array}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\begin{array}{c} \text { (Conjugated } \\ \text { base) } \end{array}}{\mathrm{HSO}_4^{-}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229703
Which of the following behaves as Lewis acid and not as Bronsted acid?
1 \(\mathrm{HCl}\)
2 \(\mathrm{H}_2 \mathrm{SO}_4\)
3 \(\mathrm{HSO}_3^{-}\)
4 \(\mathrm{SO}_3\)
Explanation:
: Lewis acids have a tendency to accept electron while Bronsted acid have a tendency to donate proton. (a) \(\mathrm{HCl} \rightarrow \mathrm{H}^{+}+\mathrm{Cl}^{-}\) Bronsted acid (c) \(\mathrm{HSO}_3^{-} \rightarrow \mathrm{H}^{+}+\mathrm{SO}_3^{2-}\) Bronsted acid (b) \(\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{H}^{+}+\mathrm{HSO}_4^{-}\) Bronsted acid (d) \(\mathrm{SO}_3+\mathrm{O}^{2-} \rightarrow \mathrm{SO}_4^{2-}\) Lewis acid
UPTU/UPSEE-2009
Ionic Equilibrium
229706
Of the following compounds, which one is the strongest Bronsted acid in a aqueous solution?
1 \(\mathrm{HCIO}_3\)
2 \(\mathrm{HCIO}_2\)
3 \(\mathrm{HOCI}\)
4 \(\mathrm{HOBr}\)
Explanation:
: The central atom in oxoacids, higher oxidation number more strongly it behave bronsted acid. \(\mathrm{HCIO}_3\) \(\begin{aligned} & +1 x+(-2) \times 3=0 \\ & =1+x-6=0 \\ & x-5=0 \\ & x=+5 \end{aligned}\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO}_2 \rightarrow+3\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO} \rightarrow+1\) Oxidation no. for \(\mathrm{Br}\) in \(\mathrm{HBrO} \rightarrow+1\) Hence, \(\mathrm{HClO} 3\) is the strongest Bronsted acid in aqueous solution
WB-JEE-2017
Ionic Equilibrium
229608
Which element from group 15 gives most basic compound with hydrogen?
1 Nitrogen
2 Bismuth
3 Arsenic
4 Phosphorus
Explanation:
Basic character of group 15 hydrides decreases down the group. Thus, $\mathrm{NH}_3$ is most basic and Bismuth is least basic. order of basic strength is$\mathrm{NH}_3>\mathrm{PH}_3>\mathrm{As}>\mathrm{Bi}$
: According to Bronsted Lowry concept bases are the substance which have tendency to accept a proton. $\underset{\text { (acid) }}{\mathrm{H}_2 \mathrm{SO}_4}+\underset{\text { (base) }}{\mathrm{H}_2 \mathrm{O}} \longrightarrow \underset{\begin{array}{c} \text { (Conjugated } \\ \text { acid) } \end{array}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\begin{array}{c} \text { (Conjugated } \\ \text { base) } \end{array}}{\mathrm{HSO}_4^{-}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229703
Which of the following behaves as Lewis acid and not as Bronsted acid?
1 \(\mathrm{HCl}\)
2 \(\mathrm{H}_2 \mathrm{SO}_4\)
3 \(\mathrm{HSO}_3^{-}\)
4 \(\mathrm{SO}_3\)
Explanation:
: Lewis acids have a tendency to accept electron while Bronsted acid have a tendency to donate proton. (a) \(\mathrm{HCl} \rightarrow \mathrm{H}^{+}+\mathrm{Cl}^{-}\) Bronsted acid (c) \(\mathrm{HSO}_3^{-} \rightarrow \mathrm{H}^{+}+\mathrm{SO}_3^{2-}\) Bronsted acid (b) \(\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{H}^{+}+\mathrm{HSO}_4^{-}\) Bronsted acid (d) \(\mathrm{SO}_3+\mathrm{O}^{2-} \rightarrow \mathrm{SO}_4^{2-}\) Lewis acid
UPTU/UPSEE-2009
Ionic Equilibrium
229706
Of the following compounds, which one is the strongest Bronsted acid in a aqueous solution?
1 \(\mathrm{HCIO}_3\)
2 \(\mathrm{HCIO}_2\)
3 \(\mathrm{HOCI}\)
4 \(\mathrm{HOBr}\)
Explanation:
: The central atom in oxoacids, higher oxidation number more strongly it behave bronsted acid. \(\mathrm{HCIO}_3\) \(\begin{aligned} & +1 x+(-2) \times 3=0 \\ & =1+x-6=0 \\ & x-5=0 \\ & x=+5 \end{aligned}\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO}_2 \rightarrow+3\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO} \rightarrow+1\) Oxidation no. for \(\mathrm{Br}\) in \(\mathrm{HBrO} \rightarrow+1\) Hence, \(\mathrm{HClO} 3\) is the strongest Bronsted acid in aqueous solution
WB-JEE-2017
Ionic Equilibrium
229608
Which element from group 15 gives most basic compound with hydrogen?
1 Nitrogen
2 Bismuth
3 Arsenic
4 Phosphorus
Explanation:
Basic character of group 15 hydrides decreases down the group. Thus, $\mathrm{NH}_3$ is most basic and Bismuth is least basic. order of basic strength is$\mathrm{NH}_3>\mathrm{PH}_3>\mathrm{As}>\mathrm{Bi}$
: According to Bronsted Lowry concept bases are the substance which have tendency to accept a proton. $\underset{\text { (acid) }}{\mathrm{H}_2 \mathrm{SO}_4}+\underset{\text { (base) }}{\mathrm{H}_2 \mathrm{O}} \longrightarrow \underset{\begin{array}{c} \text { (Conjugated } \\ \text { acid) } \end{array}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\begin{array}{c} \text { (Conjugated } \\ \text { base) } \end{array}}{\mathrm{HSO}_4^{-}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229703
Which of the following behaves as Lewis acid and not as Bronsted acid?
1 \(\mathrm{HCl}\)
2 \(\mathrm{H}_2 \mathrm{SO}_4\)
3 \(\mathrm{HSO}_3^{-}\)
4 \(\mathrm{SO}_3\)
Explanation:
: Lewis acids have a tendency to accept electron while Bronsted acid have a tendency to donate proton. (a) \(\mathrm{HCl} \rightarrow \mathrm{H}^{+}+\mathrm{Cl}^{-}\) Bronsted acid (c) \(\mathrm{HSO}_3^{-} \rightarrow \mathrm{H}^{+}+\mathrm{SO}_3^{2-}\) Bronsted acid (b) \(\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{H}^{+}+\mathrm{HSO}_4^{-}\) Bronsted acid (d) \(\mathrm{SO}_3+\mathrm{O}^{2-} \rightarrow \mathrm{SO}_4^{2-}\) Lewis acid
UPTU/UPSEE-2009
Ionic Equilibrium
229706
Of the following compounds, which one is the strongest Bronsted acid in a aqueous solution?
1 \(\mathrm{HCIO}_3\)
2 \(\mathrm{HCIO}_2\)
3 \(\mathrm{HOCI}\)
4 \(\mathrm{HOBr}\)
Explanation:
: The central atom in oxoacids, higher oxidation number more strongly it behave bronsted acid. \(\mathrm{HCIO}_3\) \(\begin{aligned} & +1 x+(-2) \times 3=0 \\ & =1+x-6=0 \\ & x-5=0 \\ & x=+5 \end{aligned}\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO}_2 \rightarrow+3\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO} \rightarrow+1\) Oxidation no. for \(\mathrm{Br}\) in \(\mathrm{HBrO} \rightarrow+1\) Hence, \(\mathrm{HClO} 3\) is the strongest Bronsted acid in aqueous solution
WB-JEE-2017
Ionic Equilibrium
229608
Which element from group 15 gives most basic compound with hydrogen?
1 Nitrogen
2 Bismuth
3 Arsenic
4 Phosphorus
Explanation:
Basic character of group 15 hydrides decreases down the group. Thus, $\mathrm{NH}_3$ is most basic and Bismuth is least basic. order of basic strength is$\mathrm{NH}_3>\mathrm{PH}_3>\mathrm{As}>\mathrm{Bi}$
: According to Bronsted Lowry concept bases are the substance which have tendency to accept a proton. $\underset{\text { (acid) }}{\mathrm{H}_2 \mathrm{SO}_4}+\underset{\text { (base) }}{\mathrm{H}_2 \mathrm{O}} \longrightarrow \underset{\begin{array}{c} \text { (Conjugated } \\ \text { acid) } \end{array}}{\mathrm{H}_3 \mathrm{O}^{+}}+\underset{\begin{array}{c} \text { (Conjugated } \\ \text { base) } \end{array}}{\mathrm{HSO}_4^{-}}$
UPTU/UPSEE-2009
Ionic Equilibrium
229703
Which of the following behaves as Lewis acid and not as Bronsted acid?
1 \(\mathrm{HCl}\)
2 \(\mathrm{H}_2 \mathrm{SO}_4\)
3 \(\mathrm{HSO}_3^{-}\)
4 \(\mathrm{SO}_3\)
Explanation:
: Lewis acids have a tendency to accept electron while Bronsted acid have a tendency to donate proton. (a) \(\mathrm{HCl} \rightarrow \mathrm{H}^{+}+\mathrm{Cl}^{-}\) Bronsted acid (c) \(\mathrm{HSO}_3^{-} \rightarrow \mathrm{H}^{+}+\mathrm{SO}_3^{2-}\) Bronsted acid (b) \(\mathrm{H}_2 \mathrm{SO}_4 \rightarrow \mathrm{H}^{+}+\mathrm{HSO}_4^{-}\) Bronsted acid (d) \(\mathrm{SO}_3+\mathrm{O}^{2-} \rightarrow \mathrm{SO}_4^{2-}\) Lewis acid
UPTU/UPSEE-2009
Ionic Equilibrium
229706
Of the following compounds, which one is the strongest Bronsted acid in a aqueous solution?
1 \(\mathrm{HCIO}_3\)
2 \(\mathrm{HCIO}_2\)
3 \(\mathrm{HOCI}\)
4 \(\mathrm{HOBr}\)
Explanation:
: The central atom in oxoacids, higher oxidation number more strongly it behave bronsted acid. \(\mathrm{HCIO}_3\) \(\begin{aligned} & +1 x+(-2) \times 3=0 \\ & =1+x-6=0 \\ & x-5=0 \\ & x=+5 \end{aligned}\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO}_2 \rightarrow+3\) Oxidation no. for \(\mathrm{Cl}\) in \(\mathrm{HClO} \rightarrow+1\) Oxidation no. for \(\mathrm{Br}\) in \(\mathrm{HBrO} \rightarrow+1\) Hence, \(\mathrm{HClO} 3\) is the strongest Bronsted acid in aqueous solution
WB-JEE-2017
Ionic Equilibrium
229608
Which element from group 15 gives most basic compound with hydrogen?
1 Nitrogen
2 Bismuth
3 Arsenic
4 Phosphorus
Explanation:
Basic character of group 15 hydrides decreases down the group. Thus, $\mathrm{NH}_3$ is most basic and Bismuth is least basic. order of basic strength is$\mathrm{NH}_3>\mathrm{PH}_3>\mathrm{As}>\mathrm{Bi}$