229663
\(\mathrm{NH}_4 \mathrm{Cl}\) is acidic due to
1 Cationic hydrolysis
2 Anionic hydrolysis
3 Its ionic nature
4 \(\mathrm{pH}>7\)
Explanation:
: \(\mathrm{NH}_4 \mathrm{Cl}\) is a salt of strong acid \(\mathrm{HCl}\) and weak base \(\mathrm{NH}_4 \mathrm{OH}\). Hydrolysis:- \(\begin{aligned} & \mathrm{NH}_4 \mathrm{Cl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{HCl} \\ & \mathrm{NH}_4^{+}+\mathrm{Cl}^{-}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{H}^{+}+\mathrm{Cl}^{-} \\ & \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l) \square \quad \mathrm{NH}_4 \mathrm{OH}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \end{aligned}\) Only the cation will undergo hydrolysis and the solution will be acidic in nature due to \(\mathrm{H}^{+}\)formation. So here the cation is responsible for the acidic nature of the solution.
MHT CET-2010
Ionic Equilibrium
229666
If \(20 \mathrm{~mL}\) of an acidic solution of \(\mathrm{pH}=3\) is diluted to \(100 \mathrm{~mL}\), the \(\mathrm{H}^{+}\)ion concentration will be
229668
Which one of the following species acts as both Bronsted acid and base?
1 \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)
2 \(\mathrm{HPO}_3^{2-}\)
3 \(\mathrm{HPO}_4^{2-}\)
4 All of these
Explanation:
: \(\mathrm{HPO}_4^{2-}\) act as both Bronsted acid and bronsted base. \(\begin{array}{ll} \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{H}_2 \mathrm{PO}_4^{-}+\mathrm{OH}^{-} \\ \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{PO}_4^{3-}+\mathrm{H}_3 \mathrm{O}^{+} \end{array}\) \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)is conjugate base of \(\mathrm{H}_3 \mathrm{PO}_2\) (a monobasic acid) and does not give \(\mathrm{H}^{+}\). \(\mathrm{HPO}_3^{2-}\) is a conjugate base of \(\mathrm{H}_2 \mathrm{PO}_3^{-}\)and does not ionize further. \(\mathrm{H}_3 \mathrm{PO}_3\) is a dibasic acid.
UPTU/UPSEE-2015
Ionic Equilibrium
229670
Which of the following is an amphoteric oxide?
1 \(\mathrm{SO}_3\)
2 \(\mathrm{Mg}\)
3 \(\mathrm{Al}_2 \mathrm{O}_3\)
4 \(\mathrm{P}_4 \mathrm{O}_{10}\) МНТ СЕТ -2007
Explanation:
: Amphoteric - These are the oxides that can react with both acids and as well as bases to form salt and water. - These possess both acidic and basic properties. - \(\mathrm{Al}_2 \mathrm{O}_3, \mathrm{SiO}_2\) is an example of Amphoteric oxide - \(\mathrm{Al}_2 \mathrm{O}_3+2 \mathrm{NaOH}\) (Base) \(\rightarrow 2 \mathrm{NaAlO}_2+\mathrm{H}_2 \mathrm{O}\) - \(\mathrm{Al}_2 \mathrm{O}_3+6 \mathrm{HCl}\) (acid) \(\rightarrow 2 \mathrm{AlCl}_3+3 \mathrm{H}_2 \mathrm{O}\)
229663
\(\mathrm{NH}_4 \mathrm{Cl}\) is acidic due to
1 Cationic hydrolysis
2 Anionic hydrolysis
3 Its ionic nature
4 \(\mathrm{pH}>7\)
Explanation:
: \(\mathrm{NH}_4 \mathrm{Cl}\) is a salt of strong acid \(\mathrm{HCl}\) and weak base \(\mathrm{NH}_4 \mathrm{OH}\). Hydrolysis:- \(\begin{aligned} & \mathrm{NH}_4 \mathrm{Cl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{HCl} \\ & \mathrm{NH}_4^{+}+\mathrm{Cl}^{-}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{H}^{+}+\mathrm{Cl}^{-} \\ & \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l) \square \quad \mathrm{NH}_4 \mathrm{OH}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \end{aligned}\) Only the cation will undergo hydrolysis and the solution will be acidic in nature due to \(\mathrm{H}^{+}\)formation. So here the cation is responsible for the acidic nature of the solution.
MHT CET-2010
Ionic Equilibrium
229666
If \(20 \mathrm{~mL}\) of an acidic solution of \(\mathrm{pH}=3\) is diluted to \(100 \mathrm{~mL}\), the \(\mathrm{H}^{+}\)ion concentration will be
229668
Which one of the following species acts as both Bronsted acid and base?
1 \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)
2 \(\mathrm{HPO}_3^{2-}\)
3 \(\mathrm{HPO}_4^{2-}\)
4 All of these
Explanation:
: \(\mathrm{HPO}_4^{2-}\) act as both Bronsted acid and bronsted base. \(\begin{array}{ll} \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{H}_2 \mathrm{PO}_4^{-}+\mathrm{OH}^{-} \\ \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{PO}_4^{3-}+\mathrm{H}_3 \mathrm{O}^{+} \end{array}\) \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)is conjugate base of \(\mathrm{H}_3 \mathrm{PO}_2\) (a monobasic acid) and does not give \(\mathrm{H}^{+}\). \(\mathrm{HPO}_3^{2-}\) is a conjugate base of \(\mathrm{H}_2 \mathrm{PO}_3^{-}\)and does not ionize further. \(\mathrm{H}_3 \mathrm{PO}_3\) is a dibasic acid.
UPTU/UPSEE-2015
Ionic Equilibrium
229670
Which of the following is an amphoteric oxide?
1 \(\mathrm{SO}_3\)
2 \(\mathrm{Mg}\)
3 \(\mathrm{Al}_2 \mathrm{O}_3\)
4 \(\mathrm{P}_4 \mathrm{O}_{10}\) МНТ СЕТ -2007
Explanation:
: Amphoteric - These are the oxides that can react with both acids and as well as bases to form salt and water. - These possess both acidic and basic properties. - \(\mathrm{Al}_2 \mathrm{O}_3, \mathrm{SiO}_2\) is an example of Amphoteric oxide - \(\mathrm{Al}_2 \mathrm{O}_3+2 \mathrm{NaOH}\) (Base) \(\rightarrow 2 \mathrm{NaAlO}_2+\mathrm{H}_2 \mathrm{O}\) - \(\mathrm{Al}_2 \mathrm{O}_3+6 \mathrm{HCl}\) (acid) \(\rightarrow 2 \mathrm{AlCl}_3+3 \mathrm{H}_2 \mathrm{O}\)
229663
\(\mathrm{NH}_4 \mathrm{Cl}\) is acidic due to
1 Cationic hydrolysis
2 Anionic hydrolysis
3 Its ionic nature
4 \(\mathrm{pH}>7\)
Explanation:
: \(\mathrm{NH}_4 \mathrm{Cl}\) is a salt of strong acid \(\mathrm{HCl}\) and weak base \(\mathrm{NH}_4 \mathrm{OH}\). Hydrolysis:- \(\begin{aligned} & \mathrm{NH}_4 \mathrm{Cl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{HCl} \\ & \mathrm{NH}_4^{+}+\mathrm{Cl}^{-}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{H}^{+}+\mathrm{Cl}^{-} \\ & \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l) \square \quad \mathrm{NH}_4 \mathrm{OH}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \end{aligned}\) Only the cation will undergo hydrolysis and the solution will be acidic in nature due to \(\mathrm{H}^{+}\)formation. So here the cation is responsible for the acidic nature of the solution.
MHT CET-2010
Ionic Equilibrium
229666
If \(20 \mathrm{~mL}\) of an acidic solution of \(\mathrm{pH}=3\) is diluted to \(100 \mathrm{~mL}\), the \(\mathrm{H}^{+}\)ion concentration will be
229668
Which one of the following species acts as both Bronsted acid and base?
1 \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)
2 \(\mathrm{HPO}_3^{2-}\)
3 \(\mathrm{HPO}_4^{2-}\)
4 All of these
Explanation:
: \(\mathrm{HPO}_4^{2-}\) act as both Bronsted acid and bronsted base. \(\begin{array}{ll} \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{H}_2 \mathrm{PO}_4^{-}+\mathrm{OH}^{-} \\ \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{PO}_4^{3-}+\mathrm{H}_3 \mathrm{O}^{+} \end{array}\) \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)is conjugate base of \(\mathrm{H}_3 \mathrm{PO}_2\) (a monobasic acid) and does not give \(\mathrm{H}^{+}\). \(\mathrm{HPO}_3^{2-}\) is a conjugate base of \(\mathrm{H}_2 \mathrm{PO}_3^{-}\)and does not ionize further. \(\mathrm{H}_3 \mathrm{PO}_3\) is a dibasic acid.
UPTU/UPSEE-2015
Ionic Equilibrium
229670
Which of the following is an amphoteric oxide?
1 \(\mathrm{SO}_3\)
2 \(\mathrm{Mg}\)
3 \(\mathrm{Al}_2 \mathrm{O}_3\)
4 \(\mathrm{P}_4 \mathrm{O}_{10}\) МНТ СЕТ -2007
Explanation:
: Amphoteric - These are the oxides that can react with both acids and as well as bases to form salt and water. - These possess both acidic and basic properties. - \(\mathrm{Al}_2 \mathrm{O}_3, \mathrm{SiO}_2\) is an example of Amphoteric oxide - \(\mathrm{Al}_2 \mathrm{O}_3+2 \mathrm{NaOH}\) (Base) \(\rightarrow 2 \mathrm{NaAlO}_2+\mathrm{H}_2 \mathrm{O}\) - \(\mathrm{Al}_2 \mathrm{O}_3+6 \mathrm{HCl}\) (acid) \(\rightarrow 2 \mathrm{AlCl}_3+3 \mathrm{H}_2 \mathrm{O}\)
229663
\(\mathrm{NH}_4 \mathrm{Cl}\) is acidic due to
1 Cationic hydrolysis
2 Anionic hydrolysis
3 Its ionic nature
4 \(\mathrm{pH}>7\)
Explanation:
: \(\mathrm{NH}_4 \mathrm{Cl}\) is a salt of strong acid \(\mathrm{HCl}\) and weak base \(\mathrm{NH}_4 \mathrm{OH}\). Hydrolysis:- \(\begin{aligned} & \mathrm{NH}_4 \mathrm{Cl}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{HCl} \\ & \mathrm{NH}_4^{+}+\mathrm{Cl}^{-}+\mathrm{H}_2 \mathrm{O} \square \mathrm{NH}_4 \mathrm{OH}+\mathrm{H}^{+}+\mathrm{Cl}^{-} \\ & \mathrm{NH}_4^{+}(\mathrm{aq})+\mathrm{H}_2 \mathrm{O}(l) \square \quad \mathrm{NH}_4 \mathrm{OH}(\mathrm{aq})+\mathrm{H}^{+}(\mathrm{aq}) \end{aligned}\) Only the cation will undergo hydrolysis and the solution will be acidic in nature due to \(\mathrm{H}^{+}\)formation. So here the cation is responsible for the acidic nature of the solution.
MHT CET-2010
Ionic Equilibrium
229666
If \(20 \mathrm{~mL}\) of an acidic solution of \(\mathrm{pH}=3\) is diluted to \(100 \mathrm{~mL}\), the \(\mathrm{H}^{+}\)ion concentration will be
229668
Which one of the following species acts as both Bronsted acid and base?
1 \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)
2 \(\mathrm{HPO}_3^{2-}\)
3 \(\mathrm{HPO}_4^{2-}\)
4 All of these
Explanation:
: \(\mathrm{HPO}_4^{2-}\) act as both Bronsted acid and bronsted base. \(\begin{array}{ll} \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{H}_2 \mathrm{PO}_4^{-}+\mathrm{OH}^{-} \\ \mathrm{HPO}_4^{2-}+\mathrm{H}_2 \mathrm{O} \square & \mathrm{PO}_4^{3-}+\mathrm{H}_3 \mathrm{O}^{+} \end{array}\) \(\mathrm{H}_2 \mathrm{PO}_2^{-}\)is conjugate base of \(\mathrm{H}_3 \mathrm{PO}_2\) (a monobasic acid) and does not give \(\mathrm{H}^{+}\). \(\mathrm{HPO}_3^{2-}\) is a conjugate base of \(\mathrm{H}_2 \mathrm{PO}_3^{-}\)and does not ionize further. \(\mathrm{H}_3 \mathrm{PO}_3\) is a dibasic acid.
UPTU/UPSEE-2015
Ionic Equilibrium
229670
Which of the following is an amphoteric oxide?
1 \(\mathrm{SO}_3\)
2 \(\mathrm{Mg}\)
3 \(\mathrm{Al}_2 \mathrm{O}_3\)
4 \(\mathrm{P}_4 \mathrm{O}_{10}\) МНТ СЕТ -2007
Explanation:
: Amphoteric - These are the oxides that can react with both acids and as well as bases to form salt and water. - These possess both acidic and basic properties. - \(\mathrm{Al}_2 \mathrm{O}_3, \mathrm{SiO}_2\) is an example of Amphoteric oxide - \(\mathrm{Al}_2 \mathrm{O}_3+2 \mathrm{NaOH}\) (Base) \(\rightarrow 2 \mathrm{NaAlO}_2+\mathrm{H}_2 \mathrm{O}\) - \(\mathrm{Al}_2 \mathrm{O}_3+6 \mathrm{HCl}\) (acid) \(\rightarrow 2 \mathrm{AlCl}_3+3 \mathrm{H}_2 \mathrm{O}\)
