MCQ
Select the set of amphiprotic species?
- A${H_3}{O^ + },HPO_4^{ - 2},HCO_3^ - $
- B${H_2}O,HPO_3^{ - 2},{H_2}PO_2^ - $
- ✓${H_2}PO_4^ - ,{H_2}PO_3^ - ,{H_2}O$
- DAll of these
Amphiprotic species can behave both like an acid and a base. They can donate or accept a proton.
$\underset{\text { Conjugate acid }}{ H _3 PO _4} \stackrel{+ H ^{+}}{\longleftarrow} \underset{\text { Amphiprotic }}{\stackrel{ H _2 PO _4^{-}}{ }} \stackrel{- H ^{+}}{\longrightarrow} \underset{\text { Conjugate base }}{ HPO _4^{2-}}$
$\underset{\text { Conjugate acid }}{ H _3 PO _3} \stackrel{+ H ^{+}}{\longleftarrow} \underset{\text { Amphiprotic }}{ H _2 PO _3^{-}} \stackrel{- H ^{+}}{\longrightarrow} \underset{\text { Conjugate base }}{ HPO _3^{2-}}$
$\underset{\text { Conjugate acid }}{ H _3 O ^{+}} \stackrel{+ H ^{+}}{\longleftarrow} \underset{\text { Amphiprotic }}{ H _2 O} \stackrel{- H ^{+}}{\longrightarrow} \underset{\text { Conjugate base }}{ OH ^{-}}$
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$(A)$ The hypochlorite ion is the strongest conjugate base.
$(B)$ The molecular shape of only chlorate ion is influenced by the lone pair of electrons of $Cl$.
$(C)$ The hypochlorite and chlorate ions disproportionate to give rise to identical set of ions.
$(D)$ The hypochlorite ion oxidizes the sulfite ion.