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# AMPHIPROTIC SPECIES

WHAT ARE AMPHIPROTIC SPECIES?

Note by Abhijeet Verma
2 years ago

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Amphiprotic species are those which can act as both acid and base by accepting or donating proton. For example, $$HSO_{4}^{-}$$ is an amphiprotic species.

• $$\color{red}{HSO_{4}^{-}+H^{+}\rightarrow H_{2}SO_{4}}$$

$$\color{green}{\text{Working as base}}$$

(Although equilibrium constant $$(K_{b})$$ is very small in this reaction, as $$H_{2}SO_{4}$$ is a strong acid.)

• $$\color{red}{HSO_{4}^{-}+OH^{-}\rightarrow SO_{4}^{2-}+H_{2}O}$$

$$\color{green}{\text{Working as acid}}$$

(Equilibrium constant is better in this case, as $$H_{2}SO_{4}$$ is a dibasic strong acid, and it furnishes both $$H^{+}$$ easily) · 2 years ago

Just checked on Google. Both our definitions are correct. These are the species that can donate a proton and can act as both acids and bases. · 2 years ago

They must also be capable of accepting proton · 2 years ago

Well, not necessary. Your statement is true only when talking about Arrhenius acids, but not about the other two types. · 2 years ago

Look up on Wikipedia! Amphoteric behaves as both acids and bases! While amphiprotic are those amphoteric species which do so by accepting and donating H+ · 2 years ago

These species are the name given to those Acids, especially Arrhenius Acids, which are capable of releasing an H(+ve) ion. For example HCl is an amphiprotic acid, as it can readily release an H(+ve) ion. (SO4)2- is not an amphiprotic species, as it does not have an H+ ion to release. · 2 years ago

HCl is not amphiprotic!! · 2 years ago

Are you sure dude? I guess you are mistaking! · 2 years ago

Well, if you are saying that they can act as both acid and bases, then what are amphoteric species like Aluminium oxide and Zinc oxide?? · 2 years ago

Yeah! They are some typical amphoteric species!

$$Al_{2}O_{3}+NaOH\rightarrow NaAlO_{2}+H_{2}O$$ $$Al_{2}O_{3}+HCl \rightarrow AlCl_{3}+H_{2}O$$ · 2 years ago

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