Multiple Choice
As shown by the equations:
H2O + HCO3− ⇆ H3O+ + CO32−
H2O + HCO3− ⇆ H2CO3 + OH−
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17. Acid and Base Equilibrium
Amphoteric Species
Multiple Choice
Which of the following species is/are amphoteric?
A
CO32-
B
HF
C
NH4+
D
HPO32-
E
CH3O-
Verified step by step guidance1
Understand the concept of amphoteric species: Amphoteric species are those that can act as both an acid and a base. This means they can donate a proton (H+) in some reactions and accept a proton in others.
Analyze each given species to determine if it can act as both an acid and a base. Start with CO3^{2-}: This ion is the conjugate base of HCO3^{-}, and it can accept a proton to form HCO3^{-}, but it does not typically donate a proton, so it is not amphoteric.
Consider HF: Hydrofluoric acid can donate a proton to form F^{-}, but it does not typically accept a proton to form H2F^{+}, so it is not amphoteric.
Evaluate NH4^{+}: This ion can donate a proton to form NH3, but it does not accept a proton to form NH5^{+}, so it is not amphoteric.
Examine HPO3^{2-}: This ion can donate a proton to form PO3^{3-} and can also accept a proton to form H2PO3^{-}, making it amphoteric. Finally, consider CH3O^{-}: This ion can accept a proton to form CH3OH, but it does not donate a proton, so it is not amphoteric.
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