Answer
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Step 1:I'll solve this problem step by step, focusing on the acid-base properties of the bicarbonate ion (HCO3).
Step 2:: Identify the Chemical Species
The bicarbonate ion (HCO3) is a polyatomic ion composed of hydrogen (H), carbon (C), and oxygen (O) atoms.
Step 3:: Analyze the Acid-Base Behavior
The bicarbonate ion (HCO3) is an amphoteric species, which means it can act as both an acid and a base depending on the context: - As a base: It can accept a proton (H+) - As an acid: It can donate a proton (H+)
Step 4:: Chemical Equilibrium Reactions
- Base reaction: $$HCO_{3}^{-} + H^{+} \rightarrow H_{2}CO_{3}
- Acid reaction: HCO_{3}^{-} \rightarrow CO_{3}^{2 -} + H^{+}
Step 5:: Acid-Base Classification
The bicarbonate ion is technically a weak base. It's the conjugate base of carbonic acid (H^2CO3).
Final Answer
HCO^3 is an amphoteric ion that primarily behaves as a weak base, capable of both accepting and donating protons depending on the chemical environment.
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