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Chapter 16: Problem 19

(a) The hydrogen carbonate ion \(\left(\mathrm{HCO}_{3}^{-}\right)\) is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water.

Short Answer

Expert verified
When the hydrogen carbonate ion, HCO₃⁻, acts as an acid, it donates a proton (H⁺) to a water molecule, resulting in the formation of a hydronium ion (H₃O⁺) and the carbonate ion (CO₃²⁻): \(HCO_3^- + H_2O \rightarrow H_3O^+ + CO_3^{2-}\) When acting as a base, HCO₃⁻ accepts a proton (H⁺) from a water molecule, forming a hydroxide ion (OH⁻) and carbonic acid (H₂CO₃): \(HCO_3^- + H_2O \rightarrow OH^- + H_2CO_3\)

Step by step solution

01

Write the equation for the hydrogen carbonate ion acting as an acid

When HCO₃⁻ acts as an acid, it donates a proton (H⁺) to a water molecule. This results in the formation of a hydronium ion (H₃O⁺) and the carbonate ion (CO₃²⁻). The balanced chemical equation for this reaction is: \(HCO_3^- + H_2O \rightarrow H_3O^+ + CO_3^{2-}\)
02

Write the equation for the hydrogen carbonate ion acting as a base

When HCO₃⁻ acts as a base, it accepts a proton (H⁺) from a water molecule. This results in the formation of a hydroxide ion (OH⁻) and carbonic acid (H₂CO₃). The balanced chemical equation for this reaction is: \(HCO_3^- + H_2O \rightarrow OH^- + H_2CO_3\) In conclusion, we have demonstrated the amphiprotic behavior of the hydrogen carbonate ion through the two balanced chemical equations presented above.

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Most popular questions from this chapter

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