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Zorluk: OrtaDefinitions and Theories of Acids and Bases

Complete the following statement on acid-base conjugate pairs under the Brønsted-Lowry theory.

Cevap:When the hydrogen carbonate ion (HCO3−HCO_3^-) acts as a Brønsted-Lowry base by accepting a proton, it forms 【carbonic acid】 as its conjugate acid. Conversely, when it acts as a Brønsted-Lowry acid by donating a proton, it forms the 【carbonate】 ion as its conjugate base.

Cevap

The conjugate acid formed when HCO3−HCO_3^- accepts a proton is carbonic acid (H2CO3H_2CO_3), and the conjugate base formed when it donates a proton is the carbonate ion (CO32−CO_3^{2-}).
According to the Brønsted-Lowry theory, an acid is a proton (H+H^+) donor and a base is a proton acceptor. The hydrogen carbonate ion (HCO3−HCO_3^-) is amphiprotic. When acting as a base by accepting H+H^+, it forms its conjugate acid, carbonic acid (H2CO3H_2CO_3). When acting as an acid by donating H+H^+, it leaves behind its conjugate base, the carbonate ion (CO32−CO_3^{2-}).

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1
Identify the species formed when HCO3−HCO_3^- acts as a proton acceptor (base).
According to the Brønsted-Lowry definition, a base accepts a proton (H+H^+). Adding H+H^+ to HCO3−HCO_3^- yields H2CO3H_2CO_3 (carbonic acid).
Accepting a proton increases the number of hydrogen atoms by 1 and raises the net electric charge by +1 (from -1 to 0).
2
Identify the species formed when HCO3−HCO_3^- acts as a proton donor (acid).
According to the Brønsted-Lowry definition, an acid donates a proton (H+H^+). Removing H+H^+ from HCO3−HCO_3^- yields CO32−CO_3^{2-} (carbonate ion).
Donating a proton decreases the number of hydrogen atoms by 1 and reduces the net electric charge by 1 (from -1 to -2).

Anahtar Kavram

Brønsted-Lowry Acid-Base Theory and Amphiprotic Conjugate Pairs
Tahmini Süre:1m 30s
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Definitions and Theories of Acids and Bases

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