How Does Hydrogen Donate a Proton with Only One?

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SUMMARY

The discussion centers on the Bronsted-Lowry theory of acids and bases, specifically addressing how hydrogen can act as a proton donor despite having only one proton. It is clarified that in chemical equations, the term "proton" refers specifically to the hydrogen ion (H+), which is indeed the proton donor. The example provided indicates that water (H2O) can also act as a proton donor in certain reactions, demonstrating the role of different substances in proton donation.

PREREQUISITES
  • Understanding of Bronsted-Lowry acid-base theory
  • Basic knowledge of chemical equations and notation
  • Familiarity with the concept of hydrogen ions (H+)
  • Knowledge of water's role in acid-base reactions
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  • Research the Bronsted-Lowry theory in detail
  • Learn about the role of water as an acid and base in chemical reactions
  • Explore examples of proton donation in various chemical reactions
  • Study the properties and behavior of hydrogen ions (H+) in solution
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Chemistry students, educators, and professionals interested in acid-base chemistry and the behavior of protons in chemical reactions.

Witcher
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Homework Statement
I have a question that is more about why and less about how. If i am posting in the wrong section for my question i apologize ahead of time and ask that you direct me to the correct forum.
Relevant Equations
HCO3-(aq) + H2O(l) -> H2CO3(aq) + OH (aq)
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My question for Bronsted Lowry chemical equation is about the donating and accepting electrons. In the bottom chemical equation, the acid is a proton donor. How can hydrogen donate a proton when it has only 1? Or is the subscript the proton in chemical equations
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Witcher said:
...Or is the subscript the proton in chemical equations...
No, the proton is the proton in chemical equations.

In your example, water is the proton donor. Proton cannot be the proton donor, as you have surmised.
 
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