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Bronsted Lowry Concept Of Acids and Bases
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The Brønsted-Lowry concept defines acids as proton donors and bases as proton acceptors. In this framework, acids donate hydrogen ions (H+) while bases accept them. This definition allows for a broader understanding of acid-base reactions beyond just aqueous solutions, encompassing reactions in va...

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  • April 30, 2024
  • 2
  • 2023/2024
  • Exam (elaborations)
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Subjects

  • lewis acid
  • lewis base
  • conjugate acid base pairs

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  • University of calcutta
  • BOTANY (BOT)
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Bronsted-Lowry Concept Of Acids and Bases

The Brønsted-Lowry concept of acids and bases, proposed independently by
Johannes Nicolaus Brønsted and Thomas Martin Lowry in 1923, is one of the
fundamental theories used to describe and understand acid-base reactions in
chemistry. This concept defines acids and bases in terms of the transfer of
protons (H+ ions) between substances.

According to the Brønsted-Lowry theory:

Acids: Acids are substances that can donate a proton (H+) to another substance. In
other words, an acid is a proton donor. When an acid donates a proton, it forms
its conjugate base.

Example: In the reaction HCl (hydrochloric acid) + H2O (water) → Cl- (chloride ion)
+ H3O+ (hydronium ion), HCl donates a proton to water, making it an acid.

Bases: Bases are substances that can accept a proton (H+) from another
substance. In other words, a base is a proton acceptor. When a base accepts a
proton, it forms its conjugate acid.

Example: In the reaction NH3 (ammonia) + H2O (water) → NH4+ (ammonium ion) +
OH- (hydroxide ion), NH3 accepts a proton from water, making it a base.

Conjugate Acid-Base Pairs: In any Brønsted-Lowry acid-base reaction, there are
always two pairs of substances involved: the acid and its conjugate base, as well
as the base and its conjugate acid. These pairs are related by the transfer of a
proton.

Example: In the reaction HCl + H2O → H3O+ + Cl-, the conjugate acid-base pairs are
HCl/Cl- and H2O/H3O+.

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