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Identify each of the following species as Bronsted?

A. NH4+
B. Cl-
C. H₂O
D. O₂

User Nageswaran
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1 Answer

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Final answer:

In Bronsted-Lowry theory, NH4+ acts as an acid, Cl- is a very weak base, H2O can be either an acid or base, and O2 is neither typically considered an acid nor a base.

Step-by-step explanation:

To identify whether the species NH₄⁺, Cl⁻, H₂O, and O₂ act as Bronsted-Lowry acids or bases, we look at their ability to donate or accept protons. According to Bronsted-Lowry theory, an acid is a proton donor, whereas a base is a proton acceptor.

  • NH₄⁺ - Ammonium ion is a proton donor, so it is a Bronsted-Lowry acid.
  • Cl⁻ - Chloride ion is typically the conjugate base of HCl, but it is a very weak Bronsted-Lowry base as it can very seldomly accept a proton.
  • H₂O - Water can act as both an acid and a base; it can donate a proton (acid) or accept a proton (base), depending on the reaction.
  • O₂ - Oxygen gas is not typically considered a Bronsted-Lowry acid or base as it does not readily donate or accept protons in its diatomic form.

User Orangecaterpillar
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