contestada

Given the reaction:
HCl(g) + H2O(l) → H3O+(aq) + Cl−(aq)
Which reactant acted as a Bronsted-Lowry acid?
A) H2O(l), because it accepted protons
B) H2O(l), because it produced hydronium ions C) HCl(g), because it donated protons
D) HCl(g), because it reacted with chloride ions

Respuesta :

Answer:

The correct answer is option C.

Explanation:

According to the Bronsted-Lowry conjugate acid-base theory:

  • An acid is defined as a substance which looses donates protons and thus forming conjugate base.
  • A base is defined as a substance which accepts protons and thus forming conjugate acid.

For the given chemical equation:

[tex]HCl(g) + H_2O(l) \rightarrow H_3O^+(aq) + Cl^-(aq)[/tex]

Here, [tex]HCl[/tex] is loosing a proton, thus it is considered as an acid and after losing a proton, it forms [tex]Cl^-[/tex] which is a conjugate base.

And, [tex]H_2O[/tex] is gaining a proton, thus it is considered as a base and after gaining a proton, it forms [tex]H_3O^+[/tex] which is a conjugate acid.

Hence,the correct answer is option C.

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