How can you determine Bronsted-lowry acids and bases?

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How can you determine Bronsted-lowry acids and bases?

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Answer 1 · 2016-04-09T16:46:33

Bronsted-Lowry acids drop $H^{+}$ $H^+$ ions. Bases pick them up again.

Explanation:

Bronsted-Lowry acids are molecules that lose $H^{+}$ $H^+$ ions. Bases are those that pick them up again.

For example,

$H_{2} O + H C l \to H_{3} O^{+} + C l^{-}$ $H_2O + HCl -> H_3O^+ + Cl^-$ .

In this reaction, hydrochloric acid loses $H^{+}$ $H^+$ , so it is a Bronsted-Lowry acid, while water picks up the $H^{+}$ $H^+$ , so it is a Bronsted-Lowry base.

Because $C l^{-}$ $Cl^-$ would now accept $H^{+}$ $H^+$ ions, it is called a conjugate base. In the same way, $H_{3} O^{+}$ $H_3O^+$ would give up the hydrogen ion and so is a conjugate acid.

Conjugate, here, simply means made or rendered.

Answer 2 · 2016-08-14T01:03:04

A Bronsted acid produces a hydrogen ion $H +$ $H+$ in a reaction While a Bronsted base absorbs a hydrogen ion $H +$ $H+$ in a reaction.

Explanation:

Water $H 2 O$ $H2O$ can be considered to be both a Bronsted acid and a Bronsted base.

2 $H 2 O$ $H2O$ ==== $H 3 O +$ $H3O+$ + OH-

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How can you determine Bronsted-lowry acids and bases?

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