# How can you determine Bronsted-lowry acids and bases?

Apr 9, 2016

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

#### Explanation:

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

For example,

${H}_{2} O + H C l \to {H}_{3} {O}^{+} + C {l}^{-}$.

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

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

Conjugate, here, simply means made or rendered.

Aug 14, 2016

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

#### Explanation:

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

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