Question

How can you determine Bronsted-lowry acids and bases?

Answer 1

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_2O + HCl -> H_3O^+ + Cl^-`.

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 `Cl^-` would now accept `H^+` ions, it is called a conjugate base. In the same way, `H_3O^+` would give up the hydrogen ion and so is a conjugate acid.

Conjugate, here, simply means made or rendered.

Answer 2

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 `H2O` can be considered to be both a Bronsted acid and a Bronsted base.

2 `H2O` ==== `H3O+` + OH-