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Bronsted-Lowry acid-base system:

Acid:

According to Bronsted Lowry, acids are substances that donate $H^{+}$(hydrogen ions) or protons. In general, Bronsted-Lowry acid is a proton donor.

Base:

According to Bronsted Lowry, a base is a substance that takes $H^{*}$

(hydrogen ion) or protons. In general, Bronsted Lowry bases are proton acceptors.

$\mathrm{HF}+{\mathrm{NH}}_3→{\mathrm{NH}}_4^{+}+{\mathrm{Cl}}^{-}$

Acid base

Acid-base neutralization:

When an acid reacts with a base to form an ionic salt with water or a solvent, the reaction is known as an acid-base neutralization reaction.

$\mathrm{HCl}\left(aq\right)+\mathrm{KOH}\left(aq\right)→{\mathrm{H}}_2\mathrm{O}\left(l\right)+\mathrm{KCl}\left(aq\right)$

Acid Base Water Salt

a.

In this reaction, $HI$ is the Bronsted Lowry acid, the substance that provides $H^{+}$(hydrogen ion) or proto.

$\mathrm{HI}\left(aq\right)+{\mathrm{H}}_2\mathrm{O}\left(l\right)→{\mathrm{H}}_3{\mathrm{O}}^{+}\left(aq\right)+{\mathrm{I}}^{-}\left(aq\right)$

Acid Base

b.

In this reaction, $H_{2}O$ is the Bronsted Lowry acid, which is the substance that provides $H^{+}$(hydrogen ion) or proto.

localid="1652610794326" $F¯$is a substance that accepts Bronsted Lowry bases, that is, $H^{+}$(hydrogen ions) or protons

${\mathrm{H}}_2\mathrm{O}\left(l\right)+{\mathrm{F}}^{-}\left(aq\right)→\mathrm{HF}\left(aq\right)+{\mathrm{OH}}^{-}\left(aq\right)$

Acid Base