# How is a salt prepared?

Sep 3, 2016

Typically this requires the addition of stoichiometric acid to base, or vice versa.

#### Explanation:

$\text{Acid + Base "rarr" Salt + Water}$

For simple strong acid and strong bases:

$H C l \left(a q\right) + N a O H \left(a q\right) \rightarrow N a C l \left(a q\right) + {H}_{2} O \left(a q\right)$

We write the reaction as shown to give the $1 : 1$ equivalence. Sometimes of course, the acid requires more than the $1$ $\text{equiv}$ for neutralization:

${H}_{2} S {O}_{4} \left(a q\right) + 2 N a O H \left(a q\right) \rightarrow N {a}_{2} S {O}_{4} \left(a q\right) + 2 {H}_{2} O \left(a q\right)$.

Both given salts are innocent. A salt such as $\text{sodium acetate}$ or $\text{sodium fluoride}$ may cause water hydrolysis:

${F}^{-} + {H}_{2} O \left(a q\right) r i g h t \le f t h a r p \infty n s H F \left(a q\right) + H {O}^{-}$

i.e. the salts of weak acids compete for the proton in the equilibrium reaction.