Salts

A crystalline compounds composed of the negative ion of an acid and the positive ion of a base.

Neutralization: the reaction of a base and an acid to produce a salt and water.
sodium hydroxide + hydrochloric acid yields sodium chloride + water
While the reaction shown here usually comes to mind when salt production is mentioned, there are many reactions that produce salts. It is even possible to have salts that do not produce neutral solutions.

Salts can also be formed by the reaction of an acidic or basic anhydride with a corresponding base, acid, or anhydride.

* acidic anhydride + base salt
SO3 + 2NaOH Na2SO4 + H2O

* basic anhydride + acid salt
Na2O + H2SO4 Na2SO4 + H2O

* basic anhydride + acidic anhydride salt
Na2O + SO3 Na2SO4

Certain acids and bases react to produce only a partial neutralization. These reactions produce either acidic salts or basic salts.

* This reaction produces an acidic salt:

H2SO4 (aq) + NaOH (aq) NaHSO4 (aq) + H2O (l)

Sodium hydrogen sulfate is an acidic salt because it still contains an ionizable hydrogen atom.

Naming salts:
the name of a salt is related to the name of the acid that forms it.

* Binary acids produce salts ending with ide.
* Ternary acids ending in ic produce salts ending with ate.
* Ternary acids ending in ous produce salts ending with ite.
* Any prefixes in the ternary acid remain in the salt name.
* In naming acidic and basic salts, each ion in the salt is named separately.
o Hydrogen is named immediately before the names of any negative ions.
+ A prefix is used to indicate more than one hydrogen.
o Hydroxide is named immediately after the names of any positive ions.
+ The hydroxide is commonly placed in parenthesis.

material safety data sheets
Examples of Salts:

CaCl2 - calcium chloride
K2SO4 - potassium sulfate
NaHC2O4 - sodium hydrogen oxalate
NaHS - sodium hydrogen sulfide
NaH2PO4 - sodium dihydrogen phosphate
Sn(OH)NO3 - tin (II) hydroxide nitrate