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Acid-Base Theories Section 20.3

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Salts

Learning Objectives Describe the reaction of an acid with carbonates, bases and alkalis to form a salt Explain that salts are formed, when the H+ of an acid is replaced by the metal or NH+ Explain that a base readily accepts H+ ions (examples include OH- and NH3)

What is an acid? Around 1810 Humphrey Davy discovered that hydrochloric acid is made of only hydrogen and chlorine This led to it being established that hydrogen was common to all acids An early definition of an acid states that they have at least one hydrogen atom that can be replaced by a metal atom

This simple definition can be used to help us establish the reactions of metals and acids, as well as acids with carbonates.

Bronsted-Lowry Theory Stated that an acid is a proton donor and a base is a proton acceptor. For example HCl + NH3 Cl- + NH4+ Note acids and bases can only react in pairs: one acid and one base

when the H+ of an acid is replaced by the metal 1. Mg(s) + 2HCl (aq) ===> MgCl2(aq) + H2(g) when the H+ of an acid is replaced by the NH+ Nitric Acid + Ammonium Hydroxide: HNO3 + NH4OH >>>> NH4NO3 + H2O