Text 21 A
Every chcmical reaction requires some time for its complctiQn, but
some reactions arc very fast and some arc very slow. Reactions between
ions in solution without change in oxidation state arc usually extremely
fast. An example is the neutralization of an acid by a base, which proceeds
as fast as the solutions can be mixed. Presumably nearly every time a
hydronium ion collides with a hydroxide ion reaction occurs, and the
number of collisions is vciy great, so that there is little delay in the reaction.
The formulation of a precipitate, such as that o f silver chloridc when a
solution containing silver ion is mixed with a solution containing chloridc
ion, may require a few scconds, to permit the ions to diffuse together to
form the crystalline grains of the precipitate:
Ag*(aq) + Cl'(aq) -» AgCl(c).
On the other hand, ionic oxidation-rcduction reactions arc sometimes
very slow. An example is the oxidation of a stannous ion by a fcrric ion:
2FC5* + Sn*’ —» 2Fc2* + Sn4\
This reaction docs not occur every time a stannous ion collides with one
or two fcrric ions. In order for a reaction to take place, the collision must be
of such a nature that electrons can be transferred from one ion to another,
and collisions that permit this electron transfer to occur may be rare.
An example of a reaction that is extremely slow at room temperature
is that between hydrogen and oxygen:
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