Acid and Base

Acids and Bases Intro and Review

Theories:

Arrhenius Theory
-first theory concerning acids and bases
-all acids conduct rise hydrogen ions (H+) in weewee

e.g.

-all bases produce hydrated oxide ions (OH-1)in water
-acid-base neutralization is simply the combination of hydrogen ions with hydroxide ions to produce water

e.g.

Today we know that hydrogen ions solely come through in water when they are attached to something else.
When they attach themselves to water molecules they form hydronium ions (H3O+).

Lewis diagram:




Non-metal oxides
-called acidic anhydrides (anhydride means without water)
-these controvert with water to form molecular acids breaking H+

E.g. SO3(g) + H2O(l) ( H2SO4(aq)

Note: H2CO3 is overly unstable to be isolated as a fresh compound. CO is not an acidic anhydride.

Bases:
Two categories 1) Ionic compounds that contain hydroxide ions or O2-
2) Molecular compounds that react with water to give hydroxide ions

Bronsted-Lowry Theory of Acids and Bases
-acids are proton donors
-bases are proton acceptors
-acid-base reactions involve an proton careen from acid to base
-involves conjugate acid-base pairs

e.g.



NH3and CH3COOH



Note: Conjugate acid-base pairs differ by one proton and a charge of 1

Amphoteric/Amphiprotic
-a substance able-bodied of reacting as an acid or a base
-water in the higher up examples is amphoteric
-another example is HCO3-1 which is part of the buffer system in our blood




Polyprotic Acids
-acids that watch more than one ionisable hydrogen

e.g. H2SO4 is an example of a diprotic acid


Strong and asthenic Acids and Bases
-strong acids and bases complete react with water to release all of their hydrogen or hydroxide ions
-weak acids and bases only partially ionize/ separate and thus form equilibrium systems and have equilibrium constants associated with them
-since at that place are a lot more weak acids and bases, we only need to memorize the strong ones

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