Compare and contrast weak bases and strong bases.

A base is a chemical species that accepts protons, donates electrons or releases hydroxide
ions while dissolved in water. The resulting aqueous solution thence reacts with an acid to form a
salt. Bases have a pH of above 7, and turn litmus paper blue. Strong and weak bases have been
compared and contrasted, by a number of properties discussed in this essay.
Weak and strong bases:
All bases release the hydroxide ion (OH-) ions while dissolved in water according to the
Arrhenius Concept of bases, albeit to different extents. The concentration of the resulting OH-
ions is used to define the strength of a base. Strong bases dissociate totally in water, ionizing
completely (into metal and hydroxide ions) while in aqueous solutions, having pH values closer
to 14. This also makes them good conductors of electricity. Examples of strong bases include
sodium hydroxide, potassium hydroxide and calcium hydroxide. Weak bases, on the other hand,
dissociate partially in aqueous form, and their deficient ions also make them poor electricity
conductors. The pH values are of the range of 7 to10. The dissociation reaction for weak bases is
represented by double half arrows in a chemical reaction. Examples of weak bases include
methylamine and glycine. Strong bases have higher base dissociation constant (K b ) compared to
the weak bases, from their less complete dissociation in aqueous state. The p K b values are
around 0 for strong bases, but very high for the weak bases. The higher concentration of
electrolytes in solution following the dissociation of strong bases make them more reactive
compared to weak bases.
Conclusion:
Bases are defined by their properties of accepting protons, donating electrons and
releasing OH- ions while in aqueous states. The distinction between strong and weak bases is
brought about by the difference in their extent of dissociation, which affects the pH, conduction
of electricity and reactivity in chemical reactions.

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