Guide
1
The essence of this theory is that the melt (dissolves in water) virtually all electrolytes decomposed into ions, which are both positively and negatively charged (which is called electrolytic dissociation).Under the influence of an electrical current negative (anions "-") move toward the anode (+) and positively charged (cations, "+") move towards the cathode (-).Electrolytic dissociation - is reversible (the reverse process is called "molarization").
2
Degree (a) electrolytic dissociation depends on the nature of the electrolyte solvent and their concentration.This ratio of the number of molecules (n), which are broken up to the total number of ions introduced to the solution of molecules (N).You get: a = n / N
3
Thus, strong electrolytes - substa
nces completely dissociate into ions when dissolved in water.By strong electrolytes typically include substances with strongly polar or ionic bonds: the salts which are readily soluble, strong acids (HCl, HI, HBr, HClO4, HNO3, H2SO4), and a strong base (KOH, NaOH, RbOH, Ba(OH) 2, CsOH, Sr (OH) 2, LiOH, Ca (OH) 2).The strong electrolyte substance dissolved in it is mostly in the form of ions (anions and cations);molecules that undissociated - practically no.
4
weak electrolytes - such substances, which dissociate into ions only partially.Weak electrolytes together with ions in solution contain undissociated molecules.Weak electrolytes do not give a strong concentration in the solution of ions.

Weaknesses include:
- organic acids (almost all) (C2H5COOH, CH3COOH and so on.);
- some of the inorganic acid (H2S, H2CO3 etc.);
- practically all salts, sparingly soluble in water, ammonium hydroxide, and any base (Ca3 (PO4) 2; Cu (OH) 2; Al (OH) 3; NH4OH);
- water.

They practically do not conduct electricity, or conduct, but bad.