Definition and Process of Electrolytes and Non-Electrolytes

Definition and Process of Electrolytes and Non-Electrolytes
Electrolytes and Non-Electrolytes - Definition, History, Process, Strength, Weakness, Compounds, Example: A solution is a homogeneous mixture of two or more substances that dissolve themselves and each of the constituent substances cannot be physically edited again.

Definition of Solution
Solution is a homogeneous mixture of two or more substances which dissolve themselves and each of the constituent substances cannot be physically edited again. The solution consists of solvents and solutes. Based on the electrical conductivity (ionisation power), the solution is divided into 2 types, namely electrolyte and non-electrolyte solutions.

History of electrolyte and non-electrolyte solutions
In 1884, Svante Arrhenius, a famous chemist from Sweden put forward the theory of electrolytes which until now the theory persisted even though he was barely given his doctorate at Upsala University, Sweden, for expressing this theory.
According to Arrhenius, the electrolyte solution in water dissociates into positive and negative electrically charged particles called ions (positive ions and negative ions). The number of positive ion charges will equal the number of negative ion charges, so the charge of the ions in the neutral solution. These ions are in charge of delivering an electric current. Solutions that can conduct electric current are called electrolyte solutions.
This solution gives symptoms in the form of lights or the emergence of gas bubbles in the solution. Electrolyte solutions contain charged particles (cations and anions). Based on experiments conducted by Michael Faraday, it is known that if an electric current is flowed into an electrolyte solution an electrolysis process will occur which produces gas.
This gas bubble is formed because positive ions undergo a reduction reaction and negative ions undergo oxidation. For example, in the HCl solution an electrolysis reaction occurs which produces hydrogen gas as follows.
HCl (aq) → H + (aq) + Cl- (aq)
Reduction reaction: 2H + (aq) + 2e- → H2 (g)
Oxidation reaction: 2Cl- (aq) → Cl2 (g) + 2e-

Understanding Electrolytes
Electrolytes are dissolved or dissolved substances in the form of ions and then the solution becomes an electrical conductor, ions are electrically charged atoms. Electrolyte substances can be acids, bases, water or can also be other chemical compounds. Electrolytes are generally in the form of acids, salts or bases. This solution is subdivided into 2, namely: strong electrolytes and weak electrolytes.

Strong electrolytes
Strong electrolyte solutions are solutions that have a strong electrical conductivity, because the solutes in solvents (generally water), all turn into ions (α = 1).

Classified as strong electrolytes are:
Strong acids, such as: HCl, HCl03, H2SO4, HNO3 and others.
Strong bases, namely alkaline and alkaline earth bases, such as: NaOH, KOH, Ca (OH) 2, Ba (OH) 2 and others.
Salts that dissolve easily, such as: NaCl, KI, Al2 (SO4) 3 and others
Example :
Acids, for example sulfuric acid (H2SO4), nitric acid (HNO3), hydrochloric acid (HCl)
Bases, for example sodium hydroxide (NaOH), potassium hydroxide (KOH), barium hydroxide (Ba (OH) 2)
Weak electrolytes
Weak electrolyte solution is a solution with low electrical conductivity with a value of the degree of ionization of: O <α <1.