1. Electrolytes
Pure water does not conduct electricity. It is the substances dissolved that permit the passage of current. These substances are called “electrolytes”

2. Electrolyte
An electrolyte is a substance that when dissolved in water permits the passage of an electric current

3. Electric conductibility
The electric conductibility of a solution is its capacity to allow the passage of an electric current

4. Different water/Different electrolytes
Ocean water, river water and lake water all have electrolytes with different concentrations.
Many living organisms need electrolytes to survive.

5. Electric dissociation
Electric dissociation is the separation of a dissolved substance into two ions of opposing charges

6. Strength of an electrolyte
The strength of an electrolyte depends on the rate of dissociation. The higher the rate the stronger the electrolyte
(the more ions forming the stronger the electrolyte)
NaCl : very good electrolyte (high dissociation rate)
HF: weak electrolyte (low dissociation rate)

7. Types of electrolytes
Acids, bases and salts are the 3 important types of electrolytes ,

8. Acids
An acid is a substance that release H+ ions in an aqueous solution
(Aqueous solution = water as its solvent)

9. Bases
A base is a substance that releases OH- ions in an aqueous solution

10. Salts
A salt is a substance that provides a bond between a metal ion (+) and a non metal ion (-)

11. pH
The pH is a property that permits to distinguish a solution from acidic, basic or neutral.
We can use an indicator to determine the pH

12. pH scale
The pH scale goes from 0 to 14. It determines the degree of acidity of a substance
pH <  acid
pH > base
pH =  neutral
The pH scale is logarithmic meaning that the difference of 1 unit between two substances is in reality 10 times greater
i.e. A pH of 3 is 10 times more acidic than a pH of 4