# data[].attributes.body
Dissociation - a general process in which ionic compounds separate into smaller ions, usually in a reversible manner.

Dissolution/Dissolving - the process where ionic crystals break up into ions in water.

Hydration/Solvation - the process where ions become surrounded with water molecules, via electrostatic forces.

Electrolyte - a substance that contains free ions, behaving as an electrically conductive medium.

Precipitate - an insoluble solid that forms in a solution during a chemical reaction.

# data[].attributes.body
Electrolytes are chemicals that break into ions (ionize) when they are dissolved in water. The positively-charged ions are cations; the negatively charged ions are anions.

Substances can be categorized as: s trong electrolytes, weak electrolytes, or non-electrolytes.

# data[].attributes.headline
STRONG VS. WEAK ELECTROLYTES AND NON-ELECTROLYTES

# data[].attributes.subject
STRONG VS. WEAK ELECTROLYTES AND NON-ELECTROLYTES

# data[].attributes.body
Strong Electrolytes:

strong acids

HCl
(hydrochloric acid)
HBr
(hydrobromic acid)
HI
(hydroiodic acid)
HNO₃
(nitric acid)
HClO₃
HClO4
H₂SO₄
(sulfuric acid)

strong bases

Group 1 & 2 metal hydroxides:
NaOH
(sodium hydroxide)
KOH
(potassium hydroxide)
LiOH
Ba(OH)₂
Ca(OH)₂

salts

NaCl
KBr
MgCl2

Weak Electrolytes:

weak acids

HF
(hydrofluoric acid),
HC₂H₃O₂
(acetic acid),
H₂CO₃
(carbonic acid),
H₃PO₄
(phosphoric acid)

weak bases

NH₃
(ammonia)
“N” compounds,
eg. C₅H₅N (pyridine)

Non Electrolytes:

sugars and carbohydrate , C₆H₁₂O₆ (glucose)

fats and lipids, cholesterol

alcohols, C₂H₅OH (ethyl alcohol)

other carbon compounds, C₅H₁₂ (pentane)

# data[].attributes.headline
Factors affecting conductivity of electrolytes

# data[].attributes.subject
Factors affecting conductivity of electrolytes

# data[].attributes.body
Concentration of ions (higher conc, higher conductivity)

Type of substance

Temperature (warmer the solution, higher the conductivity)

# data[].attributes.body
Strong electrolytes are substances that completely ionize in water.

This means 100% of the dissolved chemical breaks into cations and anions.

Examples: Strong acids, strong bases, salts. Sodium hydroxide is a strong base and strong electrolyte.

# data[].attributes.body
Weak electrolytes are substances that partially ionize in water.

Any dissociation into ions between 0% and 100% makes a chemical a weak electrolyte, but in practice, around 1% to 10% of a weak electrolyte breaks into ions.

Examples: Weak acids, weak bases, nitrogen-containing molecules.
(Water is considered a weak electrolyte by some sources because it partly dissociates into H⁺ and OH– ions.)

# data[].attributes.headline
SUMMARY: How to identify strong, weak, and non-electrolytes.

# data[].attributes.subject
SUMMARY: How to identify strong, weak, and non-electrolytes.

# data[].attributes.body
1. Is it a strong acid? There are only 7 of them and you’ll encounter them a lot in chemistry, so it’s a good plan to memorize them. Strong acids are strong electrolytes.

2. Is it a strong base? This is a slightly larger group than the strong acids, but you can identify the strong bases because they are metal hydroxides. Any element from the first two columns of the periodic table combined with a hydroxide is a strong base. Strong bases are strong electrolytes.

3. Is it a salt? Salts are strong electrolytes.

4. Does the chemical formula contain nitrogen or “N”? It may be a weak base, which would make it a weak electrolyte.

5. A weak acid is a weak electrolyte.

6. Is it a carbon compound? Most organic compounds are non-electrolytes.

7. Is it none of the above? There’s a good chance it’s a non-electrolyte or a weak electrolyte.

# data[].attributes.body
Examples: Most carbon compounds, fats, sugars, alcohols.

If a substance doesn’t ionize in water at all, it’s a non-electrolyte.

# data[].attributes.headline
TEST FOR ANIONS APPLYING SOLUBILITY RULES - PART 1

# data[].attributes.subject
TEST FOR ANIONS APPLYING SOLUBILITY RULES - PART 1

# data[].attributes.body
esting for:
Cl-        - add silver nitrate solution - white precipitate forms
Br-        - add silver nitrate solution - cream (beige colored) precipitate forms
I-            - add silver nitrate solution - yellow precipitate forms
SO ₄ 2-  - add BaCl 2 solution - white precipitate forms
CO ₃ 2-  - add few drops of acid -  CO ₂ gas is given off
NO ₃-   - add sodium hydroxide aluminium foil, heat it - NH ₃ smell is detected
OH⁻    - add Universal indicator or litmus - indicator turns blue

# data[].attributes.body
Add Ag⁺ or Pb²⁺salt solution to the halide.

A yellow precipitate (ppt) forms.

# data[].attributes.body
VIDEO

# data[].attributes.body
VIDEO

# data[].attributes.body
VIDEO

# data[].attributes.attachment_link.title
Copper carbonate reacts with sulfuric acid

# data[].attributes.body
Hydroxide solutions are all insoluble, as illustrated in video.

# data[].attributes.attachment_link.description
This video is a demonstration of the colour of three metal hydroxide precipitates - copper(II) hydroxide, iron(II) hydroxide and iron(III) hydroxide. Solutions containing copper(II) ions are typically blue in colour. When sodium hydroxide is added, copper(II) hydroxide forms as a blue precipitate. It decomposes to form copper(II) oxide when it is left to stand.

# data[].attributes.headline
DO EXERCISE 2 ON PAGE 15 OF YOUR DIGITAL NOTES

# data[].attributes.subject
DO EXERCISE 2 ON PAGE 15 OF YOUR DIGITAL NOTES

# data[].attributes.body
HOMEWORK FOR NEXT LESSON

# data[].attributes.headline
DO QUESTION 2 ON PAGE 21 of the digital notes on Classroom

# data[].attributes.subject
DO QUESTION 2 ON PAGE 21 of the digital notes on Classroom

# data[].attributes.body
HOMEWORK FOR NEXT LESSON

# data[].attributes.body
ANSWERS TO EXPERIMENT