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Electrolytes (Simplified)

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Sections
Solutions
Solubility and Intermolecular Forces
Solutions: Mass Percent
Percent Concentrations
Molarity
Osmolarity
Parts per Million (ppm)
Solubility: Temperature Effect
Intro to Henry's Law
Henry's Law Calculations
Dilutions
Solution Stoichiometry
Electrolytes (Simplified)
Equivalents
Molality
The Colligative Properties
Boiling Point Elevation
Freezing Point Depression
Osmosis
Osmotic Pressure

Electrolytes are compounds that can conduct electricity once they are dissolved in a solvent.

Understanding Electrolytes

Whenever you add a solute to a solvent there are three possible outcomes: the solute dissolves completely, dissolves partially or doesn't dissolve at all into ions.

Concept #1: Strong Electrolytes

Strong Electrolytes break up into ions completely and are grouped into 3 categories: Soluble Ionic Compounds, Strong Acids and Strong Bases.

Example #1: Write a balanced equation for the dissociation of the following strong electrolyte in water: Fe(NO3)3

Concept #2: Weak Electrolytes

Weak Electrolytes partially break up into ions and are grouped into 3 categories: Insoluble Ionic Compounds, Weak Acids and Weak Bases.

Example #2: Benzoic acid, C6H5COOH, is a weak acid. Would you expect benzoic acid solution to contain:

Concept #3: Non-Electrolytes

Non-Electrolytes do NOT break up into ions at all and are commonly referred to as molecular compounds.

Example #3: The dissolution of a compound is given by the reaction below:

Identify each of the following solutions as either electrolytic, weakly electrolytic or non-electrolytic.

Practice: Each of the following reactions depicts a solute dissolving in water. Classify each solute as a strong electrolyte, a weak electrolyte or a non-electrolyte.

Practice: Which of the following represents a non-electrolyte?

a) (CH3)2NH2                             b) NaOH                       c) HIO3                         d) C2H5OH                    e) CsNH2