1. Chemistry in Aqueous Solution
Electrolytes
Chemistry in Aqueous Solution

2. Types of Electrolytes
Strong : Completely dissociated (break into ions)
Weak : Partially dissociate
Non : No dissociation occurs

3. Examples of Electrolytes
Strong: Soluble Ionic Compounds
NaNO3 (s)  Na+ + NO3- (these are (aq))
Weak: Molecular Acids
HC2H3O2 (l)  H+ + C2H3O2-
Non: Molecular Non-acids (alcohols)
CH3OH (l)  does not dissociate

4. Say what you mean! Three types of equations: Each is more specific…
Molecular
Ionic
Net ionic
Each is more specific…
Does not specify if they dissociate or not
Specifies which ones dissociate
Specify if an ion changes its dissociation

5. Examples of Equations Molecular: Ionic: which are dissociated?
NaCl(aq)+AgNO3(aq)AgCl(s)+NaNO3(aq)
Ionic: which are dissociated?
Na+ + Cl- + Ag+ + NO3- AgCl(s)+ Na+ + NO3-
Net Ionic: which ones changed?
Cl- + Ag+ AgCl(s)
Spectator ions are removed since they don’t change

6. Dissolve vs. Dissociate
Dissolve means to mix together to become homogenous.
Dissociate means to break apart upon dissolving.
You can dissolve without dissociating (non electrolyte) but…
You CANNOT dissociate without dissolving.

7. Dissolving
Non-electrolyte (no ions)

8. Dissociation
Strong electrolyte (all as ions)

9. Weak Dissociation Weak electrolyte (few ions in solution)
Photos courtesy Hal Bender, Clackamas Community College

10. Conductivity More ions = more conductivity
Non electrolytes = no conductivity
Weak electrolytes = small conductivity
Strong Electrolytes = large conductivity