Chemistry in Aqueous Solution Types of Electrolytes Strong Completely dissociated break into ions Weak Partially dissociate Non No dissociation occurs Examples of Electrolytes Strong Soluble Ionic Compounds ID: 536844
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Slide1
Electrolytes
Chemistry in Aqueous SolutionSlide2
Types of Electrolytes
Strong : Completely dissociated (break into ions)
Weak : Partially dissociate
Non : No dissociation occursSlide3
Examples of Electrolytes
Strong: Soluble Ionic Compounds
NaNO
3
(s)
Na
+
+ NO
3
-
(these are (
aq
))
Weak: Molecular Acids
HC
2
H
3
O
2
(l) H
+
+ C
2
H
3
O
2
-
Non: Molecular Non-acids (alcohols)
CH
3
OH (l) does not dissociateSlide4
Say what you mean!
Three types of equations:
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 dissociationSlide5
Examples of Equations
Molecular:
NaCl
(
aq
)+AgNO
3
(
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 changeSlide6
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.Slide7
Dissolving
Non-electrolyte (no ions)Slide8
Dissociation
Strong electrolyte (all as ions)Slide9
Weak Dissociation
Weak electrolyte (few ions in solution)
Photos courtesy Hal Bender, Clackamas Community College
http://dl.clackamas.edu/ch105-03/examples.htmSlide10
Conductivity
More ions = more conductivity
Non electrolytes = no conductivity
Weak electrolytes = small conductivity
Strong Electrolytes = large conductivity