1. Dissolving an Ionic Electrolyte

2. Stationary ions can NOT
Dissolving an Ionic Electrolyte
The dissolving of an ionic electrolyte.
All salts are ionic electrolytes!
Hydroxide bases are ionic electrolytes! + ― + ―
Stationary ions can NOT
conduct electricity
Free moving ions can
conduct electricity

3. Dissolving an Ionic Electrolyte
Ex. (1) Write the dissolving reaction for each of the following ionic electrolytes.
NaCl(s) → _____________________________
BaCl2(s) → ____________________________
Sr(OH)2(s) → __________________________ +1 -1 1+ 1- 1
H2O 1 Na + 1 Cl
(aq)
(aq) +2 -1 2+
H2O 1- 1 1 Ba + 2 Cl
(aq)
(aq) +2 -1
H2O 2+ 1- 1 1 Sr + 2 OH
(aq)
(aq)

4. Dissolving an Ionic Electrolyte
Mg(NO3)2(s) → __________________________
Na2CO3(s) → ___________________________
KOH(s) → ______________________________ +2 -1 2+
H2O 1- 1 1 Mg + 2
NO3
(aq)
(aq) +1 -2 2-
H2O 1+ 2 Na + 1 1
CO3
(aq)
(aq) +1 -1 1-
H2O 1+ 1 1 K + 1 OH
(aq)
(aq)

5. Dissolving an Ionic Electrolyte
Ex. (2) Which of the following sodium chloride samples is incapable of conducting electricity?
(1) NaCl(s) (3) NaCl(aq) (2) NaCl(l) (4) NaCl(g)
Ionic electrolytes will conduct electricity NOT only in the aqueous phase BUT also in the liquid and gases phases because the ions are free to move around!