11C Strong Electrolytes11C Strong Electrolytes.ppt11C Strong Electrolytes.ppt11C Strong Electrolytes.ppt

11C Strong Electrolytes.ppt

1. Strong Electrolytes
Substances that dissociate
completely (100%) when
dissolved in water.

2. An electrolyteis a substance which,
when dissolved in water, results in a
solution that can conduct electricity.
A nonelectrolyteis a
substance which when
dissolved, results in a
solution that does not
conduct electricity.
weakelectrolytestrong electrolyte

3. The concentration of the solutions that contain
electrolytes is referred to as the
analytical concentration or
analytical molarity ( C
SOLUTE )
AND
equilibrium concentration or
equilibrium molarity [ A ]

4. The concentration of aqueous solutions of
electrolytes is the analytical concentration ( C
SOLUTE)
The aqueous solution contains 1.025 mole NaCl in 1.000 L solution .
The solution is labeled as 1.025 M NaCl
The solution was prepared by
dissolving 59.901 g NaCl in
1.000 L of solution.
At equilibrium, the solution contains
1.025 M Na
+
ions and 1.025 M Cl

ions

5. The analytical concentration ( C
SOLUTE)
of electrolytes
The analytical concentration of
the solution is 1.025 M NaCl
C
NaCl
= 1.025 M NaCl
The equilibrium concentration of the
solution is
[Na
+
] = 1.025 M
[Cl

] = 1.025 M
The aqueous solution contains 1.025 mole NaCl in 1.000 L solution .
The solution is labeled as 1.025 M NaCl
AND

6. AQUEOUS SOLUTIONS OF
STRONG ACIDS AND
STRONG BASES

7. Consider an aqueous solution of a
strong acid (HCl, HNO
3, HBr, HI)
[H
+
] = C
SA
pH = -log [H
+
]

8. Consider a 0.120 M HCl solution
[H
+
] = C
SA
pH = -log [H
+
]
[H
+
] = 0.120 M
pH = log 0.120
pH = 0.921

9. ][
][



OH
K
H
W Consider an aqueous solution of a
strong base, MOH
where M belongs to the Group 1 elements
[OH

] = C
SB
pH = log [H
+
]
pOH = log [OH

] OR][
][



OH
K
H
W ][
][



OH
K
H
W
pH = 14.00 pOH

10. Consider a 0.120 M NaOH solution
[OH

] = C
SB
[OH

] = 0.120 M
pOH = log [OH

] pOH = 0.921
pH = 14.00 pOH pH = 13.08

11. Reactions in Aqueous Solutions
Consider the reaction between a 25.00 mL
solution of 0.100 M HCl and 50.00 mL of
0.100 M NaOH.
Instructional Materials (page 15)

12. Consider the reaction between a 25.00 mL solution
of 0.100 M HCl and 50.00 mL of 0.100 M NaOH.
Balanced chemical equation
HCl(aq) + NaOH(aq) NaCl(aq) + H
2O(l)
The number of millimoles of HCl is
The number of millimoles of NaOH is
The limiting reactant/reagent is
The excess reactant/reagent is
2.50 millimoles
5.00 millimoles
HCl
NaOH

13. Consider the reaction between a 25.00 mL solution
of 0.100 M HCl and 50.00 mL of 0.100 M NaOH.
After the reaction, the pH of the resulting
mixture is
less than 7
equal to 7
greater than 7

14. Consider the reaction between a 25.00 mL solution
of 0.100 M HCl and 50.00 mL of 0.100 M NaOH.
After the reaction, the pH of the resulting
mixture is
less than 7
equal to 7
greater than 7