Acids And Bases Worksheet - Michalek, Unit 14 Page 14
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27AP Chemsitry--Michalek
14
Unit 14 Acids and Bases
Copy Table 14.6
Notes 14.8
•
Nearly all salts are strong electrolytes.
• Therefore, salts in solution exist entirely of ions.
• Acid-base properties of salts are a consequence of the reactions of their ions in solution.
–
+
•
Many salt ions can react with water to form OH
or H
.
• This process is called hydrolysis.
An Anion’s Ability to React with Water—Salts that product basic solutions
-1
-
O↔ HNO
NaNO
-------- NO
+ H
+ OH
2
2
2
2
–
• Consider an anion, X
, as the conjugate base of an acid.
•
Anions from weak acids are basic.
•
They will cause an increase in pH.
• Anions from strong acids are neutral.
•
They do not cause a change in pH.
–
•
Anions with ionizable protons (e.g., HSO
) are amphiprotic.
4
•
They are capable of acting as an acid or a base.
•
If K
> K
the anion will tend to decrease the pH.
a
b
•
If K
> K
the anion will tend to increase the pH.
b
a
A Cations Ability to React with Water—salts that produce an acidic solution
+1
-
O ↔ NH
NH
Cl--------NH
+ H
+ OH
4
4
2
3
• Polyatomic cations that have one or more ionizable protons are conjugate acids of weak bases.
•
They tend to decrease pH.
•
Metal cations of Group 1A and heavy alkaline earth metals are cations of strong bases and do not alter pH.
•
Other metal ions can cause a decrease in pH.
Example:
-4
Calculate the pH of a 0.30 M NaF solution. The K
value for HF is 7.2 x 10
.
a
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