1. Which is the stronger acid: acetic acid or nitrous acid?
Review:
Which is the stronger acid: acetic acid or nitrous acid?
Which acid, of the same initial Molarity, will produce the greater [H3O+] in aqueous solution: benzoic acid or formic acid?
Will the acetate ion (C2H3O2-) or the nitrite ion (NO2-) be the stronger base?
Try to answer by looking at your response to #1, not the Ka table
Which acid is stronger: H2C2O4 or HC2O4-?
You DO NOT need the Ka table!

2. Acids and Bases

3. The Write-Up Data Table
titration video
The Write-Up
Data Table
Show COMPLETE calculations for 1 complete Trial and the statistical analysis at the bottom of the data table.
Brief concluding statement about the success of the standardization based on the 2 conditions mentioned on the last page.

4. Objectives:
1. Explain how certain salts can produce acidic / alkaline solutions.

5. Remember from yesterday:
Higher K = more products = stronger acid or base
The stronger the acid, the weaker it’s conjugate base will be
YOU MUST KNOW THE 7 STRONG ACIDS!!!

6. The Concept:
Salts can contain ions that are Bronsted-Lowry acids /bases
NH4Cl
in water will ionize into …
Consider (1) how each ion might react with water and the (2) K value for that reaction …

7. Consider (1) how each ion might react with water and the (2) K value for that reaction …

8. Consider (1) how each ion might react with water and the (2) K value for that reaction …

9. Consider (1) how each ion might react with water and the (2) K value for that reaction …
Cation Rules:
1. Alkaline metal and alkaline earth metal cations have no appreciable effect on the pH of a solution
2. NH4+ is a B-L acid and produces an acidic solution
3. +2 or +3 transition metals can function as B-L acids and produce acidic solutions

10. Consider (1) how each ion might react with water and the (2) K value for that reaction …
Anion Rules:
1. Anions that are conjugate bases of strong acids will have no effect on pH. WHY?
Ex: NaCl dissolved in water

11. Acids and Bases

12. Consider (1) how each ion might react with water and the (2) K value for that reaction …
Anion Rules:
1. Anions that are conjugate bases of strong acids will have no effect on pH. WHY?  extremely small Kb value
2. Anions that are conjugate bases of weak acids will produce a basic solution. WHY?
Ex: NaNO2 dissolved in water

13. Consider (1) how each ion might react with water and the (2) K value for that reaction …
Anion Rules:
1. Anions that are conjugate bases of strong acids will have no effect on pH. WHY?  extremely small Kb value
2. Anions that are conjugate bases of weak acids will produce a basic solution. WHY?  larger Kb value
3. Amphoteric anions that can function as acids or bases can produce acidic OR basic solutions, depends on competing Ka and Kb values. Ex: NaHCO3

14. Practice:
Decide whether each of the following salts would give an acidic, basic or neutral aqueous solution
a. NaNO3 b. K3PO4 c. FeCl2
d. NH4F e.NaHCO3

15. Acids and Bases