1. Today’s Objective Predict the products of neutralization reactions.
Acid-Base Chemistry
Tentative Test Date
Monday, April 19th
Today’s Objective
Predict the products of neutralization reactions.

2. Neutralization Reactions
Acid + Base  Salt + Water
Salt = Ionic Compound
Example
HCl + Ca(OH)2  CaCl2 + H2O
Acid
Water
Base
Salt

3. Example #1 Carbonic acid is used to neutralize potassium hydroxide.
H2CO3 2
+ KOH 
K2CO3 2
+ H2O
Most neutralization reactions are double replacement reactions, so the two positive ions switch places!

4. Example #2
Magnesium hydroxide is a common active ingredient in antacids. It can neutralize the excess hydrochloric acid in your stomach.
Mg(OH)2
+ HCl 2 
MgCl2
+ H2O 2

5. Acid-Base Chemistry Tentative Test Date Today’s Objective
Monday, April 19th
Today’s Objective
Determine the relative pH of salts produced in neutralization reactions.
Perform calculations related to titrations.

6. Strong versus Weak Strong Electrolytes Weak Electrolytes
Completely Dissociate
HA  H+ + A-
Partially Dissociate
HA  H+ + A-
Assume you have a strong acid and a weak acid of the same concentration.
Which acid would have a higher concentration of H+ ions?
Which acid would have a lower pH or be more acidic?
The Strong Acid
The Strong Acid

7. List of Strong Acids & Bases
Strong Bases
Hydrochloric Acid (HCl)
Hydrobromic Acid (HBr)
Hydroiodic Acid (HI)
Nitric Acid (HNO3)
Sulfuric Acid (H2SO4)
Perchloric Acid (HClO4)
Group 1A Hydroxides
Example: NaOH
Barium Hydroxide
Ba(OH)2
Strontium Hydroxide
Sr(OH)2
MEMORIZE ME!!

8. Concentrated vs Dilute
Larger Quantities of Solute in a Given Amount of Solvent
Higher Molar Concentrations
Does not depend on whether the solute is strong or weak
Larger Quantities of Solute in a Given Amount of Solvent
Lower Molar Concentrations
Does not depend on whether the solute is strong or weak

9. What’s What?
Looking at the Petri dish models, categorize them as one of the following.
Strong and Concentrated
Strong and Dilute
Weak and Concentrated
Weak and Dilute

10. Salts of Neutralization Reactions
Acid
Base
Salt
Strong
Neutral
Weak
Basic
Acidic
Need More Information

11. Example #1
Write the neutralization reaction that occurs between nitric acid and aluminum hydroxide. Determine if the salt produced will be acidic, basic, neutral, or if more information would be needed. 3 HNO3 + Al(OH)3  Al(NO3)3 + 3 H2O
Strong
Acid
Weak
Base
Acidic
Salt

12. We would need more information!
Example #2
Write the neutralization reaction that occurs between phosphoric acid and calcium hydroxide. Determine if the salt produced will be acidic, basic, neutral, or if more information would be needed. 2 H3PO4 + 3 Ca(OH)2  Ca3(PO4)2 + 6 H2O
Weak
Acid
Weak
Base
????
Salt
We would need more information!

13. Titrations
A titration is a laboratory procedure used for determining the concentration of an unknown solution.
A Buret Filled with the Titrant
An Erlenmeyer Flask with the Analyte
Ring
Stand

14. Example #1
In the prep room, there is a mystery solution of NaOH. Mrs. Stiles wants to determine its concentration, so she titrates a 25.0mL sample of NaOH solution using 0.25M sulfuric acid. If it takes 33.0mL of sulfuric acid to neutralize the base, determine the concentration of the NaOH solution.
Steps to Solve
Write a BALANCED chemical reaction.
Determine the moles of “KNOWN” solution.
Use a molar ratio to determine the moles of “UNKNOWN” solution.
Determine the concentration of the “UNKNOWN” solution.

15. Example # 1 - Continued
H2SO4 + 2 NaOH  Na2SO4 + 2 H2O Moles of “KNOWN” = Moles of Sulfuric Acid mol H2SO4

16. Example #1 - Continued
H2SO4 + 2 NaOH  Na2SO4 + 2 H2O

17. Example #2
A 10.0mL sample of acetic acid is analyzed using calcium hydroxide as the base. If a student used 30.0mL of a 0.15M solution of calcium hydroxide to completely react with the sample of acetic acid, determine the concentration of the acetic acid. 2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O

18. 2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O
Example #2 - Continued
A 10.0mL sample of acetic acid is analyzed using calcium hydroxide as the base. If a student used 30.0mL of a 0.15M solution of calcium hydroxide to completely react with the sample of acetic acid, determine the concentration of the acetic acid.
2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O
mol Ca(OH)2

19. 2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O
Example #2 - Continued
A 10.0mL sample of acetic acid is analyzed using calcium hydroxide as the base. If a student used 30.0mL of a 0.15M solution of calcium hydroxide to completely react with the sample of acetic acid, determine the concentration of the acetic acid.
2 HC2H3O2 + Ca(OH)2  Ca(C2H3O2)2 + 2 H2O