1. Your Final Grade 1st Quarter – 20% 2nd Quarter – 20% 3rd Quarter – 20%
4th Quarter - 20%
Final Exam – 20%
(SGM – 15%, Final exam 5%)

2. What’s on the final? Chapter 9 - Stoichiometry
The four types of stoichiometric conversions
Limiting reactant calculations
Chapter 11 – Gas Laws
Combined Gas Law, Ideal Gas Law
You need to know STP and formulas
Acids and Bases notes
You should also know:
Metric prefixes and conversions
Significant figures – identify and calculate using them

3. Preparing for the final
Wednesday– Notes on Acids and Bases
Thursday– Review assignment with sub.
Friday – pH Indicator Lab
Monday – 4th period and 6th period take exam
Tuesday – 5th and 7th period take exam

4. Acids and Bases

5. Definitions:
Acid - a substance that produces hydrogen ions, H+, in an aqueous solution;
Base - a substance that produces hydroxide ions, OH-, in an aqueous solution.

6. Acids Taste sour (do NOT taste a chemical to test this)
React with certain metals (Zn, Fe, Mg, etc.) to produce hydrogen gas
Changes litmus paper red
Conduct electricity
React with bases to form salts and water

7. Bases Taste bitter Feel slippery or soapy Conduct electricity
Changes litmus paper blue
React with acids to form salts and water

8. Monoprotic and polyprotic Acids
Monoprotic acid – can donate only one hydrogen ion per molecule
Diprotic acids – can donate two hydrogen ions per molecule
Triprotic acids – can donate three hyrdrogen ions per molecule

9. Reaction of acids and bases with water:
Acids and bases form ions in solution:
Acids form H+ in aqueous solutions ex: HCl(aq) H+(aq) + Cl-(aq)
Bases form OH- in aqueous solutions
ex: NaOH(aq) Na+(aq) + OH-(aq)

10. Strengths of acids and bases
A strong acid is ionizes completely in aqueous solutions;
A weak acid releases few hydrogen ions in aqueous solutions.
As with acids, the strength of a base depends on the extent to which it dissociates, or adds hydroxide ions, to the solution.

11. Neutralization and Salts
Neutralization - one type of double replacement reaction
Acid + Base Salt + water
example:
HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

12. pH Scale
pH is a measurement of the concentration of hydrogen ions (H+) in the solution.
The pH scale goes from 0 to 14
pH 7 is neutral
Anything less than 7 is acidic, and anything greater than 7 is basic
Common examples:
Tomatoes 4.0 – 4.4
Apples 2.9 – 3.3
Gastric juice 1.0 – 3.0
Blood
Saliva 6.5 – 7.5
Lemons 1.8 – 2.4

13. Some acids are useful in industry
Sulfuric acid (H2SO4)
Most commonly produced industrial chemical in the world.
Used in automobile batteries.
Hydrochloric Acid (HCl)
Produced in stomach to aid in digestion;
Used in multiple industrial processes;
Called muriatic acid in hardware stores.

14. Nitric Acid (HNO3)
This acid has a suffocating odor, stains skin, and can cause serious burns;
Used in making explosives.
Phosphoric Acid (H3PO4)
Mostly used in fertilizer production;
Has a pleasant but sour taste and is not toxic and is used as a flavoring agent
Acetic Acid (CH3COOH)
Vinegar

15. https://All About That Base
Simpsons
Acid Rain