1. DO NOW Pick up notes and small white paper.
Shift and Shout lab due tomorrow.

2. SMALL WHITE PAPER Write your name on the blank side.
List any EOC or AP tests you will be taking in the next two weeks.
SMALL WHITE PAPER

3. Remember: - If you want to go to study hall, you have to tell me by signing the clipboard.

4. THIS WEEK Monday Acid and Base notes Tuesday Acid and Base lab Wednesday Acid and Base notes Thursday Calculating pH Friday Practice
CALENDAR

5. NEXT WEEK Monday Chemistry Exam Review/11th Lit EOC Tuesday Chemistry Exam Review/11th Lit EOC Wednesday Indicator notes Thursday Review for Acid-Base test Tie and soak shirts for Tie Dye Friday Dye shirts lab
CALENDAR

6. Monday Acid and Base test Tuesday Exam Review / US History EOC Wednesday Exam Review Seniors exam – first period Thursday Exam Review Seniors exam – sixth period Friday Honors Program – morning Seventh Period exam
CALENDAR

7. ACIDS AND BASES
UNIT 15

8. ACIDS AND BASES PROPERTIES
A. Taste
Acids taste sour or tart.
Bases (water solutions) taste bitter.
B. Touch
Dilute acids feel like water. Stronger acids are corrosive.
Mild bases feel smooth and slippery. Strong bases are corrosive.
C. Reaction with metals
Acids react vigorously with metals, sometimes producing a gas. Mg + HCl  MgCl2 + H2 (g)
ACIDS AND BASES PROPERTIES

9. ACIDS AND BASES PROPERTIES
D. Reaction with Carbonates/Hydrogen Carbonates
Acids react vigorously with carbonates or hydrogen carbonates, producing a gas.
NaHCO3 + HC2H3O2  Na C2H3O2 + H2O + CO2
E. Electrical conductivity
Pure water is an extremely poor conductor of electricity.
An aqueous solution of a strong acid or base conducts electricity well.
Acids and bases are examples of electrolytes. (Electrolytes ionize when they dissolve in water. A solution containing electrolytes conducts electricity.)
ACIDS AND BASES PROPERTIES

10. ACIDS AND BASES PROPERTIES
F. Indicators
An acid-base indicator is a substance that turns one color in an acidic solution and another color in a basic solution.
Ex. Litmus (acid is red and base is blue), phenolphthalein, methyl red
G. Neutralization
If an acid and a base are mixed together, two new compounds are formed. The properties of the acid and base are destroyed; the acid and base are neutralized. One of the products formed is always an ionic compound and is called a salt. HCl + NaOH  NaCl + H2O
ACIDS AND BASES PROPERTIES

11. Indicating acids and bases
DEMO

12. DEFINING ACIDS AND BASES
To truly understand acids and bases, you must study them at the molecular level.
Acids basically are substances that have more H+ ions than OH- ions.
Bases have the opposite and when something is neutral, it has equal amounts of H+ and OH-.
Usually, acids and bases are dissolved in water; water provides both H+ and OH- ions. Sometimes you will see H3O+ (hydronium ion) instead of H+ (hydrogen ion).
DEFINING ACIDS AND BASES

13. DEFINING ACIDS AND BASES
THE ARRHENIUS DEFINITION:
Acids and bases can be understood in terms of the ions they release when they dissolve in water.
An ACID is a substance that dissociates in water to produce hydrogen ions (H+).
A BASE is a substance that dissociates in water to produce hydroxide ions (OH-).
HCl NaOH  NaCl H2O
H+ + Cl- + Na+ + OH-  Na Cl H2O
DEFINING ACIDS AND BASES

14. DEFINING ACIDS AND BASES
Arrhenius acids include HCl, HNO3, H2SO4, HC2H3O2, H2CO3, and H3PO4.
Arrhenius bases include NaOH, KOH, Mg(OH)2, Ca(OH)2, and Ba(OH)2. Notice they are all hydroxides.
With Arrhenius acids and bases, an acid-base neutralization reaction always produces water and a salt. Metals and acids produce a salt and hydrogen gas.
DEFINING ACIDS AND BASES

15. Defining acids and bases
THE BRØNSTED-LOWRY DEFINITION:
A new definition of acids and bases that is independent of how they act in water and it focuses solely on H+ ions.
Notice that OH- ions are not even addressed. NH3, a base, was not even addressed by Arrhenius’ definition.
An acid is any substance that can donate H+ ions.
A base is any substance that can accept H+ ions.
Defining acids and bases

16. DEFINING ACIDS AND BASES
HCl (g) + H2O (l)  H3O+ (aq) + Cl - (aq)
The hydronium ion is usually formed
from H+ and H2O
DEFINING ACIDS AND BASES

17. HCO HOH  H2CO3 + OH-1
base acid
gain H+ lost H+
ANOTHER EXAMPLE

18. ACIDS WHOSE IONS END IN -IDE Generally, the ion with a suffix of -ide becomes an acid with the prefix hydro- and the suffix -ic . Find the stem of the element that combines with hydrogen. HCl Hydro- chlor -ic acid HBr Hydro- brom -ic acid HCN Hydro- cyan -ic acid
NAMING ACIDS – A Review

19. NAMING ACIDS – A review ACIDS WHOSE IONS END IN “ATE”
Generally, the ion with a suffix of –ate become acids with the suffix, -ic.
H2SO4 Sulfuric acid from sulfate
HNO3 Nitric acid from nitrate
H3PO4 Phosphoric acid from phosphate
NAMING ACIDS – A review

20. ACIDS WHOSE IONS END IN “ITE” Generally, the ion with a suffix of –ite become acids with the suffix, -ous. H2SO3 Sulfurous acid from sulfite HNO2 Nitrous acid from nitrite HClO2 Chlorous acid from chlorite
NAMING ACIDS – A review

21. NAMING ACIDS – A REVIEW Anion _______ide _________ate ___________ite
(chloride, Cl-1) (chlorate, ClO3 -1) (chlorite, ClO2-1)
Acid hydro_____ic acid ________ic acid ________ous acid
hydrochloric acid, HCl chloric acid, HClO3 chlorous acid, HClO2
NAMING ACIDS – A REVIEW

22. TO DO Handout due tomorrow. We are doing a lab tomorrow.
Shift and Shout lab due tomorrow.
TO DO