1. Acids & Bases They are everywhere.. In your food In your house EVEN IN YOU!!!!!

2. What is an acid?  An acid is a solution that has an excess of H+ ions. It comes from the Latin word acidus that means "sharp" or "sour".  The more H + ions, the more acidic the solution.

3. Properties of an Acid  Tastes Sour  Conduct Electricity  Corrosive, which means they break down certain substances. Many acids can corrode fabric, skin,and paper  Some acids react strongly with metals  Turns blue litmus paper red Picture from BBC Revision Bites http://www.bbc.co.uk/schools/ks3bitesize/science/chemistry/acids_b ases_1.shtml http://www.bbc.co.uk/schools/ks3bitesize/science/chemistry/acids_b ases_1.shtml

4. Uses of Acids  Acetic Acid = Vinegar  Citric Acid = lemons, limes, & oranges. It is in many sour candies such as lemonhead & sour patch.  Ascorbic acid = Vitamin C which your body needs to function.  Sulfuric acid is used in the production of fertilizers, steel, paints, and plastics.  Car batteries

5. Arrhenius Acids  Arrhenius Acids: increase the concentration of H + (as H 3 O + ) ions in water  H 3 O + is known as the HYDRONIUM ION  Arrhenius Acids are known as proton donors  HCl + H 2 O  H 3 0 + + Cl -

6. What is a base?  A base is a solution that has an excess of OH- ions.  Another word for base is alkali.  Bases are substances that can accept hydrogen ions

7. Properties of a Base  Feel Slippery  Taste Bitter  Corrosive  Can conduct electricity. (Think alkaline batteries.)  Do not react with metals.  Turns red litmus paper blue.

8. Uses of Bases  Bases give soaps, ammonia, and many other cleaning products some of their useful properties.  The OH- ions interact strongly with certain substances, such as dirt and grease.  Chalk and oven cleaner are examples of familiar products that contain bases.  Your blood is a basic solution.

9. Arrhenius Bases  Arrhenius Bases: Produce OH - ions in water  OH - ions are known as HYDROXIDE  Arrhenius Bases are proton acceptors  NH 3 + H 2 O  NH 4 + + OH -

10. Name Game Acids  Oxyacids (acids with Oxygen)  Drop Hydrogen  -Ate becomes ic  -Ite becomes ous  Ex: H 2 SO 4 Sulfuric Acid H 3 PO 3 Phosphorous Acid  Non Oxyacids:  Hydrogen becomes Hydro  -Ide endings become ic  Add acid on the end Bases  No changes to the rules we’ve already learned ;)  Just Remember OH - is hydroxide

11. Weak  In chemistry there are strong and weak bases  Weak acids form conjugate bases  Weak bases form conjugate acids  conjugate means that the acids and bases don’t completely dissociate (Break apart)

12. Strong  Unlike weak acids or bases,  Strong acids and bases completely dissociate in water.  We are ONLY concerned about strong acids and bases for this class

13. Strong Acids and Bases Acids  HI  H + + I -  HBr  H + + Br -  HClO 4  H + + ClO 4 -  HCl  H + + Cl -  HClO 3  H + + ClO 3 -  H 2 SO 4  H + + HSO 4 -  HNO 3  H + + NO 3 - Bases  NaOH  Na + + OH -  KOH  K + + OH -  LiOH  Li + + OH -  RbOH  Rb + + OH -  CsOH  Cs + + OH -  Ca(OH) 2  Ca 2+ +2OH -  Ba(OH) 2  Ba 2+ +2OH -  Sr(OH) 2  Sr 2+ + 2OH -

14. pH Scale  pH is a measure of how acidic or basic a solution is. The pH scale ranges from 0 to 14.  Acidic solutions have pH values below 7  A solution with a pH of 0 is very acidic.  A solution with a pH of 7 is neutral. Pure water has a pH of 7. Basic solutions have pH values above 7.

15. pH Scale A change of 1 pH unit represents a tenfold change in the acidity of the solution. For example, if one solution has a pH of 1 and a second solution has a pH of 2, the first solution is not twice as acidic as the second— it is ten times more acidic.

16. Acid – Base Reactions  A reaction between an acid and a base is called neutralization. An acid-base mixture is not as acidic or basic as the individual starting solutions.

17. Acid – Base reactions  Each salt listed in this table can be formed by the reaction between an acid and a base.