1. Strong acids are towards 0, weak acids are closer to 7. Strong bases are towards 14, weak bases are closer to 7.

2. Acids and Bases Arrhenius Acids and Bases vIf a compound releases a H + ion when it dissociates it is an acid vIf a compound releases an OH - ion when it dissociates, it is a base HCl H + + Cl - KOH K + + OH -

3. Ammonia (NH 3 ) is a base, but it does not release OH - ions when it dissociates in the same manner as other bases. Instead it takes a H + from water. NH 3 + H 2 O NH 4 + + OH -

4. Acids - donate hydrogen ions Bases - accept hydrogen ions NH 3 + H 2 O NH 4 + + OH - Base Acid

5. NH 3 + H 2 O NH 4 + + OH - In solutions, many reactions can go both ways. Reaction goes to the right Reaction goes to the left

6. NH 3 + H 2 O NH 4 + + OH - When you look at the reaction from left to right, NH 3 is a base because it is accepting a hydrogen, and H 2 O is an acid because it is donating a hydrogen.

7. NH 3 + H 2 O NH 4 + + OH - Reading the reaction from right to left, NH 4 + is an acid because it is donating a hydrogen and OH - is a base because it is accepting a hydrogen. These are conjugate acid - base pairs.

8. Identify the acid/base pairs H 3 PO 4 + NO 2 - HNO 2 + H 2 PO 4 - CN - + HCO 3 - HCN + CO 3 -2 HCN + SO 3 -2 HSO 3 - + CN - H 2 O + HF F - + H 3 O+

9. Acids - Good conductors, taste sour, turn blue litmus red, phenolphthalien clear, pH 0-6.9 Bases - Good Conductors, slippery, turns red litmus blue, phenolphthalien pink, pH 7.1 - 14 Salts - Good conductors, neutral Why are they all good conductors?????

10. Acids begin with H+ Binary Change the H to hydro Change the anion to an –ic endings

11. Polyatomics No hydro Change –ate ending to –ic Change –ite ending to - ous

12. HCl HNO 3 HNO 2 HBr

13. pH is a measure of the concentration of the H + ion. pH = -log [H + ] For example a solution with a H + concentration of 1 x 10 -12 M would have the following pH. pH = -log [1 x 10 -12 ] pH = 12

14. What makes some acids and bases stronger than others? HCl is a strong acid because it dissociates 100%, how strong an acid or base is, is determined by the dissociation constant of that chemical. CH 3 COOH + H 2 O CH 3 COO - + H 3 O + K a = [CH 3 COO - ] [H 3 O + ] [CH3COOH]

15. The higher the dissociation constant, the stronger the acid or base. Weak acids and bases always have a K a for acid, K b for base. Strong acids and bases do not because they dissociate 100%

16. Background information for titrations - page 626 What is a neutralization reaction? What is a titration? What materials are used in a titration and what are they used for? Draw a picture of the set up for a titration. What is the equivalence point? Is the pH really neutralized in this process? Why does the type of indicator used matter?