1. ACIDS AND BASES

2. Chapter 7 Reactions that form water: Acids and Bases Chapter 7 Reactions that form water: Acids and Bases  To learn the key characteristics of the reactions between strong acids and bases  Objective 4: To learn the key characteristics of the reactions between strong acids and bases

3. Properties of Acids  Acids are proton (hydrogen ion, H + ) donors  Acids have a pH lower than 7  Acids taste sour  Acids effect indicators  Blue litmus turns red  Methyl orange turns red  Acids react with active metals, producing H 2  Acids react with carbonates  Acids neutralize bases

4. Acids are Proton (H + ion) Donors Strong acids are assumed to be 100% ionized in solution (good H + donors). Weak acids are usually less than 5% ionized in solution (poor H + donors). HClH 2 SO 4 HNO 3 H 3 PO 4 HC2H3O2HC2H3O2 Organic acids

5. Acids Have a pH less than 7

6. Acids Effect Indicators Blue litmus paper turns red in contact with an acid. Methyl orange turns red with addition of an acid

7. Acids React with Active Metals Acids react with active metals to form salts and hydrogen gas. Mg + 2HCl  MgCl 2 + H 2 (g) Zn + 2HCl  ZnCl 2 + H 2 (g) Mg + H 2 SO 4  MgSO 4 + H 2 (g)

8. Acids React with Carbonates 2HC 2 H 3 O 2 + Na 2 CO 3 2 NaC 2 H 3 O 2 + H 2 O + CO 2

9. Effects of Acid Rain on Marble (calcium carbonate) George Washington: BEFORE George Washington: AFTER

10. Acids Neutralize Bases HCl + NaOH  NaCl + H 2 O Neutralization reactions ALWAYS produce a salt and water. H 2 SO 4 + 2NaOH  Na 2 SO 4 + 2H 2 O 2HNO 3 + Mg(OH) 2  Mg(NO 3 ) 2 + 2H 2 O

11. Properties of Bases  Bases are proton (hydrogen ion, H + ) acceptors  Bases have a pH greater than 7  Bases taste bitter  Bases effect indicators  Red litmus turns blue  Phenolphthalein turns purple  Solutions of bases feel slippery  Bases neutralize acids

12. Bases are Proton (H + ion) Acceptors  Sodium hydroxide (lye), NaOH  Potassium hydroxide, KOH  Magnesium hydroxide, Mg(OH) 2  Calcium hydroxide (lime), Ca(OH) 2 OH - (hydroxide) in base combines with H + in acids to form water H + + OH -  H 2 O

13. Bases have a pH greater than 7

14. Bases Effect Indicators Red litmus paper turns blue in contact with a base. Phenolphthalein turns bright pink in a base.

15. Bases Neutralize Acids Milk of Magnesia contains magnesium hydroxide, Mg(OH) 2, which neutralizes stomach acid, HCl. 2 HCl + Mg(OH) 2 MgCl 2 + 2 H 2 O

16. Mixing Strong Acids and Strong Bases Aqueous hydrochloric acid reacts with aqueous sodium hydroxide HCl(aq) + NaOH(aq)H 2 O(l) + NaCl (aq) Complete ionic equation: H + (aq) + Cl - (aq) + Na+(aq) + OH - (aq)H 2 O(l) + Na + (aq) + Cl - (aq) Net ionic equation: H + (aq) + OH - (aq)H 2 O(l)

17. Mixing Strong Acids and Strong Bases Aqueous hydrobromic acid reacts with aqueous sodium hydroxide HBr(aq) + NaOH(aq)H 2 O(l) + NaBr (aq) Complete ionic equation: H + (aq) + Br - (aq) + Na+(aq) + OH - (aq)H 2 O(l) + Na + (aq) + Br - (aq) Net ionic equation: H + (aq) + OH - (aq)H 2 O(l)

18. Mixing Strong Acids and Strong Bases Aqueous sulfuric acid reacts with aqueous potassium hydroxide H 2 SO 4 (aq) + 2KOH(aq)2H 2 O(l) + K 2 SO 4 (aq) Complete ionic equation: 2H + (aq) + SO 4 2- (aq) + 2K+(aq) + 2OH - (aq) 2H 2 O(l) + 2K + (aq) + SO 4 2- (aq) Net ionic equation: H + (aq) + OH - (aq)H 2 O(l)