CHAPTER 14 ACIDS AND BASES

14.1 PROPERTIES OF ACIDS AND BASES

14.1 A practical application of acids and bases. These two flowers are exactly the same genus and species, so why are they different colors?

14.1 A practical application of acids and bases. These two flowers are exactly the same genus and species, so why are they different colors? It is the pH of the soil they are grown in.

14.1 What are some properties of acids?

14.1 What are some properties of acids?  Sour taste (commonly found in foods)  Change the color of pH indicators  Most react with active metals to produce H 2  React with bases to produce water and a salt (neutralization reaction)  Conduct electricity

14.1 Naming acids Binary acids – hydrogen and one other element “hydro_________ic acid” Oxyacids – hydrogen, oxygen, and one other element “per_________ic acid” per -________-ate “_________ic acid” ________-ate “_________ous acid” ________-ite “hypo_________ous acid”hypo_________-ite

14.1 Example 1: Name the following: H 3 PO 4 HBr HClO 3 HClO 2 H 2 SO 4 HC 2 H 3 O 2 or CH 3 COOH HI HNO 3

14.1 Common industrial acids sulfuric – H 2 SO 4 most commonly produced chemical in the world metallurgy, fertilizers, petroleum refining, dehydrating agent, car batteries nitric – HNO 3 explosives, plastics, pharmaceuticals phosphoric – H 3 PO 4 fertilizers, animal feed, flavoring in food, detergents hydrochloric – HCl cleaning metals and masonry, swimming pool acid, stomach acid acetic – CH 3 COOH plastics, food supplements, fungicide carbonic – H 2 CO 3 carbonation in sodas

PH OF SOME COMMON SUBSTANCES

14.1 What are some properties of bases?

14.1 What are some properties of bases?  Taste bitter  Change the color of pH indicators  Feel slippery  React with acids to produce water and a salt  Conduct electricity

14.1 Naming bases Use ionic naming rules for –OH and other ionic bases. Some have common names (NH 3 ).

14.1 Common bases NaOH – oven cleaner, lye CaO – “lime” on lawns, cement, mortar NH 3 - ammonia, cleaner, dissolved in water is NH 4 OH Al(OH) 3, Mg(OH) 2, and NaHCO 3 – antacids NaHCO 3 – baking soda

14.1 What determines a “strong” base or acid?

14.1 The strength of acids and bases is based on how easily they form ions in solution.

14.1 The strength of acids and bases is based on how easily they form ions in solution. When the strong acid ionizes, what is the result? When the weak acid ionizes, what is the result? Why would this be important?

14.1 The strength of acids and bases is based on how easily they form ions in solution. A strong acid forms lots of H 3 O 1+, a weak acid forms few H 3 O 1+ A strong base forms lots of OH 1-, a weak base forms few OH 1- Do not confuse strength with a high concentration. A strong acid could be in a very dilute solution, and a weak acid could be in a very concentrated solution.

14.1 Without counting ions or measuring conductivity, how could strength be determined?

14.1 The arrow holds the key. Strong acid HNO 3 + H 2 O  H 3 O + + NO 3 1- Weak acid HCN + H 2 O  H 3 O + + CN 1- Strong base NaOH  Na + + OH 1- Weak base NH 4 OH  NH OH 1-

14.1 Example 2: Show dissociation of these strong bases and ionization of these strong acids when added to water Mg(OH) 2

14.1 Example 2: Show dissociation of these strong bases and ionization of these strong acids when added to water HClO 3 + H 2 O

14.1 Example 2: Show dissociation of these strong bases and ionization of these strong acids when added to water NaOH

14.1 Example 2: Show dissociation of these strong bases and ionization of these strong acids when added to water H 2 SO 4 + H 2 O

14.1 Example 3: Show ionization of these weak bases and acids when added to water HCN + H 2 O

14.1 Example 3: Show ionization of these weak bases and acids when added to water NH 3 + H 2 O

14.1 Example 3: Show ionization of these weak bases and acids when added to water H 3 PO 4 + H 2 O

14.1 Example 3: Show ionization of these weak bases and acids when added to water HCO H 2 O acting as a base

14.1