2.   Sour Taste  Electrolytes  Identified by the presence of H + ions (Arrhenius).  Proton (H + ) donor (Bronsted-Lowry).  Common Acids: vinegar, citric acid, sulfuric acid, hydrochloric acid. Acids

3.  An acid  H + in water ACIDS HNO 3, nitric acid HNO 3 HNO 3  H + + NO 3 - Strong acids are strong electrolytes and completely dissociate in water.

4.  An acid  H + in water ACIDS HClhydrochloric HBrhydrobromic HIhydroiodic HNO 3 nitric H 2 SO 4 sulfuric HNO 3 The following are examples of strong acids.

5.  The Hydronium Ion HCl H 2 O H 3 O + Cl - hydronium ion Free H + is highly reactive and does not actually exist in nature. It reacts with water to form the hydronium ion, H 3 O +. HCl (aq)  H 3 O + (aq) + Cl - (aq)

6.  Weak Acids WEAK ACIDS are weak electrolytes and do not completely dissociate in water. CH 3 CO 2 Hacetic acid H 2 CO 3 carbonic acid H 3 PO 4 phosphoric acid Dissociation of a Weak Electrolyte

7.   Bitter taste  Slippery  Like acids, they are electrolytes  Identified by the presence of OH - ions (Arrhenius).  Proton (H + ) acceptor (Bronsted- Lowry). Bases

8. Base  OH - in water BASES NaOH(aq)  Na + (aq) + OH - (aq) NaOH is a strong base Strong bases are strong electrolytes and soluble in water 04m08an1

9.   Based on the concentration of H + or OH - ions in a solution.  Strong Acids/Bases: completely dissociate into ions in a solution.  Weak Acids/Bases: do NOT completely dissociate into ions in a solution. Strength of Acids and Bases

10.  Conjugate Acids/Bases  Acids and bases are related to each other through the addition/loss of hydrogen ions  Conjugate acid-base pairs  Acids produce conjugate bases  Bases produce conjugate acids

11.  Conjugate Examples  HA + H 2 O  H 3 O + + A -  HNO 3 + NH 3  NH 4 + + NO 3 -

12.  Conjugate Acid/Base Strength  Stronger the acid, the weaker the conjugate base  Stronger the base, the weaker the conjugate acid  Weak acids/bases have strong conjugate bases/acids

13.  Strong Acid Example: HCl

14.  Weak Acid Example: CH 3 CO 2 H

15.  “BIG 6”---Strong Acids (Know them!!)  HClO 4  HI  HCl  HNO 3  HBr  H 2 SO 4

16.  Strong Bases (Know them!!)  Group I metal hydroxides (NaOH, KOH, etc.)  Soluble/Slightly soluble Group II metal hydroxides ( Ca(OH) 2, Sr(OH) 2, Ba(OH) 2 )

17.   Binary acids– containing only 2 elements (one is hydrogen)  1) Prefix “hydro—” with binary acid  2) root name for second element  3) End the name with “IC acid”  Oxyacids– acids containing hydrogen, oxygen, and a nonmetal  1) use the given polyatomic ion name from anion  2) add “IC acid” Acid Nomenclature

18.   Write name Example 1: HBr

19.   Write name. Now you try, HCl

20.   Write chemical formula Example 2: Hydrofluoric acid

21.  Now you try, hydriodic acid.

22.   Write the name. Example 3: H 2 SO 4

23.   Write the name. Example 4: HClO 2

24.   HClO 3  HClO  HClO 4 Try:

25.   Name of cation, name of anion/hydroxide  Ex. NaOH Base Nomenclature

26.   Briefly brainstorm how we measure the amount of hydrogen ions in a solution? How can we quickly measure the acidity or basicity of a solution? Brainstorm…