2. Acids Comes from Latin word acere meaning sour Sour taste Reacts w/ metals to produce hydrogen gas Turns blue litmus red Neutralizes bases Conducts electric current Bitter taste Turns red litmus blue Neutralizes acids Conducts electric current Feels slippery ( dissolve fatty acids & oils from skin reducing friction Bases

3. Strong Acids Ionize completely, weak acids do not Ex. HCl HNO 3 H 2 SO 4 Dissociates completely, weak bases do not Ex. NaOH Ca(OH) 2 Strong Bases

4. Arrhenius Acids contain the hydrogen ion or hydronium ion Ex. HCl, H 2 SO 4 Bases contain the hydroxide ion Ex. NaOH, Ca(OH) 2 Exception ammonia, NH 3

5. Bronsted-Lowry Acids donate a hydrogen ion to another substance Bases are substances that accept hydrogen ion from another substance Conjugate acid is the substance formed Conjugate base is the substance that remains Water is amphiprotic because it can act as an acid or a base Used to explain neutralization reactions Accounts for ammonia where Arrhenius does not Ex. H 2 O(l) + NH 3 (g)  NH 4 + (aq) + OH - (aq) acidbase C.A. C.B.

6. Lewis Acids are electron pair acceptors Bases are electron pair donors Explains the formation of complex ions Ex. NH 3 (g) + BCl 3 (aq)  NH 3 BCl 3 (aq) base acid

7. Substance that is one color in an acid & another in a base Common Indicators AcidBase Phenolphthaleincolorlessred Methyl Orangeredyellow Bromothymol blueyellowblue

8. Number derived from hydronium ions in solution [H 3 O + ] increases, pH decreases [H 3 O + ] decreases, pH increases pH meter more accurate than pH paper Scale Range: 1 - 6 acidic 7 neutral 8 – 14 basic

9. pH = - log [H 3 O + ] pOH = - log [OH - ] pH + pOH = 14 [H 3 O + ] x[OH - ]=1 x 10 -14 M 2 Ex. What is pH of a 0.01M nitric acid solution? Answer: pH = 2 Ex. What is [H 3 O + ] of a solution that has a pH = 9? Answer: [H 3 O + ] = 1 x 10 -9 M

10. Reaction of H 3 O + in an acid and OH - in a base to produce salt and water Titration can be used to neutralize a known solution having a known concentration with an unknown concentration of another solution Endpoint of titration found w/ indicator (may have excess acid or base) Equivalence point of titration using pH readings w/ pH meter (no excess acid or base)

11. Step 1: Calculate the number of moles of base used to titrate the acid Step 2: Determine the acid to base ratio from the chemical equation & calculate the number of moles of acid used Step 3: Use the volume of the acid & number of moles of acid to calculate the acid’s molarity

12. Allows for maintenance of fairly narrow range of pH even while another reaction is producing acids or bases Mixture of weak acid & its conjugate base or weak base & its conjugate acid Can react w/ either acid/base to remove acid or base from solution Used to keep fairly constant pH while acids/bases are added to solution be reaction Real life buffers include controlling blood pH and urine pH

13. Acidic anhydrides Formed when nonmetal oxide reacts w/ water to form an acid Burning of fossil fuels produces CO & SO 2 that combine w/ water in atmosphere to form acid rain S+O 2  SO 2 SO 2 + O 2  SO 3 SO 3 + H 2 O  H 2 SO 4 or SO 2 + H 2 O  H 2 SO 4

14. Decomposition of marble statues Lowered pH in Adirondak lakes to point they can no longer support wildlife Causes crops to grow more slowly & forests to thin out

17. Formed when metal oxide reacts w/ water to form a base Ex. Calcium oxide added to water produces calcium hydroxide a.k.a slaked lime Used to counteract acid rain damage Used in scrubbing stack gases to remove SO 2 from exhaust of power plants & factories Ca(OH) 2 + H 2 SO 4  CaSO 3 + 2H 2 O (this in large amounts is a disposal problem; buried in landfills)