Warmup Put the following descriptors in the correct spaces on the Venn diagram…

Taste Bitter Taste Sour pH of 0-6.9 pH of 7.1-14 Start with “H” End with “OH” Milk Vinegar Feel slippery Is an electrolyte Turns litmus paper pink Ammonia Lemon Juice Detergent Turns litmus paper blue Can harm skin and tissue

Ch. 15 & 16 - Acids & Bases II. pH (p. 481 - 491)

H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0  10-14M2 A. Ionization of Water H2O + H2O H3O+ + OH- Kw = [H3O+][OH-] = 1.0  10-14M2

A. Ionization of Water Find the hydroxide ion concentration of 1.0  10-2 M HCl. [H3O+][OH-] = 1.0  10-14M2 [1.0  10-2][OH-] = 1.0  10-14M2 [OH-] = 1.0  10-12 M

Compare your exponents for [H3O+] and [OH-] A. Ionization of Water How to tell if a solution is acidic or basic: Compare your exponents for [H3O+] and [OH-] Whichever has the smallest number for the exponent is MORE concentrated [H3O+] =1.0  10-2 M [OH-] = 1.0  10-12 M Acidic or basic? Acidic

pouvoir hydrogène (Fr.) B. pH Scale 14 7 INCREASING ACIDITY INCREASING BASICITY NEUTRAL pH = -log[H3O+] pouvoir hydrogène (Fr.) “hydrogen power”

pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14 B. pH Scale pH = -log[H3O+] pOH = -log[OH-] pH + pOH = 14

B. pH Scale What is the pH of 0.050 M HNO3? pH = -log[H3O+] Acidic or basic? Acidic

B. pH Scale What is the molarity of HBr in a solution that has a pOH of 9.6? pH + pOH = 14 pH + 9.6 = 14 pH = 4.4 pH = -log[H3O+] 4.4 = -log[H3O+] -4.4 = log[H3O+] [H3O+] = 4.0  10-5 M HBr Acidic