a new chapter: 17 Acids & Bases The basics: it’s just equilibrium same K expressions, with new names: K a, K b same equilibrium calculations What’s new: the concept of K w p-functions (pH, pK a, pK w ) pH scale

What do you recall about Acid /Base Chemistry?

Acid /Base Chemistry in the Garden Soil Acidity determines Flower color Plant pigments: anthocyanin Anthocyanin, red form Acid form: AH Anthocyanin, blue form Base form, A-

The chemist-gardener: how to make your hydrangeas Pink or Blue Pink form = protonated anthocyanin, acid form AH Need acid: gardeners use ferrous sulfate Reaction:

The chemist-gardener: how to make your hydrangeas Pink or Blue Blue form = deprotonated anthocyanin, base form A- Need base: gardeners use lime Reaction:

The chemist-gardener: how to choose reagents for your garden Think about it: why use ferrous sulfate? why not use HCl? Reaction differences:

Equilibrium Constants in Acid Base Chemistry K a : acid dissociation constant describes how much H+ (H 3 O+) formed General Acid Reaction:

Equilibrium Constants in Acid Base Chemistry K b : base dissociation constant describes how much OH- formed

Equilibrium Constants in Acid Base Chemistry The magnitude of K eq ( so either K a or K b ) determines the strength of acid or base HCl is a strong acid: so K a is very large, K a = 10 8, what is [H 3 O+]? Ferrous ion, Fe(2+) is a weak acid: so K a is small, K a = Now what is [H 3 O+]?

Takes Two to Tango! Acid Base Conjugate Species AH + H 2 OA - + H 3 O+ acid conjugate base conjugate acid

Takes Two to Tango! Acid Base Conjugate Species B + H 2 OBH + + HO- base conjugate acid conjugate base

Takes Two to Tango! Acid Base Conjugate Species B + AHBH + + A- base conjugate acid conjugate base

Dual Personality of Water: both an acid and a base Amphoteric (or amphiprotic) The Autoionization reaction of water. 2 H 2 0 H 3 O+ + OH- K eq =

KwKw Because K w = [H 3 O+][OH-] = and K w is a constant: then When [H 3 O+] = [OH-] = M, the solution is neutral [H 3 O+] [OH-]

KwKw When [H 3 O+] > [OH-], [H 3 O+] > M, the solution is acidic [OH-] < M [H 3 O+] > M

KwKw When [OH-] > [H 3 O+], [OH-] > M, the solution is basic Because K w = [H 3 O+] x [OH-] must be [OH-] > M [H 3 O+] < M

Because all these exponential numbers are a pain: i.e.K w = [H 3 O+][OH-] = [H 3 O+] = [OH-] = M (in neutral water) K a = we will use: The P-Function p of (a number) = -log 10 (a number) so “pH” means p of [H 3 O+], or -log 10 [H 3 O+] so the pH of neutral water, where [H 3 O+] = M is pH 7

The P-Function and K’s p of (K eq ) = -log 10 K eq = pK eq p of (K a ) = -log 10 K a = pK a p of (K w ) = -log 10 K w = pK w Examples: K eq = the pK eq = 10 K a = 1.20 x the pK eq = 4.92 K w = the pK w = 14

The P-Function simplifies exponential numbers K a = 1.20 x 10 -5, pK eq = 4.92 [H 3 O+] = 4.20 x M, pH = [OH-] = 6.66 x M, pOH = ( note number of sig figs) Examples converting from p-function: if pH = 7.47, [H 3 O+] = M= 3.39 x M, if pK a = 4.92, K a = = 1.20 x 10 -5

P-Function simplifies a large range of numbers: graphically [H 3 O+], M pH Note that on a p-scale, the smaller the p-number, the larger the actual number converts to a simpler scale

Apply the P-function to each side p of K w = p of [H 3 O+][OH-] = p of Working in P-Functions can simplify problems Recall K w = [H 3 O+][OH-] = log K w = -log ( [H 3 O+][OH-] )= -log pK w = pH + pOH = 14 -log K w = -log [H 3 O+] + ( -log [OH-] ) = -log

K w = Now apply this equation: pK w = pH + pOH = 14 to this picture [H 3 O+] [OH-]

pK w = 14 Now apply this equation: pK w = pH + pOH = 14 to this picture pH pOH

pK w When the solution is acidic [H 3 O+] > M, pH < 7 : pH is small Because pK w = pH + pOH must be 14 pH < 7 pOH > 7

pK w When the solution is ____________ [H 3 O+] __10 -7 M, pH ___ 7 : pH is ________ pOH is _______ pH is _______ Fill in the blanks!