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Unformatted text preview: Chapter 16 I. Binary Acids a. HX (partial charge) b. Strong acids i. X is strongly electronegative ii. Bond is weak c. Weak Acids i. Low electronegativity ii. Bond too strong II. Oxoacids a. Acid strength increases with # of O atoms i. Because electronegativity increases III. pH (strong acid/base calculation) a. –log[H 3 O + ] = pH b. –log[OH- ] = pOH c. pH + pOH = 14 d. 10-pH = [H 3 O + ] IV.Weak acid calculations a. HA + H 2 O ↔ H 3 O + + A- , K c b. K c = K a c. K a = acid ionization constant of HA d. K a = [H 3 O + ][A- ]/[HA] e. K a of strong acids = LARGE f. K a of H 3 O + = 1 g. K a of weak acids = small i. K a of H 2 O = 10-14 V. Ionization of weak acids, bases a. HA + H 2 O ↔ H 3 O + + A- , K a b. A- + H 2 O ↔ HA + OH- , K b c. 2H 2 O ↔ H 3 O + + OH- , K w i. K a of HA and K b of A- are inversely proportional d. BIKE i. Balanced equation ii. ICE table iii. K equation (need to know equilibrium constant) iv. Equilibrium constant expression/calculation 1. Approx if 100<[HA] /K a VI.Ionization of weak bases a. NH 3 + H 2 O ↔ NH 4 + + OH- , K b of NH 3 VII. Acidic and Basic Ions in Water a. NH 4 Cl or Na 3 PO 4 in water b. Must find active species i. Find ions present ii. NH 4 + Cl- 1. NH 4 + = active species c. Bronsted Lowry equation...
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