CHEM 112 Lecture Notes - Lecture 15: Lone Pair, Amphoterism, Stoichiometry
Document Summary
Special cases: polyprotic acids: capable of donating more than one photo, amphoteric species: capable of reacting as an acid or base. Ph > 7 is basic: poh = -log[oh-, ph + poh = 14. Kw = [h+][oh-] = 10-14: pka = -log(ka, pkb = -log(kb) Salts: always strong electrolytes, the ph of a salt solution is determined by its aqueous ions, basic: naf, acidic: fecl3, neutral: cabr2, careful with stoichiometry, ca(oh)2. Equilibrium review: ice tables: initial molarity, change in x (molar ratios), equilibrium. Sunday, october 2, 2016: what can we classify h2po4. Amphoteric: goes to h+ + hpo4, also can be: h2po4. + h2o > h3po4 + oh: what can we classify po4. 3- as and why: it"s a base because it can go through base hydrolysis: wants to get protons because it has a -3 charge; since hpo4 the reverse can happen through base hydrolysis. 3-, and is a weak acid: hso4.
