5 equilibrium and acid base

5 equilibrium and acid base - 2 SO 4 , HI, HBr, HCl, HNO 3...

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Equilibrium Definition of Equilibrium – forward rate = reverse rate Equilibrium constant (mass action ratio) Reaction Quotient Q Result Q<K shift right Q>K shift left Q=K at equilibrium Le Chatelier’s Principle 2C (s) + O 2(s) 2CO (g) Solubility K sp Common Ion Effect Solubility What is the molar solubility of AgCl (K sp = 1.8x10 -10 )? The molar solubility of BiI 3 is 1.32x10 -5 . Calculate K sp . Common Ion Effect What is the molar solubility of AgCl in 0.1M HCl? (K sp = 1.8x10 -10 ) Precipitation To a 0.0001M solution of Mg(NO 3 ) 2 , NaOH was added to a final concentration of 0.001M. Did a precipitate form? (K sp Mg(OH) 2 = 1.6x10 -12 ) K eq Meaning K >> 1 Products favored at eq. K << 1 Reactants favored at eq. K ~ 1 Considerable Prod/React present at eq.
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Acids and Bases Acid Base Arrhenious H + donor in H 2 O OH - donor in H 2 O Bronsted-Lowry H + donor H + acceptor Lewis Electron acceptor Electron donor Conjugate Acid / Base Pairs (Amphoteric substances) Strong acids – HClO 4 , H
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Unformatted text preview: 2 SO 4 , HI, HBr, HCl, HNO 3 , HClO 3 Strong bases- Group 1 metal hydroxides, Ba(OH) 2 , Sr(OH) 2 , Ca(OH) 2 to solubility limit Binary acid trend and oxoacid trends K w and K a K b = K w pH of strong acids pH of weak acids Acid dissociation in water: HA + H 2 O H 3 O + + A-[ ][ ] [ ] HA A O H K a-+ = 3 Base dissociation in water: A-+ H 2 O HA + OH-[ ][ ] [ ]--= A HA OH K b Neutralization rxns Hydrolysis of salts Buffers ] [ ] [ log HA A pK pH a-+ = Titrations Binary acid trend pH, pOH, [H + ], [OH-]; if you know 1 of the 4, you can calculate the other 3. Neutral Conjugate Bases Cl-Br-I-NO 3-ClO 4-ClO 3-Acidic Conjugate Base HSO 4-Almost all other anions are Neutral Cations Li + Na + K + Rb + Cs + Ca 2+ Sr 2+ Ba 2+ All other cations are acidic; the more positively charged, the more acidic....
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5 equilibrium and acid base - 2 SO 4 , HI, HBr, HCl, HNO 3...

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