ACIDS, BASES AND BUFFERS 4.5 / 5 based on 2 ratings ? PharmacyChemistryUniversityNone Created by: abcCreated on: 21-12-17 00:34 Molarity M = g/L / g/mol 1 of 16 Normality N = Eq/L 2 of 16 Equivalence Eq = mol x valence 3 of 16 pH of a strong acid pH = -log[H+/H3O+] 4 of 16 pOH of a strong base pOH = -log[OH-] 5 of 16 Degree of ionisation (qualitative) α = [ionised]/([unionised] + [ionised]) 6 of 16 Degree of ionisation of weak acids α (%)=100/((1+〖10〗^(pKa-pH) ) ) 7 of 16 Degree of ionisation of weak bases α (%)=100/((1+〖10〗^(pH-pKa) ) ) 8 of 16 pH of a weak acid pH = 1/2 pKa - 1/2 log[HA] 9 of 16 pH of a weak base pH = 1/2 pKa + 1/2 log[B] + 1/2 pKw 10 of 16 Dissociation of water pKw = pH + pOH = 14 (at 25℃) 11 of 16 Henderson-Hasselbalch equation (pH of acidic buffer) pH = pKa + log([salt] / [acid]) 12 of 16 pH of a basic buffer pH=pKw-pKb+ log〖[Base]/[Salt] 〗 13 of 16 Buffer capacity β=∆B/∆pH 14 of 16 Slyke's equation β = 2.303 × C × (Ka×[H3O+])/(Ka+H3O+ ] )^2 where C is the total buffer concentration 15 of 16 Maximum buffer capacity βmax=0.576C 16 of 16
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