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Unformatted text preview: 2 H 3 O 2that has an acid dissociation constant for HC 2 H 3 O 2 of 1.8 x 105 . Solve this problem by plugging the values into the HendersonHasselbalch equation for a weak acid and its conjugate base. pH = pK a + log ([A]/[HA]) pH = pK a + log ([C 2 H 3 O 2] / [HC 2 H 3 O 2 ]) pH =  log (1.8 x 105 ) + log (0.050 M / 0.20 M) pH =  log (1.8 x 105 ) + log (0.25) pH = 4.7  0.6 pH = 4.1 12. 1. Calculate the concentration of benzoic acid and benzoate in a solution whose pH = 5.2. The pKa of benzoic acid is 4.20 and the solution was prepared to be 0.005 M benzoic acid. pH = pKa + log[A/HA] 5.20 = 4.20 + log[A/HA] 1.0 = log[A/HA] 10 = [A]/[HA] → says the concentration of benzoate is ten times that of benzoic acid or the fractional amount is: [A]/([HA] + [A]) or 1/11 [HA] and 10/11 [A]. The fractional amount of [HA] is: 0.005 M x 1/11 = .0004545 M (4.5 x 104 M) The fractional amount of [A] is: 0.005 M x 10/11 = .004545 M (4.5 x 103 M)...
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 Spring '07
 Petruska,Tower
 Biochemistry, pH, Tabancay

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