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3. Alkalinity is related to the buffering capacity of an aqueous solution containing an acid and its conjugate base which can be understood using the Henderson-Hasselbalch equation, as follows. pH pKa log [base/[acid] where Ka is the acid dissociation constant. Calculate the pH of a buffer solution that is 0.050 M in benzoic acid (C6HsCOOH) and 0.150 M in sodium benzoate (CsHsCOONa). Note: Ka (benzoic acid) 6.5 x10. Outline any assumptions or simplifications in your calculation. What will happen to the final pH of the benzoic acid/benzoate solution if Fe2+ (aq) is added and complex formation occurs according to reaction [3]? The value of the formation constant is as follows: Kf (Fe(CeHsCO0)2)- 1.5x1010 K, Fe2 (aq)CHsCOO (aq)Fe2+ (CHscoo)2 (aq) 13] Explain the difference in pH due to the presence of Fe2+ species without doing a pH calculation How does the distribution of Fe2* species (aq, uncomplexed) compare with the (Fe(CHsCO0)2) (aq) in a pond containing sediment. Use the soil-water partition coefficient to explain your answKere C, is the concentration in the sediment and Cw is the concentration in the water phase.

Q1: Explain the difference in pH due to the presence of Fe2+ species without doing a pH calculation.
Q2: How does the distribution of Fe2+ species (aq, uncomplexed) compare with the (Fe(C6H5COO)2) (aq) in a pond containing sediment? Use the soil-water partition coefficient to explain your answer: ?? =??/?? where Cs is the concentration in the sediment and Cw is the concentration in the water phase.

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1.05 ic Aci d it forms a shong Camplux and it witl rather Catch u ep f e medir e ligand praent in th dietake its aishi buh

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