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97 and 997 where 2 aminobenzoic acid carries a

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Unformatted text preview: pH of 4.97 and 9.97 (where 2-aminobenzoic acid carries a negative charge and 2-aminophenol is neutral. 3. Using a ladder diagram, explain why the reaction H3PO4(aq) + F–(aq) D HF(aq) + H2PO42–(aq) is favorable, but the reaction H3PO4(aq) + 2F–(aq) D 2HF(aq) + HPO4–(aq) is unfavorable. What are the equilibrium constants for each reaction? The ladder diagram to the left shows that are no pH levels where H3PO4 is the predominate form of phosphoric acid and F– is the predominate form of hydrofluoric acid; solutions of these two species must, therefore, react, forming HF and H2PO4– as products, both of which are the predominate species between a pH of 2.148 and 3.17. On the other hand, there are no pH values where the products of the second reaction (HF and HPO42–) simultaneously are the predominate forms of phosphoric acid and hydrofluoric acid. The equilibrium constants for the two reactions are found by adding together the appropriate reactions and mulitiplying their respective equilibrium constants. For the reaction H3PO4(aq) + F–(aq) D HF(aq) + H2PO42–(aq) we add together the acid dissociation reaction for H3PO4 (Ka = 7.11!10–3), the bas...
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This homework help was uploaded on 04/01/2014 for the course CHEM 352 taught by Professor Davidharvey during the Fall '13 term at DePauw.

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