Experiment 6

Experiment 6 - Discussion Experiment 6: Determination of an...

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Unformatted text preview: Discussion Experiment 6: Determination of an Equilibrium Constant Using a Spectrophometer, was about studying the chemical reactions of Fe 3+ and SCN - producing iron thiocyanide, Fe(SCN) 2+ in aqueous solution. Then the solurtion was measured for concentrations of ions in solution using a spectrophotometer. Equilibrium constants were then determined for this reaction at a given temperature. Fe 3+ (aq) + SCN - (aq) Fe(SCN) 2+ (aq) K = [FeSCN 2+] / [Fe 3+] [SCN - ] The initial concentrations of Fe 3+ were determined through the calculation of [Fe 3+] = 0.00200 M Fe 3+(5.00mL/5.00mL+1.00mL+5.00mL) = 0.00091 M. This initial concentration calculation and concentration was used for all solutions B-1 through B-5. The initial concentrations of [SCN -] were calculated similarly to the concentrations of Fe 3+ except for that the numerator of 5.00mL varied from B-1 to B-5 from 1mL to 5mL respectively. The equilibrium concentrations for both [Fe 3+] and [SCN -] were then discovered by subtracting the...
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This note was uploaded on 09/13/2011 for the course CHEM 1A Lab taught by Professor Staff during the Fall '09 term at UCSB.

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Experiment 6 - Discussion Experiment 6: Determination of an...

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