Chem 1a Lab nov 4

Chem 1a Lab nov 4 - If K<<1 then vice versa for the...

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Discussion The purpose of the experiment was to measure concentrations of ions in solution using a spectrophotometer. Also, with this information, we were allowed to determine equilibrium constants of the reaction at a given temperature. In order to determine the concentrations of Fe(SCN)2+, Fe3+, and SCN- at equilibrium, we use the equation K=The products of a reaction to their coefficient power divided by the reactant to the power of their coefficient. Light absorbed by 5 different solutions gave us an equation of Y=1539x-.0007251. The x value varied between the 5 different solutions; the x value equaled the amount of absorbed light. By plugging in the concentration into the equilibrium constant equation, we are now able to find K. If K>>1, then equilibrium lies with the products as opposed to the reactants.
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Unformatted text preview: If K<<1, then vice versa for the previous sentence. The average value for K was 267.6032. The average value for pK was -2.43. The average deviation from the mean 19.343. The results show that the equilibrium constant is dependent upon the initial concentration. The values of pK are all relatively close; they are all negative numbers that represent the –log of K. The value of K depends upon temperature; so therefore the value of pK depends upon temperature as well. Possible sources of error that occurred in this lab could result from having the A solutions premixed; with these premixed solutions, the amount of time that they were premixed changes the composition of the solution and the absorption of light as well. The longer the solution was out, the more the light absorbency was altered....
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This note was uploaded on 09/09/2011 for the course CHEM 1A taught by Professor Van koppen during the Spring '07 term at UCSB.

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