Solubility Product Constants

Solubility Product Constants - sp K ˃ sp , which means the...

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Roshni Sheth CH 118-M3 March 24, 2010 Solubility Product Constants 1. Summary of Results In this experiment, 0.4 M solutions of A(NO 3 ) 2 , K 2 X, B(NO 3 ) 2 , and KY were first diluted to 0.2, 0.05, 0.025, 0.0125, and 0.00625 M solutions with deionized water. The AX solutions were made by adding 10 drops of each concentration A(NO 3 ) 2 to 10 drops of the same concentration of K 2 X. The BY 2 solutions were made by adding 5 drops of B(NO 3 ) 2 and 10 drops of the same concentration of KY. The new solutions were observed in a well plate to see if any precipitate formed. Then, the solutions were diluted to find a more specific range of the formation of precipitate to no formation of precipitate. For the AX solution, 0.1225 K ˃ sp 0.09. ˃ For the BY 2 solution, 0.001 K ˃ sp 1.25 x 10 ˃ -4 2. Stoichiometry and K sp It is not reasonable to compare the solubility of the two salts. The AX solution dissolves into only two ions, making x 2 =K sp , but the BY 2 solution dissolves into three ions, making x 3 =K sp . 3. Cause of Precipitation Precipitation occurs when Q
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Unformatted text preview: sp K ˃ sp , which means the measured concentration of ions is higher than the concentration of ions at equilibrium. This means that the concentrations of A 2+ and X 2-could possibly be equal when a precipitate forms, as supported by the experimental data. 4. Heat of Reaction and Solubility If the reaction was exothermic, the solubility of the ions would increase with the increase in temperature. As heat escaped the reaction, the solution would cool, and the solubility of the ions would then decrease. To prevent the effect of temperature, the reaction could be put in a hot water bath or over a Bunsen burner. 5. A More Quantitative Method Another method of determining the value of the solubility product constant more accurately would be to set up a titration. After examining the results of the titration, the concentration of one of the ions would be known, and the concentration of the other ion could be determined using stoichiometry....
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This note was uploaded on 06/28/2011 for the course CH 118 taught by Professor March during the Spring '09 term at University of Alabama at Birmingham.

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Solubility Product Constants - sp K ˃ sp , which means the...

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