1. Compare your experimental value for Ksp of Ca(OH)2 with the literature value (Ksp = 8.0 × 10-6 at 25°C). Account for any difference. (Experimental value: Trial 1- 1.0061824 x 10^-5; Trial 2- 8.001504 x 10^-6). 2. Cite possible sources of error in the experiment. 3. Why must the solution be saturated when its solubility is determined? 4. Is Ca(OH)2 more soluble in aqueous solution containing calcium ions or in pure water? Explain your observation in terms of shift in equilibrium and in terms of the ion product in relation to Ksp.

1. Compare your experimental value for Ksp of Ca(OH)2 with the literature value (Ksp = 8.0 × 10-6 at 25°C). Account for any difference. (Experimental value: Trial 1- 1.0061824 x 10^-5; Trial 2- 8.001504 x 10^-6). 2. Cite possible sources of error in the experiment. 3. Why must the solution be saturated when its solubility is determined? 4. Is Ca(OH)2 more soluble in aqueous solution containing calcium ions or in pure water? Explain your observation in terms of shift in equilibrium and in terms of the ion product in relation to Ksp.

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 11E: The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...

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