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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.

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Related questions

Select the false statement below.
A. PbCO3 is more soluble in aqueous HCl than in pure water
B. PbCl2 is less soluble in an aqueous solution of Pb(NO3)2 than inpure water
C. PbCl2 is less soluble in pure water than in aqueous KCN (Ksp ofPbCl2 = 1.7 x 10-5 and Kf of Pb(CN)42- = 2.0 x 1010)
D. PbCl2 is more soluble in aqueous HCl than in pure water

The theoretical solubility of calcium phosphate can be calculatedfrom its Ksp value, but its actual observed solubility is greaterthan its calculated theoretical solubility. Why?
A. hydrolysis involving the calcium ion acts to shift the calciumphosphate solubility equilibrium to the left, increasing thesolubility of the calcium phosphate
B. hydrolysis involving the phosphate ion acts to shift the calciumphosphate solubility equilibrium to the right, increasing thesolubility of the calcium phosphate
C. hydrolysis involving the calcium ion acts to shift the calciumphosphate solubility equilibrium to the right, increasing thesolubility of the calcium phosphate
D. hydrolysis involving the phosphate ion acts to shift the calciumphosphate solubility equilibrium to the left, increasing thesolubility of the calcium phosphate
E. hydration of the calcium ion produces an acidic solution whichresults in a greater solubility of calcium phosphate

For any slightly soluble salt placed in water, an equilibrium isestablished between the solid and ions in solution. Consider thefollowing reaction: Ca(IO3)2 (s) <----> Ca 2+ (aq) + 2IO3- a)Write the equilibrium constant expression for this reaction (Ksp).b) When calcium Iodate is added to water at 25 degrees celsius ,the equilibrium concentration of calcium ion was found to be0.011M. Calculate the value of Ksp for this salt.

Calcium oxalate (CaC2O4) is relatively insoluble in water (Ksp = 2×10-9). However, calcium oxalate is more soluble in acidic solution. How much more soluble is calcium oxalate in 0.10 M H+ than in pure water? In pure water, ignore the basic properties of C2O42-.

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