1. Why must the solution be saturated when its solubility is determined?
2. Compare your experimental value for Ksp of Ca(OH)2 with the literature value (Ksp = 8.0 × 10-6 at 25°C). Account fora anydifference.
3. 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.
4. Cite possible sources of error in the experiment.
5. The solubility of CdS in water is 1.29 x10-12 M. Determine the solubility product constant for CdS.
6. The solubility product constant of Cd(OH)2 and Co(OH)2 are 7.21 × 10–15 and 5.92 × 10–15, respectively. In terms of calculating molar solubility, which of these hydroxides is less soluble?
Trending now
This is a popular solution!
Step by step
Solved in 2 steps