K_SP for Ca(OH)_2 is determined in two separate experiments, both at the same te
ID: 1006030 • Letter: K
Question
K_SP for Ca(OH)_2 is determined in two separate experiments, both at the same temperature. - by titration of hydroxide in a simple saturated solution of Ca(OH)_2. - by titration of hydroxide in a 0.01 M CaCl_2 solution saturated with Ca(OH)_2. Identify which of the following statements is either completely "True" or at least partially "False" (assuming that the activity of each ion is equal to its molar concentration in each instance): You would expect the value for Ksp to be the same from both experiments, since K_SP is a constant at a given temperature. You would expect more Ca(OH)_2 to be able to dissolve in the simple solution, than in the CaCl_2 solution. You would expect the value for K_SP to be lesser in the second experiment, since less Ca(OH)_2 can dissolve in the presence of the additional amount of Ca^2+(aq). In the second experiment, while [Ca^2+]is greater, [OH^-] is lower than in the the first experiment. You would expect the value for K_SP to be different in the two experiments, since the presence of CaCl_2(aq) affects the equilibrium position.Explanation / Answer
1 false
Reason since there is common ion effect in second experiment
2 true
Reason there is no common ion effect in 1 st exp that is no existed Ca2+ ions to decrease the solubility
3 true
The same reason as mentioned above
4 true
5true
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