Could the Ksp in this experiment be found following the same exact procedure if the Ksp of Ca(OH)2 was [5.5 X 10—2 M3]? Explain the chemistry behind your reasoning in detail AND explain what your data would have looked like showing all calculations with units to explain how you came to this conclusion

Yes, the same procedure can be used to calculate the Ksp.

Explanation:

In order to calculate the solubility product (Ksp) of the compound, you need its solubility at 298 K (room temperature).

Next, write down the equation for equilibrium. If the units are not given in mol , convert them as such to eliminate errors in calculation.  

The final answer will contain the units because there is in the equation.

Hope that answers the question, have a great day!