a) A student A weighed .50 Ca(OH)2 for his saturated solution and student B weighed 0.23 g, Both students dissolved it in 60 ml of water and both had solid left in their solution before filtrating. After filtrating to a clear solution, which student had the most concentrated solution? What would the effect on the volume of HCl titrant used and the calculated Ksp of the reaction if one of the students had a couldy solution after filtering and proceeded to titrate it compared to a clear solution?
(b) A saturated solution of CA(OH)2 is prepared and filtered. If 9.32 mL of 0.045 M HCl is used to titrate a 10 ml sample of the solution to end point:
- how many moles of Ca^2+, OH- were in the original 10 mL sample
- what are the concentrations of Ca^2+ and OH- in the saturated solution?
- what is the molar solubility for Ca(OH)2 under these conditions?
- Calculate Ksp for Ca(OH)2 under these conditions
(c) If change in entropy of the universe can tell us whether a process will be spontaneous, why do we need delta G (Gibb's free energy)