Why is anhydrous sodium hypochlorite less stable than its calcium counterpart? Thanks much in advanced!

TLC has not yet shown us a second peak.  We were thinking about running a column using one of our TLC solvent conditions when a colleague suggested dissolving the product in chloroform.  That will be what we try next.

Wrong way round. CuCO₃ will precipitate first, as it has the lower solubility product. Calculate the concentration of carbonate needed to start precipitating Ni²⁺. What is the concentration of Cu²⁺ in equilibrium with this?

Hello, I've been stuck on a question for a while now, and I would like to have someone else look at it.
The question is: "Sodium carbonate is added in small quantities to a solution containing Ni2+ ions with a molar concentration of 0.1 and Cu2+ ions with a molar concentration of 0.1. Calculate the concentration of the first ion which starts to precipitate when the second ion starts to precipitate as well. Ksp(NiCO3) = 1.4x10^-7, Ksp (CuCO3) = 2.5x10^-10".
The way I've solved this particular question has given me an unsual answer, but basically what I've done was to calculate the concentration of the carbonate ion needed in order to make CuCO3 precepitate and then use the same concentration to calculate the concentration of Ni2+ions as requested. The result I've got is 56 M.
Can someone please tell me if I answered correctly or if I did something wrong? The result just doesn't seem right and I can't seem to find an answer on any of my Chemistry books.
Thank you very much.

We have made CH₃SO₂CH₂P(O)(OCH₂CH₃)₂ multiple times by reacting Oxone with the corresponding sulfide in methanol/water.  We extract from DCM and use the product without further purification (Blumenkopf 1986 and others).  We removed the solvent using rotary evaporation and high vacuum.  Our most recent synthesis had more than 10% more mass than theoretical and showed a broad peak in the H-1 NMR spectrum near the doublet arising from the bridging CH₂ group.  The appearance is more amorphous than crystalline.  These observations are entirely unexpected based upon our past experiences.  The only difference of which I am aware is that some of the starting sulfide came from a new bottle from the same manufacturer.  This week we tried dissolving in chloroform and removing the solvent, in the hope of stripping away what might be methanol that was present.  The mass is pretty close to what it was before, and I have not checked the NMR yet.  Does anyone have a suggestion about what to try next?