> I think that reaction is slow at room temperature and at regular > developer pH range, say above 7. I think more problem with storage of > sulfite solution alone is the pathway that involves sulfur trioxide > anion radical and maybe hydroxyl radical. > -- From a purely observational viewpoint, I have noticed that the recrystalized sulfite in the bottom of my saturated bottle most closely resembles hydrated sodium sulfite in it's dry form (i.e large clear crystals). Also, I have noticed that when left undisturbed for several days, the solution in the vi citing of the crystals becomes more dense, that is when stirred it momentarily exhibits visible convection swirls. I presume this may be due to temperature fluctuations between night and day causing a slight gradient within the bottle. Anyway, the sulfite, as measured densitometrically using fresh solution as control, seems to hold up well at saturation. No rank, sulfurous smells from the headspace either. JB ============================================================================================================= To unsubscribe from this list, go to www.freelists.org and logon to your account (the same e-mail address and password you set-up when you subscribed,) and unsubscribe from there.