It is not your terminology that is off, it is your understanding of how solubility product works. Please try to read on the subject.
I just didn't know how to describe K
sp. I did say "each ion in the compound" and not just "each ion." What I meant was that, for example, in sodium carbonate, which has a molar solubility of .0001265M, the carbonate ion dissolves just as much as the sodium carbonate, so you could say its solubility
in sodium carbonate is also .0001265M. For every unit of sodium carbonate that dissolves, two sodium ions dissolve, so you could say it's twice as soluble, having a solubility of 0.0002530M
in sodium carbonate. These numbers change when the ions are in different pairs, so the ion itself obviously does not have a solubility. Do you see where I'm coming from? I understand that an ion itself does not have a solubility. I know how to calculate K
sp. I know that it's an equilibrium constant. I know that it describes a saturated solution, where the rate of dissolution and precipitation of a compound are equal. What am I missing, great, wise, and critical Borek? I aspire to achieve your wisdom.
If you could just give me some tips on which aspects of solubility product to read about instead of just telling me to read on the subject, I'd greatly appreciate it.