Yes, but is there a way to write the solubility as a function of temperature and such and theory to back it up? Of course I can look up tables, but lets say the temperature is farther off and I want to reduce error, what can I do? Oh yea, I didn't mention it, but assume standard pressure.
The solubility at saturation is given by the equilibrium constant Ksp
, the solubility product, which you can easily look up. This governs the equilibrium:
(aq) + Cl-
(aq)] (we neglect solids in any equilibria that involve solutions, so [NaCl (s)] becomes unity - it =1 and we needn't write it in) so as you can see, the greater the Ksp
, the more NaCl would be fitted into the solution at the point of saturation. Molar solubility of NaCl in this solution = [Na+
] or [Cl-
], take your pick, they will be the same, in which case you can write Molar Solubility[NaCl]2
and readily solve for Molar Solubility[NaCl].
is like any other equilibrium constant and we can model it in terms of the Gibbs' energy of the reaction, entropy and enthalpy. Find the entropy and enthalpy changes of your reactions, and the Ksp
, and it will be easy to model changing Ksp (and, by extension, changing solubility) with temperature.