<Dl> <Dd> K s = (C 12 H 22 O 11 (a q)) (\ displaystyle K_ (\ mathrm (s)) = \ left (\ mathrm ((C) _ (12) (H) _ (22) (O) _ (11) (aq)) \ right) \,) </Dd> </Dl> <Dd> K s = (C 12 H 22 O 11 (a q)) (\ displaystyle K_ (\ mathrm (s)) = \ left (\ mathrm ((C) _ (12) (H) _ (22) (O) _ (11) (aq)) \ right) \,) </Dd> <P> is obtained . This is equivalent to defining the standard state as the saturated solution so that the activity coefficient is equal to one . The solubility constant is a true constant only if the activity coefficient is not affected by the presence of any other solutes that may be present . The unit of the solubility constant is the same as the unit of the concentration of the solute . For sucrose K = 1.971 mol dm at 25 ° C . This shows that the solubility of sucrose at 25 ° C is nearly 2 mol dm (540 g / l). Sucrose is unusual in that it does not easily form a supersaturated solution at higher concentrations, as do most other carbohydrates . </P> <P> Ionic compounds normally dissociate into their constituent ions when they dissolve in water . For example, for silver chloride: </P>

What happens to the ksp value of a solid as the temperature changes