Équilibres de solubilité Flashcards
Define solubility of a sparingly soluble salt
conc referring to max amt of solute (in g or mol) that can b dissolved in 1dm³ of solvent to make saturated sol n at given temp
Define solubility product (Ksp) of a sparingly soluble salt
eqm const which is pdt of molar conc of dissolved associated ions (each raised to appropriate pwr) in saturated sol n of salt at given temp
Define common ion effect
solubility of a sparingly soluble salt is decreased in presence of common ion fr external source
What is the relationship between ionic product and Ksp? (HINT: what occurs?)
When:
-ionic pdt > Ksp (beyond saturation pt), precipitation occurs
-ionic pdt = Ksp (Saturation pt) OR ionic pdt < Ksp (lower than saturation pt), no precipitation occurs
What to take note of when two solutions are mixed?
NEW total volume must be calculated to obtain NEW conc.
Define ionic product
pdt of molar conc of dissolved dissociated ions (each raised to appropriate pwr) in sol n at given temp (at any pt in time)
What is the difference between Ksp and Ionic Product?
Ksp is const at const temp. Ionic pdt not const; depends on conc of rxt or situation
eg
MX(s) ⇌ M+(aq) + X-(aq)
Ksp = [M+]eqm[X-]eqm (eqm conc.)
vs
Ionic product = [M+][X-] (to be calculated based on given info)
What is the general effect of complex ion form n on salt solubility?
- solubility of sparingly soluble salt increases w add n of reagent that reacts w cation (or anion) to form complex ions
- add n of complexing reagent decreases conc of cation (or anion)
- By LCP, eqm pos n of (1) shift right to increase conc of cation (or anion), so more of sparingly soluble salt dissolves