Join now for JEE/NEET and also prepare for Boards Join now for JEE/NEET and also prepare for Boards. Register Now
Hey there! We receieved your request
Stay Tuned as we are going to contact you within 1 Hour
One of our academic counsellors will contact you within 1 working day.
Click to Chat
1800-1023-196
+91-120-4616500
CART 0
Use Coupon: CART20 and get 20% off on all online Study Material
Welcome User
OR
LOGIN
Complete Your Registration (Step 2 of 2 )
Sit and relax as our customer representative will contact you within 1 business day
Criteria of precipitation of an electrolyte: Criteria of precipitation of an electrolyte:
Criteria of precipitation of an electrolyte:
Criteria of precipitation of an electrolyte A very useful conclusion is derived from the solubility product concept. No precipitation of the electrolyte occurs if the ionic product is less than the solubility product, i.e., the solution has not reached the saturation stage. Case I: When Kip<Ksp, then solution is unsaturated in which more solute can be dissolved. Case II: When Kip = Ksp, then solution is saturated in which no more solute can be dissolved. Case III: When Kip > Ksp, then solution is supersaturated and precipitation takes place. When the ionic product exceeds the solubility product, the equilibrium shifts towards left hand side, i.e., increasing the concentration of undissociated molecules of the electrolyte. As the solvent can hold a fixed amount of electrolyte at a definite temperature, the excess of the electrolyte is thrown out from the solution as precipitate. Thus, for the precipitation of an electrolyte, it is necessary that the ionic product must exceed its solubility product For example, if equal volumes of 0.02 M AgN03 solution and 0.02 M K2Cr04 solution are mixed, the precipitation of Ag2Cr04 occurs as the ionic product exceeds the solubility product of Ag2Cr04 which is 2 × 10–12.
Criteria of precipitation of an electrolyte
A very useful conclusion is derived from the solubility product concept. No precipitation of the electrolyte occurs if the ionic product is less than the solubility product, i.e., the solution has not reached the saturation stage.
Case I: When Kip<Ksp, then solution is unsaturated in which more solute can be dissolved.
Case II: When Kip = Ksp, then solution is saturated in which no more solute can be dissolved.
Case III: When Kip > Ksp, then solution is supersaturated and precipitation takes place.
When the ionic product exceeds the solubility product, the equilibrium shifts towards left hand side, i.e., increasing the concentration of undissociated molecules of the electrolyte. As the solvent can hold a fixed amount of electrolyte at a definite temperature, the excess of the electrolyte is thrown out from the solution as precipitate.
Thus, for the precipitation of an electrolyte, it is necessary that the ionic product must exceed its solubility product For example, if equal volumes of 0.02 M AgN03 solution and 0.02 M K2Cr04 solution are mixed, the precipitation of Ag2Cr04 occurs as the ionic product exceeds the solubility product of Ag2Cr04 which is 2 × 10–12.
Dear , Preparing for entrance exams? Register yourself for the free demo class from askiitians.
points won -