solubility equillibrium is dynamic equillibrium between undissolved excess solute and solvent or aqueous solution and crystal in a saturated solution. so rate of dissolving = rate of crystalization if any more solute is added it will disrupt equillibrium and a precipitate will form? because it is now supersaturated?
is there anything incorrect with this definition.
2 answers
when crystals collide with dissolved ions the substance precipitates out of solution and when crystals collide with water they for dissolved solute... does this have anything to do with equillibrium and what does precipitate out of solution imply?
solubility equillibrium is dynamic equillibrium between undissolved excess solute and solvent or aqueous solution and crystal in a saturated solution. so rate of dissolving = rate of crystalization I can buy your statement to this point if any more solute is added it will disrupt equillibrium and a precipitate will form? because it is now supersaturated?
is there anything incorrect with this definition.
If more solute is added to a saturated solution, the net effect is that no more of the solute will dissolve. A molecule or two may go into solution followed by a molecule or two that's already in solution (that's the dynamic equilibrium part--it isn't static) will come out of solution. The two (going in and coming out) occur essentially at the same time. I suppose if we wanted to talk in nanoseconds that we might say when two more molecules go into solution we have a supersaturated solution for a nanosecond or two until equilibrium (note the correct spelling of equilibrium) can correct but normally, supersaturated solutions are solutions that contain much more solute than normal AND IT IS META STABLE; that is, with careful handling a solution that is supersaturated can be passed around the room and observed. In fact, some supersaturated solution are so stable that it takes rough handling plus adding a seeding crystal plus stirring plus cooling far below the crystallization point to make it rturn to a simple saturated solution.
Please note that using periods and starting sentences with a capital letter makes it so much easier to understand. You used periods except for one end of sentence but no caps. Frankly, that's why I passed up the question when you posted yesterday; I couldn't make sense of it.
is there anything incorrect with this definition.
If more solute is added to a saturated solution, the net effect is that no more of the solute will dissolve. A molecule or two may go into solution followed by a molecule or two that's already in solution (that's the dynamic equilibrium part--it isn't static) will come out of solution. The two (going in and coming out) occur essentially at the same time. I suppose if we wanted to talk in nanoseconds that we might say when two more molecules go into solution we have a supersaturated solution for a nanosecond or two until equilibrium (note the correct spelling of equilibrium) can correct but normally, supersaturated solutions are solutions that contain much more solute than normal AND IT IS META STABLE; that is, with careful handling a solution that is supersaturated can be passed around the room and observed. In fact, some supersaturated solution are so stable that it takes rough handling plus adding a seeding crystal plus stirring plus cooling far below the crystallization point to make it rturn to a simple saturated solution.
Please note that using periods and starting sentences with a capital letter makes it so much easier to understand. You used periods except for one end of sentence but no caps. Frankly, that's why I passed up the question when you posted yesterday; I couldn't make sense of it.
1 answer