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.
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.
Your definition of solubility equilibrium is correct. It describes the dynamic equilibrium between the undissolved excess solute and the solvent or aqueous solution, as well as the crystal in a saturated solution.
However, your statement about adding more solute disrupting the equilibrium and causing a precipitate is slightly inaccurate. When you add additional solute to a saturated solution, the equilibrium shifts towards the dissolution of more solute rather than the formation of a precipitate. This results in a supersaturated solution, which means that the concentration of the solute in the solution exceeds its equilibrium solubility.
In a supersaturated solution, the rate of crystallization is still equal to the rate of dissolution, but the excess solute is temporarily retained in the solution due to the increased concentration. If any disturbances occur (such as shaking the container or introducing a seed crystal), the excess solute can rapidly crystallize out, causing a precipitate to form.
Therefore, it is not incorrect to say that adding more solute to a saturated solution can disrupt the equilibrium and, under certain conditions, lead to the formation of a precipitate.
Your definition of solubility equilibrium is generally accurate. Solubility equilibrium refers to the dynamic balance between the dissolution of an excess solute and the recrystallization (or crystalization) of the solute in a saturated solution.
In a saturated solution, the rate of dissolution of solute particles is equal to the rate of recrystallization of solute particles. This means that over time, the concentration of solute in the solution remains constant, as the rate of particles leaving the solid and entering the solution is equal to the rate of particles leaving the solution and rejoining the solid.
Regarding your statement about adding more solute disrupting equilibrium and causing a precipitate to form, there is a slight inaccuracy. When additional solute is added to a saturated solution, it does not necessarily disrupt the equilibrium and cause an immediate precipitate formation. Instead, it increases the concentration of the solute beyond its solubility limit, resulting in a supersaturated solution.
A supersaturated solution contains more solute than it normally would at that temperature and pressure. It is considered unstable because it is above its equilibrium solubility. If any disturbance occurs, such as adding a seed crystal or agitating the solution, it will trigger the rapid precipitation of excess solute until the solution reaches the saturated state again.
So, the overall concept is that adding more solute to a saturated solution can lead to supersaturation, which is an unstable state. However, the immediate formation of a precipitate depends on the presence of a seed crystal or an external disturbance.