Water ampholytic (acid+base) equilibrium:
H2O + H2O <--> H3O+ + OH-
Equilibrium is only found in a saturated solution, where the dissolved species and the undissolved species are in equilibrium with each other. In a dilute solution there is nothing that is undissolved, and so there is no equilibrium, and by definition a supersaturated solution is out of equilibrium and essentially has too much stuff dissolved in it (it will eventually return to equilibrium and some of the dissolved material will precipitate out).
When the dissolving rate equals the rate at which molecules comes out of solution the solution is in 'equilibrium'.
You get a double decomposition reaction, producing sodium hydroxide and potassium carbonate, but actually there is no real reaction; the four substances remain in perfect equilibrium in solution.
You could say ammonium hydroxide, but that is not quite correct in solution. NH3(aq) is sometimes used, but this is the equilibrium reaction. NH3 + H2O <<->> NH4(+) + OH(-)
If KI is present in a solution and PbI2 is being dissolved in it, there will be a greater concentration of I, this will cause the equilibrium to shift left, away from the increase, according to Le Chatelier's Principle. Shifting the equilibrium left will result in a greater mass of solid PbI2. Therefore the solubility of PbI2 will decrease in a solution of KI.
the reaction is at dynamic equilibrium.
Homogeneous equilibrium occurs when all reactants and products are in the same physical state, such as all being in the gas phase or all being in solution. It is characterized by the forward and reverse reactions occurring at the same rate, resulting in a constant concentration of reactants and products. The equilibrium constant for homogeneous equilibria is defined based on concentrations of species in the same phase.
Equilibrium is only found in a saturated solution, where the dissolved species and the undissolved species are in equilibrium with each other. In a dilute solution there is nothing that is undissolved, and so there is no equilibrium, and by definition a supersaturated solution is out of equilibrium and essentially has too much stuff dissolved in it (it will eventually return to equilibrium and some of the dissolved material will precipitate out).
isotonic solution, equilibrium
When the dissolving rate equals the rate at which molecules comes out of solution the solution is in 'equilibrium'.
If a solution is saturated you will not be able to dissolve any more of the material in that solution at that temperature. If the concentration of the dissolved material determines the reaction rate of a reaction you care about then you will need to adjust temperature or make other changes to speed it up. In contrast, if you have an unsaturated solution, you can dissolve more of the material in it and increase the reaction rate.
Equilibrium solubility is how much of a certain solute is in solution when the system has reached equilibrium. For example, when something like silver chloride (AgCl) is placed in water, none of it goes into solution. But given some time, an equilibrium will be reached where a small amount of AgCl is in solution and is in equilibrium with the insoluble AgCl.
Saturated
You get a double decomposition reaction, producing sodium hydroxide and potassium carbonate, but actually there is no real reaction; the four substances remain in perfect equilibrium in solution.
a supersaturated solution
A saturated solution.
equilibrium