:I think you are likely looking for the common ion effect.
2.
The soaps precipitate due to a combination of common ion effect and increased ionic strength.
3.
:Generally, the common ion effect is only a major issue in equilibrium situations.
4.
The salting out process used in the manufacture of soaps benefits from the common ion effect.
5.
This value depends on the type of salt ( AgCl vs . NaCl, for example ), temperature, and the common ion effect.
6.
Sea, brackish and other waters that contain appreciable amount of Na + interfere with the normal behavior of soap because of common ion effect.
7.
:: I guess for clarity I should state that this is not an attempt to use the common ion effect but actually solvation effects.
8.
I didn't even want to talk about the common ion effect . . . talk ) 03 : 48, 1 November 2010 ( UTC)
9.
One is the " common ion effect " already mentioned above : if the substance split into multiple components when dissolving, the concentrations of all those components will affect the precipitation rate.
10.
:: Having just read common ion effect, it doesn't really explain how the addition of a substance containing one ion ( which is present both substances ) causes the solubility product of one to be exceeded.
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