It should be determined whetherformation of a complex ion in an ion solution of Hg 2+ , I - , Ag+ and NO 2 - increase or decrease the amount of precipitate. Concept introduction: Non-common Ion Effect: - The effect of “noncommon” or diverse ions is not as striking as the common-ion effect. Moreover, diverse ions tend to increase rather than decrease solubility. As the total ionic concentration of a solution increases, interionic attractions become more important. Activities become smaller than the stoichiometric concentration. For the ions involved in the solution process, this means that higher concentrations must appear in solution before equilibrium is established—the solubility increases.
It should be determined whetherformation of a complex ion in an ion solution of Hg 2+ , I - , Ag+ and NO 2 - increase or decrease the amount of precipitate. Concept introduction: Non-common Ion Effect: - The effect of “noncommon” or diverse ions is not as striking as the common-ion effect. Moreover, diverse ions tend to increase rather than decrease solubility. As the total ionic concentration of a solution increases, interionic attractions become more important. Activities become smaller than the stoichiometric concentration. For the ions involved in the solution process, this means that higher concentrations must appear in solution before equilibrium is established—the solubility increases.
Solution Summary: The author explains the effect of non-common or diverse ions is not as striking as the common-ion effect.
It should be determined whetherformation of a complex ion in an ion solution of Hg2+, I-, Ag+ and NO2- increase or decrease the amount of precipitate.
Concept introduction:
Non-common Ion Effect: - The effect of “noncommon” or diverse ions is not as striking as the common-ion effect. Moreover, diverse ions tend to increase rather than decrease solubility. As the total ionic concentration of a solution increases, interionic attractions become more important. Activities become smaller than the stoichiometric concentration. For the ions involved in the solution process, this means that higher concentrations must appear in solution before equilibrium is established—the solubility increases.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell