(a)
Interpretation:
The net ionic equation for the precipitation of
Concept introduction:
According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.
Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.
(b)
Interpretation:
The net ionic equation for the precipitation of
Concept introduction:
According to the Le Chatelier’s principle, a change in one of the variables that describe a system at equilibrium produces a shift in the position of the equilibrium that counteracts the effect of this change.
Usually, diprotic and polyprotic acid dissociation is undergoes through several equilibrium steps.
(c)
Interpretation:
The net ionic equation for the precipitation of
Concept introduction:
Follow the lower-numbered guideline when two guidelines are in conflict. This leads to the correct prediction in most cases.
- Salts of group 1 cations (with some exceptions for Li+) and the NH4+ cation are soluble.
- Nitrates, acetates, and perchlorates are soluble.
- Salts of silver, lead, and mercury (I) are insoluble.
- Chlorides, bromides, and iodides are soluble
- Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca2+, Sr2+, and Ba2+ are slightly soluble).
- Sulfates are soluble except for those of calcium, strontium, and barium.
There are only two possibilities. Either some cation−anion combination leads to an insoluble solid—a precipitate—or no such combination is possible, or there is no reaction at all.
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General Chemistry: Principles and Modern Applications (11th Edition)
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