![]() The silver iodide is so insoluble that ammonia cannot lower the silver ion concentration enough for the precipitate to dissolve. The more concentrated ammonia pushes the equilibrium even further to the right, lowering the silver ion concentration even more. lead (II) nitrate sodium sulfate zinc acetate + sodium sulfate & barium nitrate+ potassium iodide h. This occurs with silver chloride, and with silver bromide if the ammonia is concentrated. A white precipitate of potassium nitrate B. ![]() If the adjusted silver ion concentration multiplied by the halide ion concentration is less than the solubility product, some precipitate dissolves to restore equilibrium. The effect of adding the ammonia is to lower this concentration still further. When a colorless solution of silver nitrate is mixed with a yellow-orange solution of potassium dichromate a reddish precipitate of silver dichromate is produced. The equation for this reaction is given below:Ī solution in contact with one of the silver halide precipitates contains a very small concentration of dissolved silver ions. A precipitation reaction is a reaction that yields an insoluble producta precipitatewhen two solutions are mixed. This is a reversible reaction, but the complex is very stable, and the position of equilibrium lies well to the right. The ammonia combines with silver ions to produce a complex ion called the diamminesilver(I) ion, +. The compounds are all quite insoluble, but become even less so down the group. The table below lists solubility products from silver chloride to silver iodide (a solubility product for silver fluoride cannot be reported because it is too soluble). Enough solid is always precipitated to lower the ionic product to the solubility product.
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