To get the precipitate to dissolve, you obviously need the ligand exchange equilibrium to lie well to the right, but you need the acid-base equilibrium to be easy to pull back to the left. It depends on the positions of the equilibria. Looking at it like this is helpful in explaining why some precipitates dissolve in excess ammonia while others don't. This precipitate, however, dissolves in the. There is now an interaction between the two equilibria: On adding dilute ammonia solution to the colorless solution of a salt, a white gelatinous precipitate appears. Uses advised against No Information available 1.3. Relevant identified uses of the substance or mixture and uses advised against Recommended Use Laboratory chemicals. Notice that the hexaaqua ion appears in both of these. Product Description: Ammonia solution Cat No.
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