I have [CoCl4}2 /{Co(h2O)6}2+and add AgNo3 what does silvirnitrate does and how is that consit with Chatelier
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When you add silver nitrate (AgNO3) to a solution containing [CoCl4]2- or [Co(H2O)6]2+, a chemical reaction takes place. The silver nitrate reacts with the chloride ions (Cl-) in the [CoCl4]2- complex to form silver chloride (AgCl), which is a solid precipitate that appears as a white substance. The balanced chemical equation for this reaction is:
2 AgNO3 + [CoCl4]2- → 2 AgCl + [Co(NO3)4]2-
On the other hand, silver nitrate does not directly react with the [Co(H2O)6]2+ complex since it does not contain chloride ions. Therefore, no precipitate forms in this case.
This reaction is consistent with Le Chatelier's principle, which states that when a system at equilibrium is subjected to a stress, it will respond by shifting in a direction that minimizes the effect of that stress.
In this case, the stress is the addition of silver nitrate. By adding silver nitrate to the system, the concentration of silver ions (Ag+) increases. According to Le Chatelier's principle, the system will respond by shifting in a direction that minimizes the effect of the increased Ag+ concentration.
Since Ag+ can react with Cl- to form AgCl, the system will shift to consume the excess Ag+ by forming AgCl. This ultimately results in the precipitation of silver chloride.
To summarize, silver nitrate reacts with chloride ions in the [CoCl4]2- complex to form silver chloride precipitate. Le Chatelier's principle predicts that the system will shift to minimize the effect of the increased Ag+ concentration, leading to the formation of AgCl.