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# How many precipitated ions are produced by $CrCl_3.5NH_3$ with $AgN{O_3}$ in an aqueous solution?

Last updated date: 27th Feb 2024
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Hint: $AgCl$ is an ionic compound but it is insoluble in water. It defies the aqueous law of solubility. $AgCl$ has a very strong bond between silver and chlorine ions. They have a very strong attraction between them. $AgCl$ precipitate is white in colour.

$CrCl_3.5NH_3$ is a coordinate compound. now a coordinate compound formed by d block elements. What happens is that the d block element loses their electrons. The ligands, hugely negative electrons, attack the empty orbitals. These are highly electronegative and distort the orbital. This is called hybridisation.
$CrCl_3.5NH_3$ has eight ligands and we know that the chromium can lose two, three or six electrons, so there will be only six ligands, the formula would be like $[Cr{(N{H_3})_5}Cl]C{l_2}$
$[Cr{(N{H_3})_5}Cl]C{l_2} + 2AgN{O_3} \to [Cr{(N{H_3})_5}Cl](N{O_3}) + 2AgCl$