an excess of agno3 is added to 100 ml of a 0.01 M solution of [cr(h2o)4cl2]cl.the number of agcl precipated would be:
is this question based on common ion effect
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Given, volume of solution = 100mL = 0.1L
molarity of [Cr(H₂O)₄Cl₂]Cl = 0.01M
We know,
Molarity = number of mole of solute/volume of solution {in L}
0.01 M = number of moles of solute /0.1
Number of moles of solute = 0.01 × 0.1 = 0.001 mol
In given complex [Cr(H₂O)₄Cl₂]Cl ,only one Cl ion are ionizable .
So, if number of moles of complex is 0.001 then, number of moles of ionizable Cl ions is 0.001 mol
Hence, number of AgCl precipitated = 0.001 mol
according to above explanation it is clearly shown that it is not based on common ion effect.
molarity of [Cr(H₂O)₄Cl₂]Cl = 0.01M
We know,
Molarity = number of mole of solute/volume of solution {in L}
0.01 M = number of moles of solute /0.1
Number of moles of solute = 0.01 × 0.1 = 0.001 mol
In given complex [Cr(H₂O)₄Cl₂]Cl ,only one Cl ion are ionizable .
So, if number of moles of complex is 0.001 then, number of moles of ionizable Cl ions is 0.001 mol
Hence, number of AgCl precipitated = 0.001 mol
according to above explanation it is clearly shown that it is not based on common ion effect.
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