Question

An excess of AgNO3 is added to 100 mL of a 0.01 M solution of dichlorotetraaqua-chromium

Answer 1

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.