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NEET CHEMISTRYMedium

An excess of AgNO₃ is added to 100 mL of a 0.01M solution of dichlorotetraaquachromium(III) chloride. The number of moles of AgCl precipitated would be:

A

0.002

B

0.003

C

0.01

D

0.001

Step-by-Step Solution

  1. Determine the formula: The IUPAC name 'dichlorotetraaquachromium(III) chloride' indicates the complex ion consists of Chromium(III), four aqua (H2OH_2O) ligands, and two chlorido (Cl−Cl^-) ligands inside the coordination sphere. Charge on complex ion = Oxidation state of Cr + Charge of ligands = (+3)+4(0)+2(−1)=+1(+3) + 4(0) + 2(-1) = +1. To balance this +1 charge, there must be one chloride ion (Cl−Cl^-) outside the coordination sphere.
  • Formula: [Cr(H2O)4Cl2]Cl[Cr(H_2O)_4Cl_2]Cl .

  1. Identify Ionisable Chloride: According to Werner's theory, only the anions present outside the coordination sphere (primary valency) are ionisable and can precipitate with AgNO3AgNO_3. Here, there is 1 ionisable Cl−Cl^- per formula unit .

  2. Calculate Moles: Moles of complex = Molarity ×\times Volume (in Litres) = 0.01 mol L−1×0.1 L=0.001 mol0.01 \text{ mol L}^{-1} \times 0.1 \text{ L} = 0.001 \text{ mol}. Since 1 mole of complex yields 1 mole of AgClAgCl precipitate:

  • Moles of AgClAgCl = 1×0.001=0.001 mol1 \times 0.001 = 0.001 \text{ mol}.
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