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NEET CHEMISTRYCoordination CompoundsMedium

Question

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}.

Exam Context & Concepts Covered

This question aligns with the NEET CHEMISTRY syllabus, specifically targeting concepts from Coordination Compounds. Mastering this topic is crucial for scoring well in the upcoming medical entrance examinations. Solving conceptually related problems will help you understand the nuances of these concepts and improve your problem-solving speed.

CHEMISTRYCoordination Compoundsexcesssolutiondichlorotetraaquachromiumiiichloridenumber

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