On treatment of 100 mL of 0.1 M solution of CoCl 3 ⋅ 6 H 2 O with excess AgNO 3 ; 1.2 × 1 0 22 ions are precipitated. The complex is :-

Question

On treatment of 100 mL of 0.1 M solution of CoCl 3 ​ ⋅ 6 H 2 ​ O with excess AgNO 3 ​ ; 1.2 × 1 0 22 ions are precipitated. The complex is :-

TestHub · Accepted Answer

To determine the complex, we first calculate the moles of CoCl₃ ∙ 6H₂O:

Moles = Volume (L) x Molarity (M) = $0.1 L \times 0.1 M = 0.01 m o l$ .

Next, we find the moles of AgCl precipitated:

Moles of AgCl = Number of ions / Avogadro's number

Moles of AgCl = $1.2 \times 1 0^{22} / (6.022 \times 1 0^{23} i o n s / m o l) \approx 0.02 m o l$ .

Since 0.01 mol of the complex yields 0.02 mol of AgCl, this means 2 Cl⁻ ions per complex molecule are outside the coordination sphere and precipitate with Ag⁺.

Therefore, the complex is $[Co (H_{2} O)_{4} Cl_{2}] Cl \cdot 2 H_{2} O$ .

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