1. Tardigrade
  2. Question
  3. Chemistry
  4. A solution containing 2.675 g of CoCl3 ⋅ 6NH3 (molar mass = 267 g mol-1) is passed through a cation exchanger. The chloride ions obtained in solution were treated with excess of AgNO3 to give 4.78 g of AgCl. The formula of the complex is:

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Q. A solution containing $2.675\, g$ of $CoCl_{3} \cdot 6NH_{3}$ (molar mass $= 267 \,g mol^{-1}$) is passed through a cation exchanger. The chloride ions obtained in solution were treated with excess of $AgNO_{3}$ to give $4.78\, g$ of $AgCl$. The formula of the complex is:

Coordination Compounds

Solution:

No. of moles of complex =$\frac{2.675}{267.5}=0.01$
No. of moles of AgCl ==$\frac{4.78}{143.5}=0.03$
This shows that three Cl- ions are precipitated. Thus, formula of the complex is $[Co(NH_{3})_{6}]Cl_{3}.$