`1.1g` of `CoCl_(3).6NH_(3)` (mol.wt. `=267`) was dissolved in 100g of `H_(2)O`. The freezing point of the solution was `-0.29^(@)C`. How many moles of solute particles exist in solution for each mole of solute introduced ? `K_(f)` for `H_(2)O=1.86^(@)C.m^(-1)`

Explanation

To solve the problem step by step, we will follow these calculations:

### Step 1: Calculate the change in freezing point (ΔTf)
The freezing point depression (ΔTf) is given as:
\[ \Delta T_f = 0 - (-0.29) = 0.29 \, ^\circ C \]

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