The ** change in freezing point** is also related to the molality of the solution:

$\overline{){{\mathbf{\Delta T}}}_{{\mathbf{f}}}{\mathbf{=}}{\mathbf{i}}{\mathbf{\xb7}}{\mathbf{m}}{\mathbf{\xb7}}{{\mathbf{K}}}_{{\mathbf{f}}}}$

$\overline{){{\mathbf{\Delta T}}}_{{\mathbf{f}}}{\mathbf{=}}{{\mathbf{T}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{pure}\mathbf{}\mathbf{solvent}}{\mathbf{-}}{{\mathbf{T}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{solution}}}$

**Step 1: **van’t Hoff factor (i)

iron (III) chloride **→ FeCl _{3}**

▪ **FeCl _{3}**

▪

Use the van't Hoff factors in the table below to calculate each colligative property:

Van't Hoff Factors at 0.05 m Concentration in Aqueous Solution

Solute | /Expected | /Measured |

Nonelectrolyte | 1 | 1 |

NaCl | 2 | 1.9 |

MgSO_{4} | 2 | 1.3 |

MgCl_{2} | 3 | 2.7 |

K_{2}SO_{4} | 3 | 2.6 |

FeCl_{3} | 4 | 3.4 |

Calculate the melting point of a 0.111 m iron(III) chloride solution.

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Our tutors have indicated that to solve this problem you will need to apply the Freezing Point Depression concept. If you need more Freezing Point Depression practice, you can also practice Freezing Point Depression practice problems.

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Based on our data, we think this problem is relevant for Professor Kesling's class at CAMPBELL.