**Problem d: Freezing Point Depression Calculation****Objective:**Determine the freezing point depression when 210 grams of NaCl (sodium chloride) is added to 1000 grams of water.**Hint:**Consider the change in the number of particles when NaCl dissolves in water.**Explanation:**When NaCl dissolves in water, it dissociates into sodium (Na⁺) and chloride ions (Cl⁻), increasing the total number of dissolved particles. This process affects the colligative properties of the solution, resulting in a lower freezing point compared to pure water.**Key Concepts:**- **Freezing Point Depression (ΔTf):** A colligative property that describes the decrease in the freezing point of a solvent when a solute is added.- **Van't Hoff Factor (i):** Represents the number of particles the solute breaks into; for NaCl, i = 2 because it dissociates into two ions.- **Formula:** ΔTf = i * Kf * m - **ΔTf:** Freezing point depression - **Kf:** Freezing point depression constant for water (1.86 °C kg/mol) - **m:** Molality of the solution (moles of solute per kg of solvent)Use the information and hints provided to calculate the freezing point depression for the given solution.

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Answered: d. Determine the freezing point…

d. Determine the freezing point depression if you add 210 g of NaCl to 1000 g of water. (Hint: what happens to the number of particles when NaCl dissolves in water?)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

**Problem d: Freezing Point Depression Calculation**

**Objective:**
Determine the freezing point depression when 210 grams of NaCl (sodium chloride) is added to 1000 grams of water.

**Hint:**
Consider the change in the number of particles when NaCl dissolves in water.

**Explanation:**
When NaCl dissolves in water, it dissociates into sodium (Na⁺) and chloride ions (Cl⁻), increasing the total number of dissolved particles. This process affects the colligative properties of the solution, resulting in a lower freezing point compared to pure water.

**Key Concepts:**
- **Freezing Point Depression (ΔTf):** A colligative property that describes the decrease in the freezing point of a solvent when a solute is added.
- **Van't Hoff Factor (i):** Represents the number of particles the solute breaks into; for NaCl, i = 2 because it dissociates into two ions.
- **Formula:** ΔTf = i * Kf * m
- **ΔTf:** Freezing point depression
- **Kf:** Freezing point depression constant for water (1.86 °C kg/mol)
- **m:** Molality of the solution (moles of solute per kg of solvent)

Use the information and hints provided to calculate the freezing point depression for the given solution.

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