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Which of the following solutions would have the highest Freezing Point? (assume ideal dissociation for electrolytes) 0.15 m Glucose (non-electrolyte) O 0.10 m NaCl O 0.10 m MgCl₂ O 0.10 m Na3PO4

Which of the following solutions would have the highest Freezing Point? (assume ideal dissociation for electrolytes) 0.15 m Glucose (non-electrolyte) O 0.10 m NaCl O 0.10 m MgCl₂ O 0.10 m Na3PO4

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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
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**Question: Freezing Point of Solutions** **Which of the following solutions would have the highest Freezing Point? (assume ideal dissociation for electrolytes)** - O 0.15 m Glucose (non-electrolyte) - O 0.10 m NaCl - O 0.10 m MgCl₂ - O 0.10 m Na₃PO₄ **Explanation:** In general, the freezing point of a solution is lower than that of the pure solvent. This phenomenon is known as freezing point depression. It is dependent on the number of particles present in the solution rather than their nature. For non-electrolytes, the number of particles in the solution only depends on its molarity. However, for electrolytes, which dissociate in water, the number of particles also depends on the degree of dissociation. For the provided solutions: 1. **0.15 m Glucose (non-electrolyte)**: Glucose does not dissociate in solution, so the number of particles remains 0.15 m. 2. **0.10 m NaCl**: Sodium chloride (NaCl) dissociates into 2 ions (Na⁺ and Cl⁻), leading to a total concentration of particles = 0.10 m * 2 = 0.20 m. 3. **0.10 m MgCl₂**: Magnesium chloride (MgCl₂) dissociates into 3 ions (Mg²⁺ and 2 Cl⁻), leading to a total concentration of particles = 0.10 m * 3 = 0.30 m. 4. **0.10 m Na₃PO₄**: Sodium phosphate (Na₃PO₄) dissociates into 4 ions (3 Na⁺ and PO₄³⁻), leading to a total concentration of particles = 0.10 m * 4 = 0.40 m. Based on the above information, the solution with the fewest particles in solution has the highest freezing point. Therefore, the answer is **0.15 m Glucose (non-electrolyte)** since it has the highest freezing point among the options provided.
Transcribed Image Text:**Question: Freezing Point of Solutions** **Which of the following solutions would have the highest Freezing Point? (assume ideal dissociation for electrolytes)** - O 0.15 m Glucose (non-electrolyte) - O 0.10 m NaCl - O 0.10 m MgCl₂ - O 0.10 m Na₃PO₄ **Explanation:** In general, the freezing point of a solution is lower than that of the pure solvent. This phenomenon is known as freezing point depression. It is dependent on the number of particles present in the solution rather than their nature. For non-electrolytes, the number of particles in the solution only depends on its molarity. However, for electrolytes, which dissociate in water, the number of particles also depends on the degree of dissociation. For the provided solutions: 1. **0.15 m Glucose (non-electrolyte)**: Glucose does not dissociate in solution, so the number of particles remains 0.15 m. 2. **0.10 m NaCl**: Sodium chloride (NaCl) dissociates into 2 ions (Na⁺ and Cl⁻), leading to a total concentration of particles = 0.10 m * 2 = 0.20 m. 3. **0.10 m MgCl₂**: Magnesium chloride (MgCl₂) dissociates into 3 ions (Mg²⁺ and 2 Cl⁻), leading to a total concentration of particles = 0.10 m * 3 = 0.30 m. 4. **0.10 m Na₃PO₄**: Sodium phosphate (Na₃PO₄) dissociates into 4 ions (3 Na⁺ and PO₄³⁻), leading to a total concentration of particles = 0.10 m * 4 = 0.40 m. Based on the above information, the solution with the fewest particles in solution has the highest freezing point. Therefore, the answer is **0.15 m Glucose (non-electrolyte)** since it has the highest freezing point among the options provided.
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