In the lab, a student needs to determine the van't Hoff factor for a deicer in water. Using the same deicer, he prepares six solutions at different concentrations. The freezing point depression constant for water is 1.86 K/m.
In the lab, a student needs to determine the van't Hoff factor for a deicer in water. Using the same deicer, he prepares six solutions at different concentrations. The freezing point depression constant for water is 1.86 K/m.
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
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Freezing Point Depression versus Molality**
**Graph and Equation Analysis**
The above image depicts a graph titled "Freezing point depression versus molality." The graph is a linear plot that shows the relationship between the freezing point depression (ΔTf) of a solution and its molality (m).
- **X-axis (horizontal):** It represents the molality (m) of the solution, ranging from 0 to 5.
- **Y-axis (vertical):** It indicates the freezing point depression (in Kelvin, K), ranging from 0 to 30.
The data points on the graph form a linear pattern, indicating a direct proportionality between the freezing point depression and the molality. The equation of the line, given as y = 6x, represents this relationship where:
- **y:** Freezing point depression (ΔTf)
- **x:** Molality (m)
- **Slope:** 6, meaning for each unit increase in molality, the freezing point depression increases by 6 K.
**Lab Exercise**
In this scenario, a student is required to determine the van't Hoff factor (i) for a deicer dissolved in water. To achieve this, the student prepares six solutions with different molalities.
- **Freezing point depression constant for water (Kf):** 1.86 K·m^-1
**Task:**
Calculate the van’t Hoff factor (i) using the provided data and the freezing point depression equation.
\[ \Delta T_f = i \cdot K_f \cdot m \]
Given that the slope of the line (represented by 6 in the equation y = 6x) is equal to the product \( i \cdot K_f \), solve for \( i \):
\[ 6 = i \cdot 1.86 \]
\[ i = \frac{6}{1.86} \]
**Determine the van't Hoff factor (i):**
\[ i = \boxed{\_\_\_\_} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7eaef044-20a7-420f-b57c-5d0c5f8d0743%2F6ebcb0f0-91d9-4245-9208-55fb94695a80%2Fg8spcug_reoriented.jpeg&w=3840&q=75)
Transcribed Image Text:**Freezing Point Depression versus Molality**
**Graph and Equation Analysis**
The above image depicts a graph titled "Freezing point depression versus molality." The graph is a linear plot that shows the relationship between the freezing point depression (ΔTf) of a solution and its molality (m).
- **X-axis (horizontal):** It represents the molality (m) of the solution, ranging from 0 to 5.
- **Y-axis (vertical):** It indicates the freezing point depression (in Kelvin, K), ranging from 0 to 30.
The data points on the graph form a linear pattern, indicating a direct proportionality between the freezing point depression and the molality. The equation of the line, given as y = 6x, represents this relationship where:
- **y:** Freezing point depression (ΔTf)
- **x:** Molality (m)
- **Slope:** 6, meaning for each unit increase in molality, the freezing point depression increases by 6 K.
**Lab Exercise**
In this scenario, a student is required to determine the van't Hoff factor (i) for a deicer dissolved in water. To achieve this, the student prepares six solutions with different molalities.
- **Freezing point depression constant for water (Kf):** 1.86 K·m^-1
**Task:**
Calculate the van’t Hoff factor (i) using the provided data and the freezing point depression equation.
\[ \Delta T_f = i \cdot K_f \cdot m \]
Given that the slope of the line (represented by 6 in the equation y = 6x) is equal to the product \( i \cdot K_f \), solve for \( i \):
\[ 6 = i \cdot 1.86 \]
\[ i = \frac{6}{1.86} \]
**Determine the van't Hoff factor (i):**
\[ i = \boxed{\_\_\_\_} \]
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