When 131. g of glycine (C2H5NO2) are dissolved in 1350. g of a certain mystery liquid X, the freezing point of the solution is 2.00 °C less than the freezing point of pure X. Calculate the mass of iron(III) nitrate (Fe(NO,),) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i=3.04 for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.
When 131. g of glycine (C2H5NO2) are dissolved in 1350. g of a certain mystery liquid X, the freezing point of the solution is 2.00 °C less than the freezing point of pure X. Calculate the mass of iron(III) nitrate (Fe(NO,),) that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i=3.04 for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.
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...
Related questions
Question
100%
![### Freezing Point Depression Calculation
When 131. g of glycine \((C_2H_5NO_2)\) are dissolved in 1350. g of a certain mystery liquid \(X\), the freezing point of the solution is 2.00 °C less than the freezing point of pure \(X\).
**Question:**
Calculate the mass of iron(III) nitrate \((Fe(NO_3)_3)\) that must be dissolved in the same mass of \(X\) to produce the same depression in freezing point. The van't Hoff factor \(i = 3.04\) for iron(III) nitrate in \(X\).
Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.
---
### Solution Steps:
1. **Determine the Molal Freezing Point Depression Constant (\(K_f\))**:
Given data for glycine:
- Mass of glycine = 131. g
- Molar mass of glycine (C₂H₅NO₂) ≈ 75.07 g/mol
- Depression in freezing point = 2.00 °C
Calculate the molality (m):
\[
\text{Molality (m)} = \frac{\text{moles of solute}}{\text{kg of solvent}} = \frac{\frac{131\, \text{g}}{75.07\, \text{g/mol}}}{1.350\, \text{kg}} \approx 1.292 \text{ mol/kg}
\]
Using the freezing point depression equation:
\[
\Delta T_f = K_f \cdot m \implies K_f = \frac{\Delta T_f}{m} = \frac{2.00\, \text{°C}}{1.292\, \text{mol/kg}} \approx 1.548\, \text{°C·kg/mol}
\]
2. **Calculate the Required Mass of \(Fe(NO_3)_3\)**:
- Molar mass of \(Fe(NO_3)_3\) ≈ 241.86 g/mol
- Molality required to produce the same depression: m = \(\frac{2.00 °C}{1.548°C·kg/mol} ≈ 1.292 \text{ mol/kg}\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1067c048-27d4-462b-825c-b686bc07047b%2F357a6ef0-ad32-431d-83b1-53262f52028f%2Fs4wlr5.png&w=3840&q=75)
Transcribed Image Text:### Freezing Point Depression Calculation
When 131. g of glycine \((C_2H_5NO_2)\) are dissolved in 1350. g of a certain mystery liquid \(X\), the freezing point of the solution is 2.00 °C less than the freezing point of pure \(X\).
**Question:**
Calculate the mass of iron(III) nitrate \((Fe(NO_3)_3)\) that must be dissolved in the same mass of \(X\) to produce the same depression in freezing point. The van't Hoff factor \(i = 3.04\) for iron(III) nitrate in \(X\).
Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.
---
### Solution Steps:
1. **Determine the Molal Freezing Point Depression Constant (\(K_f\))**:
Given data for glycine:
- Mass of glycine = 131. g
- Molar mass of glycine (C₂H₅NO₂) ≈ 75.07 g/mol
- Depression in freezing point = 2.00 °C
Calculate the molality (m):
\[
\text{Molality (m)} = \frac{\text{moles of solute}}{\text{kg of solvent}} = \frac{\frac{131\, \text{g}}{75.07\, \text{g/mol}}}{1.350\, \text{kg}} \approx 1.292 \text{ mol/kg}
\]
Using the freezing point depression equation:
\[
\Delta T_f = K_f \cdot m \implies K_f = \frac{\Delta T_f}{m} = \frac{2.00\, \text{°C}}{1.292\, \text{mol/kg}} \approx 1.548\, \text{°C·kg/mol}
\]
2. **Calculate the Required Mass of \(Fe(NO_3)_3\)**:
- Molar mass of \(Fe(NO_3)_3\) ≈ 241.86 g/mol
- Molality required to produce the same depression: m = \(\frac{2.00 °C}{1.548°C·kg/mol} ≈ 1.292 \text{ mol/kg}\
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY