The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant R. Suppose the osmotic pressure of a certain solution is measured to be 19. atm at an absolute temperature of 386. K. Write an equation that will let you calculate the molarity c of this solution. Your equation should contain only symbols. Be sure you define each symbol other than R. You Gation: Definitions of your symbols: = 19. atm = 386. K olo X E A S ? O olo A
The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant R. Suppose the osmotic pressure of a certain solution is measured to be 19. atm at an absolute temperature of 386. K. Write an equation that will let you calculate the molarity c of this solution. Your equation should contain only symbols. Be sure you define each symbol other than R. You Gation: Definitions of your symbols: = 19. atm = 386. K olo X E A S ? O olo A
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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![**Osmotic Pressure and Molarity Calculation**
The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant \( R \). Suppose the osmotic pressure of a certain solution is measured to be 19. \( \text{atm} \) at an absolute temperature of 386. \( \text{K} \).
**Problem Statement:**
Write an equation that will let you calculate the molarity \( c \) of this solution. Your equation should contain only symbols. Be sure you define each symbol other than \( R \).
**Definitions of Symbols:**
- \( \Pi = 19 \, \text{atm} \) (Osmotic Pressure)
- \( T = 386 \, \text{K} \) (Absolute Temperature)
**Equation:**
\[ \Pi = cRT \]
In this problem, you will need to rearrange the formula to solve for molarity \( c \):
\[ c = \frac{\Pi}{RT} \]
Inserting the given values:
\[ c = \frac{19 \, \text{atm}}{R \times 386 \, \text{K}} \]
This equation will allow you to calculate the molarity \( c \) of the solution. Note that you will need to know the value of the gas constant \( R \) to complete the calculation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cb3c08b-867c-49fa-a9fe-3ee9eddee973%2F3c515fe8-e30c-4226-bbba-2d0d5b81d681%2F5f2o2sm_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Osmotic Pressure and Molarity Calculation**
The osmotic pressure exerted by a solution is equal to the molarity multiplied by the absolute temperature and the gas constant \( R \). Suppose the osmotic pressure of a certain solution is measured to be 19. \( \text{atm} \) at an absolute temperature of 386. \( \text{K} \).
**Problem Statement:**
Write an equation that will let you calculate the molarity \( c \) of this solution. Your equation should contain only symbols. Be sure you define each symbol other than \( R \).
**Definitions of Symbols:**
- \( \Pi = 19 \, \text{atm} \) (Osmotic Pressure)
- \( T = 386 \, \text{K} \) (Absolute Temperature)
**Equation:**
\[ \Pi = cRT \]
In this problem, you will need to rearrange the formula to solve for molarity \( c \):
\[ c = \frac{\Pi}{RT} \]
Inserting the given values:
\[ c = \frac{19 \, \text{atm}}{R \times 386 \, \text{K}} \]
This equation will allow you to calculate the molarity \( c \) of the solution. Note that you will need to know the value of the gas constant \( R \) to complete the calculation.
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