Homework Help is Here – Start Your Trial Now!
Science
Chemistry
16.456 g of ethylamine (MM = 45.08 g/mol) are dissolved and diluted with water to 175.00 ml. Calculate the molarity of the ethylamine.

16.456 g of ethylamine (MM = 45.08 g/mol) are dissolved and diluted with water to 175.00 ml. Calculate the molarity of the ethylamine.

Chemistry
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...
See similar textbooks
icon
Related questions
Question
**Calculation of Molarity of Ethylamine** To determine the molarity of ethylamine, use the following information: - Amount of ethylamine: 16.456 g - Molar mass (MM) of ethylamine: 45.08 g/mol - Volume of the solution after dilution: 175.00 mL **Calculation:** 1. **Convert the volume from milliliters to liters:** \[ 175.00 \text{ mL} = 0.17500 \text{ L} \] 2. **Calculate the moles of ethylamine:** \[ \text{Moles of ethylamine} = \frac{\text{mass}}{\text{molar mass}} = \frac{16.456 \text{ g}}{45.08 \text{ g/mol}} = 0.3648 \text{ mol} \] 3. **Calculate the molarity (M):** \[ M = \frac{\text{moles of solute}}{\text{liters of solution}} = \frac{0.3648 \text{ mol}}{0.17500 \text{ L}} = 2.084 \text{ M} \] Thus, the molarity of the ethylamine solution is 2.084 M.
Transcribed Image Text:**Calculation of Molarity of Ethylamine** To determine the molarity of ethylamine, use the following information: - Amount of ethylamine: 16.456 g - Molar mass (MM) of ethylamine: 45.08 g/mol - Volume of the solution after dilution: 175.00 mL **Calculation:** 1. **Convert the volume from milliliters to liters:** \[ 175.00 \text{ mL} = 0.17500 \text{ L} \] 2. **Calculate the moles of ethylamine:** \[ \text{Moles of ethylamine} = \frac{\text{mass}}{\text{molar mass}} = \frac{16.456 \text{ g}}{45.08 \text{ g/mol}} = 0.3648 \text{ mol} \] 3. **Calculate the molarity (M):** \[ M = \frac{\text{moles of solute}}{\text{liters of solution}} = \frac{0.3648 \text{ mol}}{0.17500 \text{ L}} = 2.084 \text{ M} \] Thus, the molarity of the ethylamine solution is 2.084 M.
Expert Solution
steps

Step by step

Solved in 2 steps with 2 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Solutions
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.
Similar questions
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS