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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2
![**Problem 2: Determining the Mass of Solute**
*Question:*
How many grams of solute are present in 1.65 L of a 0.286 M solution of C₃H₇NO₂?
---
*Explanation:*
To solve this problem, you need to first understand the relationship between molarity (M), volume (L), and moles of solute. Molarity is defined as moles of solute per liter of solution.
1. Calculate the number of moles of C₃H₇NO₂ in the solution using the formula:
\[
\text{Moles of solute} = \text{Molarity (M)} \times \text{Volume (L)}
\]
2. Determine the molar mass of C₃H₇NO₂ by adding the atomic masses of carbon (C), hydrogen (H), nitrogen (N), and oxygen (O) from the periodic table.
3. Using the moles of solute and the molar mass, calculate the mass of the solute using the formula:
\[
\text{Mass (g)} = \text{Moles} \times \text{Molar mass (g/mol)}
\]
This will give you the number of grams of C₃H₇NO₂ in the solution.
Note: No graphs or diagrams are associated with this problem.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F73c907c8-87d1-4587-9999-d2cfccbe64de%2Fb48b6c4a-3650-48fa-ab29-41aa3c5f768d%2F8enotoo_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem 2: Determining the Mass of Solute**
*Question:*
How many grams of solute are present in 1.65 L of a 0.286 M solution of C₃H₇NO₂?
---
*Explanation:*
To solve this problem, you need to first understand the relationship between molarity (M), volume (L), and moles of solute. Molarity is defined as moles of solute per liter of solution.
1. Calculate the number of moles of C₃H₇NO₂ in the solution using the formula:
\[
\text{Moles of solute} = \text{Molarity (M)} \times \text{Volume (L)}
\]
2. Determine the molar mass of C₃H₇NO₂ by adding the atomic masses of carbon (C), hydrogen (H), nitrogen (N), and oxygen (O) from the periodic table.
3. Using the moles of solute and the molar mass, calculate the mass of the solute using the formula:
\[
\text{Mass (g)} = \text{Moles} \times \text{Molar mass (g/mol)}
\]
This will give you the number of grams of C₃H₇NO₂ in the solution.
Note: No graphs or diagrams are associated with this problem.
Expert Solution
Step 1
To calculate the grams of solute first of all e calculate the moles of solute.
The molarity of the solution is defined by the mole of solute present in one liter of solution. The molarity of a solution is calculated by the following formula:
For the given solution:
Molarity of the solution =0.286 M
Mole of solute =?
The volume of the solution = 1.65 L
Step 2
Calculation of mole of sulute:
Step by step
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