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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Question
![**Problem Statement:**
How many milliliters of an aqueous solution of 0.191 M sodium sulfate is needed to obtain 11.7 grams of the salt?
**Input Field:**
- A text box where students can input their answer in milliliters (mL).
**Additional Information:**
- This problem requires knowledge of molarity, molar mass calculations, and the relationship between volume, concentration, and mass. Students should consider the molar mass of sodium sulfate and utilize the formula:
\[
\text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}}
\]
and
\[
\text{Volume (L)} = \frac{\text{Moles}}{\text{Concentration (M)}}
\]
- Students are encouraged to ensure unit conversions where necessary (e.g., converting liters to milliliters).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb692af84-21f3-4e00-9062-ab31ad5014d9%2Fbc06708d-1b36-4980-b8e4-1c43cac66fe2%2Fmfatmai_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
How many milliliters of an aqueous solution of 0.191 M sodium sulfate is needed to obtain 11.7 grams of the salt?
**Input Field:**
- A text box where students can input their answer in milliliters (mL).
**Additional Information:**
- This problem requires knowledge of molarity, molar mass calculations, and the relationship between volume, concentration, and mass. Students should consider the molar mass of sodium sulfate and utilize the formula:
\[
\text{Moles} = \frac{\text{Mass (g)}}{\text{Molar Mass (g/mol)}}
\]
and
\[
\text{Volume (L)} = \frac{\text{Moles}}{\text{Concentration (M)}}
\]
- Students are encouraged to ensure unit conversions where necessary (e.g., converting liters to milliliters).
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