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:**
How many grams of solute are present in 50.0 ml of a 0.850 M solution of Potassium dichromate (K₂Cr₂O₇)?
---
**Explanation:**
To find the grams of solute, we need to use the formula:
\[ \text{Mass of solute (g)} = \text{Molarity (M)} \times \text{Volume (L)} \times \text{Molar mass of solute (g/mol)} \]
1. **Convert volume from ml to L:**
\[ 50.0 \, \text{ml} = 0.0500 \, \text{L} \]
2. **Calculate the number of moles of K₂Cr₂O₇:**
\[ \text{Moles} = 0.850 \, \text{M} \times 0.0500 \, \text{L} \]
\[ \text{Moles} = 0.0425 \, \text{moles} \]
3. **Calculate the molar mass of K₂Cr₂O₇:**
\- Potassium (K) = 39.10 g/mol
\- Chromium (Cr) = 51.996 g/mol
\- Oxygen (O) = 16.00 g/mol
\[ \text{Molar mass of K₂Cr₂O₇} = (2 \times 39.10) + (2 \times 51.996) + (7 \times 16.00) \]
\[ \text{Molar mass of K₂Cr₂O₇} = 294.18 \, \text{g/mol} \]
4. **Calculate the mass of solute:**
\[ \text{Mass of solute} = 0.0425 \, \text{moles} \times 294.18 \, \text{g/mol} \]
\[ \text{Mass of solute} = 12.50 \, \text{g} \]
Therefore, there are 12.50 grams of potassium dichromate present in 50.0 ml of a 0.850 M solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F081cd3d5-be26-4896-83a7-8d497d45a428%2Fb1a0191a-90dd-4c56-93f2-a759569de5b9%2F8mg9uov_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
How many grams of solute are present in 50.0 ml of a 0.850 M solution of Potassium dichromate (K₂Cr₂O₇)?
---
**Explanation:**
To find the grams of solute, we need to use the formula:
\[ \text{Mass of solute (g)} = \text{Molarity (M)} \times \text{Volume (L)} \times \text{Molar mass of solute (g/mol)} \]
1. **Convert volume from ml to L:**
\[ 50.0 \, \text{ml} = 0.0500 \, \text{L} \]
2. **Calculate the number of moles of K₂Cr₂O₇:**
\[ \text{Moles} = 0.850 \, \text{M} \times 0.0500 \, \text{L} \]
\[ \text{Moles} = 0.0425 \, \text{moles} \]
3. **Calculate the molar mass of K₂Cr₂O₇:**
\- Potassium (K) = 39.10 g/mol
\- Chromium (Cr) = 51.996 g/mol
\- Oxygen (O) = 16.00 g/mol
\[ \text{Molar mass of K₂Cr₂O₇} = (2 \times 39.10) + (2 \times 51.996) + (7 \times 16.00) \]
\[ \text{Molar mass of K₂Cr₂O₇} = 294.18 \, \text{g/mol} \]
4. **Calculate the mass of solute:**
\[ \text{Mass of solute} = 0.0425 \, \text{moles} \times 294.18 \, \text{g/mol} \]
\[ \text{Mass of solute} = 12.50 \, \text{g} \]
Therefore, there are 12.50 grams of potassium dichromate present in 50.0 ml of a 0.850 M solution.
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