Q1. In an experiment, 10.0-grams of an unknown calcium nitrate hydrate is heated to drive off all of the water of hydration. After heating, 6.95-grams of anhydrous calcium nitrate remain. Find the hydrate formula.
Q1. In an experiment, 10.0-grams of an unknown calcium nitrate hydrate is heated to drive off all of the water of hydration. After heating, 6.95-grams of anhydrous calcium nitrate remain. Find the hydrate formula.
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
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![### Hydrate Formula Problems and Error Analysis
**Q1. Hydrate Formula Calculation**
**Problem Statement:**
In an experiment, 10.0 grams of an unknown calcium nitrate hydrate is heated to drive off all of the water of hydration. After heating, 6.95 grams of anhydrous calcium nitrate remain. Find the hydrate formula.
**Solution Approach:**
To find the hydrate formula of calcium nitrate, follow these steps:
1. **Determine the mass of water lost:**
\[ \text{Mass of water lost} = \text{Mass of hydrated sample} - \text{Mass of anhydrous sample} \]
\[ \text{Mass of water lost} = 10.0 \, \text{g} - 6.95 \, \text{g} \]
\[ \text{Mass of water lost} = 3.05 \, \text{g} \]
2. **Calculate the moles of anhydrous calcium nitrate (Ca(NO\(_3\))\(_2\)):**
\[ \text{Molar mass of Ca(NO\(_3\))\(_2\)} = 40.08 + 2 \times (14.01 + 3 \times 16.00) \]
\[ \text{Molar mass of Ca(NO\(_3\))\(_2\)} = 164.10 \, \text{g/mol} \]
\[ \text{Moles of Ca(NO\(_3\))\(_2\)} = \frac{6.95 \, \text{g}}{164.10 \, \text{g/mol}} \]
\[ \text{Moles of Ca(NO\(_3\))\(_2\)} \approx 0.0423 \, \text{mol} \]
3. **Calculate the moles of water (H\(_2\)O):**
\[ \text{Molar mass of H\(_2\)O} = 2 \times 1.01 + 16.00 = 18.02 \, \text{g/mol} \]
\[ \text{Moles of H\(_2\)O} = \frac{3.05 \, \text{g}}{18.02 \, \text{g](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F793b6aff-f148-4523-8250-7b38a941d7e6%2F974f7e18-10a4-4215-b624-28afcc092b7c%2Fq6wxobm_processed.png&w=3840&q=75)
Transcribed Image Text:### Hydrate Formula Problems and Error Analysis
**Q1. Hydrate Formula Calculation**
**Problem Statement:**
In an experiment, 10.0 grams of an unknown calcium nitrate hydrate is heated to drive off all of the water of hydration. After heating, 6.95 grams of anhydrous calcium nitrate remain. Find the hydrate formula.
**Solution Approach:**
To find the hydrate formula of calcium nitrate, follow these steps:
1. **Determine the mass of water lost:**
\[ \text{Mass of water lost} = \text{Mass of hydrated sample} - \text{Mass of anhydrous sample} \]
\[ \text{Mass of water lost} = 10.0 \, \text{g} - 6.95 \, \text{g} \]
\[ \text{Mass of water lost} = 3.05 \, \text{g} \]
2. **Calculate the moles of anhydrous calcium nitrate (Ca(NO\(_3\))\(_2\)):**
\[ \text{Molar mass of Ca(NO\(_3\))\(_2\)} = 40.08 + 2 \times (14.01 + 3 \times 16.00) \]
\[ \text{Molar mass of Ca(NO\(_3\))\(_2\)} = 164.10 \, \text{g/mol} \]
\[ \text{Moles of Ca(NO\(_3\))\(_2\)} = \frac{6.95 \, \text{g}}{164.10 \, \text{g/mol}} \]
\[ \text{Moles of Ca(NO\(_3\))\(_2\)} \approx 0.0423 \, \text{mol} \]
3. **Calculate the moles of water (H\(_2\)O):**
\[ \text{Molar mass of H\(_2\)O} = 2 \times 1.01 + 16.00 = 18.02 \, \text{g/mol} \]
\[ \text{Moles of H\(_2\)O} = \frac{3.05 \, \text{g}}{18.02 \, \text{g
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