### 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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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 by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter3: Composition Of Substances And Solutions

Section: Chapter Questions

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Question

### 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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