When a sample of a hydrated CaBr was heated to a constant weight, 3.24 g of the anhydrous (dry) CaBr was obtained and 1.75 g of water was released. What is the empirical formula of the hydrate? CaBr2.2H₂0 CaBr₂.6H₂0 none of these choices is correct CaBr-12H₂O
When a sample of a hydrated CaBr was heated to a constant weight, 3.24 g of the anhydrous (dry) CaBr was obtained and 1.75 g of water was released. What is the empirical formula of the hydrate? CaBr2.2H₂0 CaBr₂.6H₂0 none of these choices is correct CaBr-12H₂O
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Chapter1: Chemical Foundations
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![**Question:**
When a sample of a hydrated CaBr\(_2\) was heated to a constant weight, 3.24 g of the anhydrous (dry) CaBr\(_2\) was obtained and 1.75 g of water was released. What is the empirical formula of the hydrate?
**Options:**
1. CaBr\(_2 \cdot\) 2H\(_2\)O
2. CaBr\(_2 \cdot\) 6H\(_2\)O
3. None of these choices is correct
4. CaBr\(_2 \cdot\) 12H\(_2\)O
**Explanation:**
The problem involves determining the empirical formula of a hydrate of calcium bromide. The sample was heated, and the water of hydration was removed, resulting in a certain mass of anhydrous CaBr\(_2\) and a known mass of water released. To find the empirical formula of the hydrate, one must calculate the molar ratio of CaBr\(_2\) to H\(_2\)O.
**Steps:**
1. Calculate moles of anhydrous CaBr\(_2\):
\[
\text{Moles of CaBr\(_2\)} = \frac{3.24 \, \text{g}}{199.9 \, \text{g/mol}}
\]
2. Calculate moles of water:
\[
\text{Moles of H\(_2\)O} = \frac{1.75 \, \text{g}}{18.02 \, \text{g/mol}}
\]
3. Determine the ratio of moles of water to moles of CaBr\(_2\).
4. Use this ratio to determine which hydrate formula matches the data.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0c8c77ea-16d7-4384-a2cd-ff8117500861%2Fced919b5-dcd9-4f10-a15b-1ce263e7299e%2F113lb4_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
When a sample of a hydrated CaBr\(_2\) was heated to a constant weight, 3.24 g of the anhydrous (dry) CaBr\(_2\) was obtained and 1.75 g of water was released. What is the empirical formula of the hydrate?
**Options:**
1. CaBr\(_2 \cdot\) 2H\(_2\)O
2. CaBr\(_2 \cdot\) 6H\(_2\)O
3. None of these choices is correct
4. CaBr\(_2 \cdot\) 12H\(_2\)O
**Explanation:**
The problem involves determining the empirical formula of a hydrate of calcium bromide. The sample was heated, and the water of hydration was removed, resulting in a certain mass of anhydrous CaBr\(_2\) and a known mass of water released. To find the empirical formula of the hydrate, one must calculate the molar ratio of CaBr\(_2\) to H\(_2\)O.
**Steps:**
1. Calculate moles of anhydrous CaBr\(_2\):
\[
\text{Moles of CaBr\(_2\)} = \frac{3.24 \, \text{g}}{199.9 \, \text{g/mol}}
\]
2. Calculate moles of water:
\[
\text{Moles of H\(_2\)O} = \frac{1.75 \, \text{g}}{18.02 \, \text{g/mol}}
\]
3. Determine the ratio of moles of water to moles of CaBr\(_2\).
4. Use this ratio to determine which hydrate formula matches the data.
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