Question:
When 2.46 g of a hydrated salt (MSO\(_4 \cdot x\)H\(_2\)O) is completely dehydrated, 1.20 g of anhydrous salt is obtained. If molecular weight of anhydrous salt is 120 g mol\(^{-1}\), find x.
When 2.46 g of a hydrated salt (MSO\(_4 \cdot x\)H\(_2\)O) is completely dehydrated, 1.20 g of anhydrous salt is obtained. If molecular weight of anhydrous salt is 120 g mol\(^{-1}\), find x.
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x = (moles of water) (moles of salt)
Updated On: May 2, 2026
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The Correct Option is C
Solution and Explanation
Concept: Hydrated salts and mole ratio
---
Step 1: Mass of water lost
\[ 2.46 - 1.20 = 1.26 \text{ g} \] ---
Step 2: Moles of anhydrous salt
\[ \frac{1.20}{120} = 0.01 \text{ mol} \] ---
Step 3: Moles of water
\[ \frac{1.26}{18} = 0.07 \text{ mol} \] ---
Step 4: Ratio
\[ x = \frac{0.07}{0.01} = 7 \] --- Final Answer: \[ \boxed{7} \]
---
Step 1: Mass of water lost
\[ 2.46 - 1.20 = 1.26 \text{ g} \] ---
Step 2: Moles of anhydrous salt
\[ \frac{1.20}{120} = 0.01 \text{ mol} \] ---
Step 3: Moles of water
\[ \frac{1.26}{18} = 0.07 \text{ mol} \] ---
Step 4: Ratio
\[ x = \frac{0.07}{0.01} = 7 \] --- Final Answer: \[ \boxed{7} \]
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