(D) Mass of hydrated salt = $61 \ g$ Mass of anhydrous $BaCl_2$ = $52 \ g$ Mass of water lost = $61 \ g - 52 \ g = 9 \ g$ Molar mass of $BaCl_2 = 137

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(D) Mass of hydrated salt = $61 \ g$ Mass of anhydrous $BaCl_2$ = $52 \ g$ Mass of water lost = $61 \ g - 52 \ g = 9 \ g$ Molar mass of $BaCl_2 = 137 + 2 \times 35.5 = 208 \ g/mol$ Molar mass of $H_2O = 18 \ g/mol$ Moles of $BaCl_2 = \frac{52}{208} = 0.25 \ mol$ Moles of $H_2O = \frac{9}{18} = 0.5 \ mol$ Ratio of moles of $H_2O$ to $BaCl_2 = \frac{0.5}{0.25} = 2$ Therefore,the formula is $BaCl_2 \cdot 2H_2O$.

Class 11 Chemistry Some Basic Concepts of Chemistry Percentage composition and Molecular formula

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$A$ sample of a hydrate of barium chloride weighing $61 \ g$ was heated until all the water of hydration was removed. The dried sample weight is $52 \ g$. The formula of the hydrated salt is: (atomic mass: $Ba = 137 \ amu, Cl = 35.5 \ amu$)

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A
$BaCl_2 \cdot 4H_2O$
B
$BaCl_2 \cdot 3H_2O$
C
$BaCl_2 \cdot H_2O$
D
$BaCl_2 \cdot 2H_2O$

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$A$ sample of a hydrate of barium chloride weighing $61 \ g$ was heated until all the water of hydration was removed. The dried sample weight is $52 \ g$. The formula of the hydrated salt is: (atomic mass: $Ba = 137 \ amu, Cl = 35.5 \ amu$)

Similar Questions

The molecular mass of caffeine is $194 \, a.m.u.$. It contains $28.9 \%$ of nitrogen by mass. The number of nitrogen atoms in one molecule of caffeine is ...............

Insulin contains $3.4\%$ sulphur. The minimum molecular weight of insulin is

$A$ compound possesses $8\%$ sulphur by mass. The least molecular mass is

Analysis of a $60 \, g$ compound gives $C = 24 \, g$,$H = 4 \, g$,and $O = 32 \, g$. What is its empirical formula?

$A$ sample of calcium carbonate $(CaCO_3)$ has the following percentage composition: $Ca = 40\%$; $C = 12\%$; $O = 48\%$. If the law of constant proportions is true,then the weight of calcium in $4 \, g$ of a sample of calcium carbonate obtained from another source will be $... \, g$.

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