(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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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: $Ba = 137 \ amu, Cl = 35.5 \ amu$)

Similar Questions

The molecular mass of an organic compound is $108 \ g \ mol^{-1}$. If $C, H,$ and $N$ atoms are present in the weight ratio of $9 : 1 : 3.5$,what is the molecular formula?

An organic compound contains $C = 74.0\%$,$H = 8.65\%$ and $N = 17.3\%$. Its empirical formula is:

$A$ substance contains $38.8\% \, C$,$16\% \, H$,and $45.2\% \, N$. What is the empirical formula of the substance?

The molecular formula of sulphur is

An organic compound has $42.1 \%$ carbon,$6.4 \%$ hydrogen and the remainder is oxygen. If its molecular weight is $342$,then its molecular formula is:

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