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

Question

A sample of a hydrate of barium chloride weighing 61 g was heated until all the water of hydration is removed. The dried sample weighed 52 g. The formula of the hydrated salt is: (atomic mass, Ba = 137 amu. Cl = 35.5 amu) (A) BaCl 2 ⋅ H 2 O (B) BaCl 2 ⋅ 2 H 2 O (C) BaCl 2 ⋅ 3 H 2 O (D) BaCl 2 ⋅ 4 H 2 O

Tardigrade Admin · Accepted Answer

underset61 gmBaCl 2 ⋅ xH 2 O arrow underset52BaCl 2 + underset9 gmxH 2 O 52 gm CaCl 2 combines with 9 gm H 2 O 208 gm BaCl 2 combines with 36 gm H 2 O nH2O=(36/18)=2 So the formula will be, BaCl 2 ⋅ 2 H 2 O

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

$B a C l_{2} \cdot H_{2} O$

$B a C l_{2} \cdot 2 H_{2} O$

$B a C l_{2} \cdot 3 H_{2} O$

$B a C l_{2} \cdot 4 H_{2} O$

$61 g m B a C l_{2} \cdot x H_{2} O \to 52 B a C l_{2} + 9 g m x H_{2} O$

$52 g m C a C l_{2}$ combines with $9 g m H_{2} O$

$208 g m B a C l_{2}$ combines with $36 g m H_{2} O$

$n_{H_{2} O} = \frac{36}{18} = 2$

So the formula will be, $B a C l_{2} \cdot 2 H_{2} O$

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

BaCl2​⋅H2​O

BaCl2​⋅2H2​O

BaCl2​⋅3H2​O

BaCl2​⋅4H2​O