A sample of $4.88 g$ of hydrated barium chloride, $BaCl X_{2} \cdot x H X_{2} O$ , loses $0.72 g$ of water completely on heating (Ba = 137, Cl = 35.5, O = 16, H = 1). Which of the following statements is/are correct?

Answer: A, B, C

Anhydrous

BaCl X_{2}

= 4.88 - 0.72 = 4.16

= 4.16/208 = 0.0200

mol; water

= 0.72/18 = 0.0400

mol, so

x = 2

. For the hydrate (

M = 244

): Ba

= 137/244 = 56.1%

and Cl

= 71/244 = 29.1%

. The figure 34.1\% is the Cl content of the anhydrous salt (

71/208

), not of the hydrate.