The solubility of B a S O 4 in water is 2.42 × 1 0 - 3 g L - 1 at 298 K. The value of its solubility product ( K s p ) will be (Given molar mass of B a S O 4 = 233 g m o l - 1 )

Question

The solubility of B a S O 4 in water is 2.42 × 1 0 - 3 g L - 1 at 298 K. The value of its solubility product ( K s p ) will be (Given molar mass of B a S O 4 = 233 g m o l - 1 ), 1.08 × 1 0 - 14 m o l 2 L - 2, 1.08 × 1 0 - 12 m o l 2 L - 2, 1.08 × 1 0 - 10 m o l 2 L - 2, 1.08 × 1 0 - 8 m o l 2 L - 2

MARKS App · Accepted Answer

Solubility of BaSO 4 , s = 2.42 × 10 − 3 233 molL − 1 = 1.04 × 1 0 - 5 ( m o l L - 1 ) BaSO 4 s ⇌ Ba 2 + s aq + SO 4 2 − s sq K s p = [ B a 2 + ] [ S O 4 2 - ] = s 2 = ( 1.04 × 1 0 - 5 ) 2 = 1.08 × 1 0 - 10 m o l 2 L - 2

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