Calculate the solubility of a gas having partial pressure $0.15 \ bar$ at $25^{\circ} C$.
$[K_{H} = 0.16 \ mol \ dm^{-3} \ bar^{-1}]$
$[K_{H} = 0.16 \ mol \ dm^{-3} \ bar^{-1}]$
- A$2.4 \times 10^{-2} \ mol \ dm^{-3}$
- B$3.0 \times 10^{-2} \ mol \ dm^{-3}$
- C$2.7 \times 10^{-2} \ mol \ dm^{-3}$
- D$1.8 \times 10^{-2} \ mol \ dm^{-3}$
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