The vapour pressure of a saturated solution of a sparingly soluble salt (A2B3) is 31.8 mm Hg at 40°C. If the vapour pressure of pure water is 31.9 mm Hg, the solubility product (Ksp) of A2B3, at the same temperature is
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Answer:
5.47*10^(-5)
Explanation:
Let stability of A2B2 be 5 moles/litre
A2B2⇌2A++2B−
2s 2s
Ksp=(2s)2×(2s)2=16×s4
Now, PPo−P=Nn=55.564
⇒31.831.9−31.8=55.564s⇒S=0.043 moles/litre
∴Ksp=16×(0.043)4=5.47×10−5
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