Calculate the boiling point of a solution containing 0.456 g of camphor (molar mass 152) dissolved in 31.4 gm of acetone (b.pt = 56.30
c.if molal elevation constant per 100 gm of acetone is 17.2 c
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Answer:The boiling point of the solution is .
Explanation:
Weight of solvent(acetone) = 31.4 g
Molar mass of camphor = 152 g/mol
Mass of camphor added = 0.456 g
per 100 gram of solvent
The boiling point of the solution is .
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