ON adding more solid solute to a solution,does solution will freeze more rapidly ?
Please tell me about it , I am very confused it should not more rapidly freeze a/c to me
Due to colligative properties of solutions there is depression of freezing point of solution in comparison with pure solvent. It means that the freezing point of a pure solvent is lowered by the addition of a solute. Mathematical law for this phenomenon is ΔTF=KF·b·i (for ideal solutions) where ΔTF – the freezing point depression, ΔTF =TF (pure solvent) TF (solution). KF – the cryoscopic constant, which is dependent on the properties of the solvent. b – the molality (mol solute per kg of solvent) i – the van 't Hoff factor (number of ion particles per individual molecule of solute). For a more accurate calculation at a higher concentration, equation proposed by Ge and Wang should be used. It includes activity of solute which depends on concentration. So more solid solution – more freezing point depression and the time for crystallization of such solution will be increased. Answer: solution will not freeze more rapidly because you should cool it to lower temperature
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Which of the following substances is good reducing agent? a. HI b.KBr c.FeCl3 d.KClO3 Please tell me its answer. I have a doubt why KBr or KClO3 are not good reducing agent than HI . thank you very much
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