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@Dexter
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acetone pretty polar whereas chcl3 is very less polar so +ve deviation
B.
benzene is non polar whereas methanol has h bonding so +ve deviation
C.
hno3 has intramolecular h bonding whereas with hno3 it forms intermolecular h bonds which are weaker so +ve deviation
D. h bonding b/w h+ of hcl and O of h2o so -ve deviation
however the ques is single correct
so where am i wrong
Chloroform and acetone shows negative deviation
And Any mineral acid with water also shows negative deviation in general
H of CHCl3 is polar enough to form hydrogen bonding with O of acetone
ok makes sense
logic theek hai ?
also wha bout B and C
Logic is simple na.. like for eg HNO3 and H20 yaha to bohot bdhia h-bonding hogi intermolecular forces kafi badh jayege unlike molecules (HNO3 and H20) ke beech me so it will show negative deviation
intramolecular H bonds are stronger tho
But that doesnt prevent it from getting volatile
samjha nahi
how does volatility matter
See intermolecular forces zyada hoge to hamara mixture less volatile ban jayega to less vapour p i.e it is showing negative deviation
And that benzene and methanol one.. tbh i dont remember the exact reason uska positive deviation ka
benzene just gets in the way of h bonding
Yeah makes sense Methanol-Methanol ka to strong H bonding hota hai warna
thats exactly my point
intramolecular forces are stronger
But in the pure HNO3 the H bonding is not significant right?
The h2o hno3 h bonding is way stronger
why
oh nice idea
hmm
i read the theory once again and remembered ion dipole interactions are stronger than h bonds
in C option h2o (dipole) interacts with polar acetone so -ve deviation
+solved @iTeachChem @Real potato
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