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Best Answer - Chosen by Asker In formic acid,H atom hsving I =0 is attached with -COOH group which does not change the ionisation of the acid. But, -CH3 group attached with -COOH group in CH3-COOH has +ve inductive effect and so reduces the ionisation of acetic acid. Hence,formic acid is stronger acid than acetic acid.

The methyl group in acetic acid is electron-donating. This stabilises the induced charge in the carboxyl group, and weakening the strength of the acid. In formic acid, there is only a hydrogen atom, which cannot donate electrons. Hence, the carboxyl group is not stabilised at all, and is a stronger acid.

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because alcohol molecules can overcome the bonds that hold them in a liquid state more than water, therefore, alcohol has a low boiling point

elementary, the bp of most of alcohols are much lower than water. & all other factors remaining const. the rate of evaporation of a liq is inversely proportional to its bp. Because alcohol has low boiling point as compared to water. Diethyl ether will evaporator more quickly than alcohol. Alcohol evaporates faster than water because it is a more volatile molecule than water. Liquid water is a very stable substance because it can hydrogen bond with itself. Alcohol can hydrogen bond with other molecules which have accessible hydrogen bonding atoms (F, O, or N), but because of it's molecular geometry it cannot hydrogen bond with itself. Since most alcohol molecules are very small they are not strongly bound by dispersion forces either and are easily converted to a gaseous state. Alcohol (ethanol) evaporates faster as it has a lower boiling point, (78.4 degrees C). This is due to the fewer hydrogen bonds formed between ethanol molecules, water molecules can form 2 each but ethanol forms one per molecule.

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2 years ago

Best Answer - Chosen by Asker With roughly the same number of carbon atoms and therefore the same number of electrons, the alcohol will have a much higher boiling point. That is because alcohols exhibit some hydrogen bonding due to the H bonded to an O. (R-C-OH) Hydrogen bonds are the intermolecular attractions that occur when the H of one alcohol molecule is attracted to the O of an adjacent alcohol molecule. Ether's on the other hand do not exhibit hydrogen bonding, and therefore have much weaker intermolecular attractions which are due primarily to London dispersion forces. Both the alcohol and the ether, with the same number of electrons, will have about the same strength of London dispersion forces. With the same number of electrons, they will have similar polarizabilities. It is the polarizability of a molecule that determines the magnitude of the London dispersion forces.