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True. Ethanol does on a molecule by molecule basis have stronger intermolecular forces between itself and water than methanol and water. and more soluble in water than methanol. False. Yet, my chemistry textbook says that both ethanol and methanol are miscible in water, but the more the carbon chain increases, the less miscible it becomes. True.
Oxygen is much more electronegative than hydrogen, so oxygen has to attract the electron pair towards itself forming a polar compound. This means it should have to disassociate into ions in aqueous solution and conduct electricity but it doesn't. In some other posts of the same site mentions, why ethanol doesn't disassociate much in water, but ...
Non-polar Solute and Solvent. For the solute to dissolve, the dispersion forces between the molecules in the solute and solvent need to break. This only requires very little energy. However when the solute dissolves into the solvent, they are able to be make dispersion forces with each other. The making of these forces releases very little energy.
Ethanol is a polar molecule. Ethanol's chemical formula is CH 3 CH 2 OH. The electronegativity difference between carbon (2.55) and hydrogen (2.20) is...
Your ethanol is a polar, protic solvent because the hydroxyl is capable of hydrogen bonding or donating the proton (its Bronsted-Lowry acidity is about that of water, pKa 15.7 vs 16). DMSO is a polar, aprotic solvent because it does not contain hydrogens that can H-bond nor are (appreciably) acidic.
0. It is true that acetone is less polar than ethanol. I thought the dipole moment is proportional to polarity, and if so, the dipole moment of acetone should be lower than ethanol. But the dipole moment of acetone is higher than ethanol. Why is it higher? Regarding your statement about differences in polarity, did you consider differences in ...
It is not uncommon that organic compounds with polar substituents are less soluble in higher alkanols. Vanillin is a typical example, the solubilities are in the range of 4.15 mol/L in methanol, 2.5 mol/L in ethanol and 1.8 mol/L in 1-propanol.
11. Solomons and Fryhle has an example in which they have showed a very simple substitution reaction. The question was to synthesize methyl iodide. What they have done is taken methyl chloride and produced methyl iodide in the presence of NaI N a I and ethanol through an SN2 S N 2 mechanism. Why did they use ethanol?
6. When you say "phenol is more polar than alcohol", how are you quantifying polarity? Phenol has only moderate solubility in water, while ethanol and other small alcohols are infinitely miscible. Several small alcohols also have an appreciably higher dipole moment (~1.6 D) compared to phenol (1.2 D). – Nicolau Saker Neto.
The order must be HCl > Ethanol > hexane > benzene. It is because benzene is a perfectly symmetrical molecule and dipole moment vectors cancel each other completely. But hexane is not that symmetric and hence there is a dipole moment due to difference in electronegativity of C and H atoms (but it is almost negligible).