We have to remember that to argue that somepoint is even more acidic because it produces more hydronium ions in solution or that it is due to a reduced pKa, while absolutely true, execute not answer the OP"s question of "WHY".

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We have to remember that to argue that something is more acidic bereason it produces even more hydronium ions in solution or that it is because of a reduced pKa, while absolutely true, perform not answer the OP"s question of "WHY".
Of course, but if you tell me it"s not a homejob-related, I ca solution that question also
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If you use the Bronsted-Lowry meaning, you deserve to say that the conjugate bases of both molecules are OH- and also SH-. As oxygen is even more electronegative than sulfur, it will lure electrons more than sulhair does. This means that oxygen will be charged more than sulfur, and it will want to obtain a proton even more than sulfur. Hence, OH- (hydroxide) is a stronger base than SH- (hydrsulfide), which means that H2S is a more powerful acid than H2O. This likewise holds with the Lewis interpretation of an acid.
If you usage the Bronsted-Lowry definition, you have the right to say that the conjugate bases of both molecules are OH- and also SH-. As oxygen is even more electronegative than sulfur, it will tempt electrons even more than sulfur does. This means that oxygen will be charged more than sulfur, and it will certainly want to receive a proton more than sulhair. Hence, OH- (hydroxide) is a more powerful base than SH- (hydrsulfide), which suggests that H2S is a stronger acid than H2O. This additionally holds through the Lewis definition of an acid.
I do not understand this explanation: since oxygen is more electronegative than sulhair, it must retain the extra electron more strongly than sulfur! The factor H2S is even more acid than H2O is in the different bond enthalpies of S-H and O-H.
I don"t understand this explanation: considering that oxygen is even more electronegative than sulhair, it must retain the additional electron more strongly than sulfur! The reason H2S is even more acid than H2O is in the various bond enthalpies of S-H and O-H.
Yes, it will desire to retain the electron more, and also it will hog it towards itself. Oxygen will certainly be even more negatively charged than sulhair once compounded via hydrogen, so it will certainly desire to obtain a proton even more than sulhair (prolots will be attracted more in the direction of oxygen).
I"m surprised that nobody has discussed the duty hydrogen bonding plays in the comparichild of these 2 compounds and also the pH effects that difference leads to.
Yes, it will certainly want to retain the electron even more, and also it will certainly hog it towards itself. Oxygen will be even more negatively charged than sulfur as soon as compounded with hydrogen, so it will desire to get a proton even more than sulhair (prolots will certainly be attracted more towards oxygen).
But the bond between H+ and also OH- is not ionic, is covalent; it indicates that the charge on the ions does not count incredibly a lot, what counts is the capability of developing a covalent bond in between one of the lone pairs on the oxygen and the proton, that is the possibility for the oxygen to *give* a pair of electrons to the H+.
I"m surprised that nobody has stated the role hydrogen bonding plays in the comparichild of these two compounds and also the pH effects that distinction leads to.

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I thought the hydrogen bond were more responsible of properties prefer boiling point and also vaporization enthalpy, but I"d choose to recognize your explacountry.