Why h3o is the strongest acid

I refer you to an acid strength table, for instance, here. Also, I'd like to refer you to this excellent discussion on the matter, where, by the way, orthocresol lent a hand. Sign up to join this community. The best answers are voted up and rise to the top. Stack Overflow for Teams — Collaborate and share knowledge with a private group. Create a free Team What is Teams? Learn more. Ask Question. Asked 5 years, 4 months ago.

Active 5 years ago. Viewed 20k times. Improve this question. Mukul Goyal Mukul Goyal 89 1 1 gold badge 2 2 silver badges 9 9 bronze badges. Sth acts as acid if protonates anything , not necessarily water. I think you mean "something acts as acid towards a compound if it protonates that compound". I guess I should say "something", sorry for imperfection my English. Add a comment. Active Oldest Votes. First of all, please remember that equilibria are dynamic. Everyone, corrections are very welcome!

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A: The mathematical ratio between the species mass and its molar mass will be equivalent to the species All acid—base equilibria favor the side with the weaker acid and base. Thus the proton is bound to the stronger base. Recall from Chapter 4 that the acidic proton in virtually all oxoacids is bonded to one of the oxygen atoms of the oxoanion.

Conversely, the conjugate bases of these strong acids are weaker bases than water. In fact, a 0. Consequently, it is impossible to distinguish between the strengths of acids such as HI and HNO3 in aqueous solution, and an alternative approach must be used to determine their relative acid strengths.

One method is to use a solvent such as anhydrous acetic acid. Measurements of the conductivity of 0. The fully protonated species is always the strongest acid because it is easier to remove a proton from a neutral molecule than from a negatively charged ion. Predict whether the equilibrium for each reaction lies to the left or the right as written.

Identify the conjugate acid—base pairs in each reaction. Equilibrium always favors the formation of the weaker acid—base pair.