H2SO4 → 2H+ + SO42-
Note the production of positively charged hydrogen ions and also the reaction arrow, which only points to the right. All of the reactant (acid) is ionized into product.
Weak Acids
Weak acids do not completely dissociate into their ions in water. For example, HF dissociates into the H+ and F- ions in water, but some HF remains in solution, so it is not a strong acid. There are many more weak acids than strong acids. Most organic acids are weak acids. Here is a partial list, ordered from strongest to weakest.
HO2C2O2H - oxalic acid
H2SO3 - sulfurous acid
HSO4 - - hydrogen sulfate ion
Answers
Answer:
Well, sulfuric acid reacts with water to give TWO equiv of hydronium ions, and ONE equiv sulfate ions…
H2SO4+2H2O(s)→2H3O++SO2−4H2SO4+2H2O(s)→2H3O++SO42−
Explanation:
This is a much more complicated question than it may appear at first sight.
H2SO4 is classified as a strong acid - which in simple terms means that it readily ( and completely) dissociates . When H2SO4 is dissolved in water , only the first dissociation is complete: The equation is
H2SO4(aq) → H+(aq) + HSO4- (aq)
The HSO4- produced is a weak acid that only partially dissociates in water.
It is therefore incorrect to say that :
[H+] = 2 x [H2SO4] The [H+] contributed by the dissociation of HSO4- can be calculated from the Ka of the acid ; Ka = 1.2 x 10-2
To calculate the [H+] from the second dissociation is complicated. But there is a short cut that gives a reasonably close approximation.
Take a 0.25M solution of H2SO4 in water .
From the first complete dissociation , [H+] = 0.25M
To which must be added the [H+] from the second partial dissociation
Short cut methos
Ka = [H+]² / [HSO4-]
1.2*10^-2 = [H+]² / 0.25
[H+]² = 0.25 ( 1.2*10^-2)
[H+]² = 3*10^-3
[H+] = 0.055M
The [H+] of a 0.25M H2SO4 solution = 0.25M + 0.055M = 0.305M
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Answer:
the dilute sulphuric acid present in the glass vessel is in the ionized state;i.e.,the acid is dissociated onto it's ions
Explanation:
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