Why do strong and weak acids ionise in the same mole ratio?

For example, 1 mole of hydrochloric acid, which fully ionises, produces one mole of hydrogen ions. One mole of acetic acid, which ionises at about 1% also produces one mole of hydrogen ions. I don't see the sense in this. I figure a mole of acetic acid will consist of less molecules than a mole of HCl (and therefore less Hydrogen), and of these, 99% will fail to decompose. Yet, still, equal quantities produce the same amount of hydrogen ions. What is the piece of logic my brain is missing in understanding this?

Thanks in advance for any help.

Answer:
Those acids are stronger which has greater capacity to give H oins in aquas form. In balenced chemical equations we see that each acid gives one mole of H gass as you mentioned. but what hapens actualy? in reality the acetate oin CH3COO formed is less stable than Cl oin. Thats why in acetic acid these CH3COO oin combine with free H oins to produce CH3COOH again. decreasing the power of an acid. CH3COO is the conjugate base of CH3COOH. stable will be the conjugate base of an acid, greater will be its streangth to give H oins in aquas form.
Moles is a quantity of RATIO not of actual amount. Technically there will be less Hydogen but the ratio of hydrogen in HCl of Hydrogen to Chlorine in the same as the ratio of moles of Hyrdogen to Oxygen in Hydroxide (OH). This is also to say the Bromic acid HBr2 has 2 moles of Bromide to every 1 mole of Hydrogen. See? You are thinking on CONCENTRATION...which is to say that the concentration of hydrogen in the HCl will be greater than in the acetic acid which is much weaker.
There is an equilibrium reaction involved with regards to the acetic acid dissociation in water

CH3COOH -----------> H+ + CH3COO-
<-----------

I just think you're overanalyzing it... If you think in concentration, the moles of H+ of acetic acid in water will be lower than that of the H+ from HCl, but with the chemical equation such as what's above, where you do not indicate concentration, you'd be lost if you think of concentrations.

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