why does 0.05M HCl has a higher concentration of H+ than 0.5M CH3COOH?

Answer 1

HCl fully dissociated in water.
HCl = H+ + Cl-

CH3COOH only partially dissociates. in water.

CH3COOH = ch3cooh + H+ + ch3coo-

The idea being that a large number the hydrogen atoms in CH3COOH remain attached to to the rest of the molecule. Only a few hydrogen ions detach (dissociate) from the rest of the molecule (CH3COO-). Hence as only a few H+'s are in solution than the pH is higher.

Answer 2

0.05M HCl has a higher concentration of H+ ions because it dissociates more fully than CH3COOH. An equilibrium is set up:
HCl <----> H+ + Cl-
where the equilibrium is to the right, but in CH3COOH the equilibrium is set up as follows:
CH3COOH <----> H+ + CH3COO-
and here the equilibrium is further to the left, with fewer H+ ions.

Answer 3

HCl is a mineral acid. This means that it is made of inorganic ions which dissociate ( ionise) rapidly in water to give a large conc of H+ ions.

EG: HCl +H20 --->2H+ + OH- + Cl-

Acetic acid CH3COOH is an organic acid. It doesn't ionise as well because the charge on ions are not as pronounced.. ( This is a thumb rule.)

Hence dilute soln. of HCl has a higher conc of H+ ions

Answer 4

HCl diassociates almost completely when in solution where as CH3COOH only partialy disassociates into ions when in solution. The more dissasociation the greater the acidity of the solution. (This is a very simplistic view altough id be here forever explaining the full reason as im rubbish at explaning

Answer 5

HCl is a strong acid; it ionizes completely (or close enough) in water. CH3COOH is a weak acid, it does not ionize completely, and therefore gives off fewer H+ ions per unit of Molarity.

Answer 6

HCl disassociates more readily in water and leads to higher conc. of H+ ions