Question

Eque molar concentration of HCl acid as well as acetic acid required the same volume in strength of alkali for complete neutralization yet acetic acid is weak are strong ? yes or now why /

Answer 1

When in solution:

HCl -> H+ Cl-

CH3CO-OH -> R-O- + H+

When in solution with a base

NaOH -> Na+ + HO-

We have the overall reaciton with acetic acid as

NaOH + CH3CO-OH -> Na+ -O-CO-CH3 + H2O

the Base will attack the products of the acetic acid ionization and produce water, thus the products of the acid ionization will be removed, this will pull the acetic acid forward to ionization in attempt to maintain equilibrium.

Thus, the strength of the acid doesn't matter.

Answer 2

Essentially:

There will always be base available for the dissociated acetic acid to attack as the Base is strong and completely dissociates in solution. The removal of products from the ionization of the acetic acid in solution will push it more towards ionization in order to maintain its equilibrium.

Answer 3

blah I made an error the Bronsted base will attack the H+ or bronsted acid

Answer 4

In the end acid strength doesn't matter because the base will pull the ionization of Acetic acid forward till it is completely neutralized.

HCl will completely dissociate in solution and just be neutralized the same way.

Also they contain the same amount of protons so both their reactions are 1 to 1

Answer 5

please solve that equation and one other and then send me ok

Answer 6

Sorry that last line I mean they are both monoprotic

Answer 7

I dont follow, you should be able to write the chemical equations on your own. It is very simple with bronsted acid base reactions

Answer 8

In fact the reaction with HCl is almost identical to that of acetic acids reaction equation