Question

Does the presence of an acid in a water solution affect the pH of the solution?

Answer 1

My word.....

Explanation:

By definition, `pH-="pouvoir hydrogene"`, i.e. `"power of hydrogen"` is equal to `-log_10[H_3O^+]`.

Strong acids gives low to negative `pH` values, depending on the concentration of the acid, and the inherent acid strength. Weaker acids give `pH<7`...

Strong acids protonate the water solvent and give solutions that are stoichiometric in `H_3O^+`...

`HCl(aq) +H_2O(l) rarr H_3O^+ + Cl^-`

A weaker acid will not give such a precipitous drop in `pH`, however, the `pH` will drop somewhat from `7`...the `pH` of `1.0*mol*L^-1` acetic acid is `2.37`.........