pH for strong acids

[Libby Stafford 1L]

How do we calculate pH for strong acids when we don't have an equilibrium constant to find the product of the two products?

[Chem_Mod]

Strong acids don't have a Ka value since the acid is assumed to have dissociated almost completely. For these problems, use the pH = -log[H+] equation to find pH.

[Chris Korban 1D]

Because strong acids don't have an equilibrium constant due to complete dissociation, you must use ph=-log[H+] and this uses the concentration of protons in the reaction and it allows to calculate the ph of the acid which should be pretty low if its a strong acid

[Rainy Liu Ruoshui_2K]

HA -----> H+ + A-. Thus, it does not have an equilibrium constant because it is totally deprotonated. Thus, the pH of a strong acid is a given number and we don't need to calculate it.

[cnyland]

Because we assume that strong acids have completely dissociated, there is no equilibrium constant or Ka value, so you would just use the pH equation that Dr. Lavelle gave us during lecture!

[Janys Li - 1L]

Hi,

Strong acids are assumed to dissociate completely. They do not have a Ka value because [H+][A-]/[HA] would have 0 in the denominator, which makes the number infinitely large.

[Jelix Tsan 2H]

For strong acids, pH is simply calculated by taking the negative log of the H+ concentration that results from the acids, and this is easy to deduce because strong acids are assumed to dissociate 100%.