The pOH is 6,4.
In pure water, the product [H+][OH-]=10-14 mol2, so, if pH=4, then pOH=10
pH = 1 - pOH
pH refers to the “potential of hydrogen”. It can be used to determine whether a solution is acidic, basic or neutral. In contrast, pOH is a measure of hydroxide ion (OH –) concentration. The key difference between pH and pOH is that pH is a measure of hydrogen ions whereas pOH is a measure of hydroxide ions.
pOh=14-pH
(apex)
4.7 as the pH of ammonia is 9.3 and the pH + the pOH of a substance always equals 14.
pH + pOH = 14. So pOH = 14 - 10.95 = 3.05 pOH = -log[OH-] [OH-] = 8.91 x 10-4 M
The pOH is 6,4.
The pOH is 6,4.
pH = 1 HCl is a strong acid so fully dissociates, so the concentration of H+ is equal to that of the HCl and pH=-log[H+]
pH plus pOH equals 14.
4.7 as the pH of ammonia is 9.3 and the pH + the pOH of a substance always equals 14.
pH + pOH = 14. So pOH = 14 - 10.95 = 3.05 pOH = -log[OH-] [OH-] = 8.91 x 10-4 M
Yes, if both solutions are at 25oC then in both solutions this is valid: pH + pOH = 14.0
The pOH is 6,4.
pH + pOH =14
The pOH is 6,4.
It will have a pOH of 12. Because pH+pOH=14
pH is -log[H(subscript 3)O+] pOH is the [OH-] pOH = 14 - pH apex
pH + pOH =14
pH = 1 HCl is a strong acid so fully dissociates, so the concentration of H+ is equal to that of the HCl and pH=-log[H+]
I will assume you are asking about the pH of pure water if pKw is 14.26. The relationship between pH, pOH, and pKw is as follows: pH + pOH = pKw. If it is pure, neutral water (no acids or bases present), then pH = pOH, so: pH + pOH = 14.26 2(pH) = 14.26 pH = pOH = 7.13