The chemical formula of hydronium is H3O +.
Equation: H2CrO4 + H2O <=> H3O+ + HCrO4- <=> H3O+ + CrO42-
The pH is a measure of the concentration of H3O+ in a solution. The lower the pH, the higher the concentration of H3O+. This is because of the way it is defined:pH = - log10 [H3O+]or in other words, the pH is the negative logarithm (in base 10) of the concentration of H3O+.Water, and water-based solutions have a special property: if you multiply the concentration of H3O+ and the concentration of OH-, you always get a constant number, no matter what. Mathematically, that is:[H3O+] * [OH-] = 1 x 10-14This also says the the two concentrations are inverselyproportional. So when one is high, the other has to be low.So, getting back to your question, we know the pH of each solution. From that we know the concentration of H3O+. Again, lower the pH, the higher the concentration of H3O+. And since the concentrations of H3O+ and OH- are inversely proportional, when H3O+ is high, the OH- concentration is low. So which solution has the lowest amount of H3O+? That's the one that has the highest pH, and that will also have the highest concentration of OH-.See the Related Questions for more information about pH, acids and bases.
In its most basic form pH = -log[H3O+] where [H3O+] is the concentration of hydrogen ions from the dissociating acid in water (protolyse). pH= -log[H3O+] = -log[2.4*10-10] = 9.6
pH = - log[H3O+]
The chemical formula of hydronium is H3O +.
h3o is a carbonates
H3o+.
H3O is a strong acid.
H2O is a polar molecule; +H3O is even more so.
In neutral solutions, [H3O+] = [H2O].In bases, [OH-] = [H3O+].In bases, [OH-] is greater than [H3O+].In acids, [OH-] is greater than [H3O+].In bases, [OH-] is less than [H3O+].
Hydronium ions have the formula H3O+
A basic solution has more OH- ions A solution with more H3O+ is acidic.
β = 2.3C {Ka[H3O+] / (Ka+[H3O+])2}
The conjugate base for the hydronium ion (H3O+) is indeed water
By definition: pH = -log[H3O+]So pH = -log(7.4*10-9) = 8.13
H3o+