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I would like to clear something up with my understanding about acid or base strength and the pH.
For an acid:
Strength refers to Ka (pKa)
pH refers to concentration of H+ ions
A LOW pH means that there are FREE H+ ions in a solution. So this should mean that BOUND H+ ions RAISE the pH. You get the bound H+ions when there is a base present, right?
So you can be a strong acid (high Ka), but if there is a strong base mopping all that H+ up, then the pH will be higher that what it would be if there was a weaker base instead.
So it's not the act of giving your proton away that makes you a good pH lowerer, but you must factor in the quality of base in the environment too.
IF this is all true, H3O+ is BOUND hydrogen ion to water, but we take this as the FREE H+ ion. Why is that?
For an acid:
Strength refers to Ka (pKa)
pH refers to concentration of H+ ions
A LOW pH means that there are FREE H+ ions in a solution. So this should mean that BOUND H+ ions RAISE the pH. You get the bound H+ions when there is a base present, right?
So you can be a strong acid (high Ka), but if there is a strong base mopping all that H+ up, then the pH will be higher that what it would be if there was a weaker base instead.
So it's not the act of giving your proton away that makes you a good pH lowerer, but you must factor in the quality of base in the environment too.
IF this is all true, H3O+ is BOUND hydrogen ion to water, but we take this as the FREE H+ ion. Why is that?