I'm so confused... $\ce{HClO}$ is a weak acid. then why is its conjugate base, $\ce{ClO-}$, a weak base in water? shouldn't they be inversely proportional? shouldn't $\ce{ClO-}$, be a strong base?

If $\ce{HClO}$ is a weak acid, that means it does not readily give up a proton and has a strong pull on them. So when it becomes a conjugate base, $\ce{ClO-}$, shouldn't it readily take protons and therefore be a strong base in water?

ALSO, when an acid is dissolved in water, and some of that acid dissociates into $\ce{H3O+}$, is the Kw of water negligible and you only consider the Ka when finding pH? But that confuses me because I thought you use 14, the exponent of Kw when finding pH.

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    $\begingroup$ Hypochlorous acid is stronger acid than water so chlorate is weaker base than hydroxide. $\endgroup$ – Mithoron Jan 30 '15 at 0:55
  • $\begingroup$ Weak acid compared to HCl and many inorganic acids, but not as weak as e.g. acetic acid. $\endgroup$ – Greg Jan 30 '15 at 10:08
  • $\begingroup$ @Greg pKa of HClO is 7.5. pKa of acetic acid is 4.75. clas.sa.ucsb.edu/staff/Resource%20folder/Chem109ABC/… $\endgroup$ – DavePhD Jan 30 '15 at 11:43
  • $\begingroup$ @DavePhD is H3O+ a strong conjugate acid? $\endgroup$ – bonCodigo Nov 19 '17 at 3:43

(Ka)(Kb) = Kw. Some teachers tell their students that the conjugate base of a weak acid is strong but it's not true. What is true is that the stronger the acid, the weaker the conjugate base and vice versa.

Yes to your second question. When calculating the pH of a solution, the hydronium ion concentration is usually controlled by the strongest acid in the solution. This is the case in the type of problems found in lower level chem classes. In a higher level class problems with acids close enough in strength so that both acids matter may be encountered.


It's true that as the strength of an acid goes up, the strength of its conjugate base goes down. For example, hydrochloric acid (pKa -7 or so) is really strong and chloride anion is a really weak base. On the other side of the spectrum, an alkane (pKa ~50) is a very weak acid, but its conjugate base will deprotonate nearly anything. So at the extremes it's clear: strong acid gives weak conjugate base and weak acid gives strong conjugate base.

For compounds with pKa's between 0 and 14, such as hypochlorous acid with an intermediate pKa, both the acid and the conjugate base are weak. We call them "weak" acids because they don't completely dissociate in water. However, their conjugate bases are also "weak" because they're weaker than hydroxide.

It comes down to just how weak do you mean by "weak".

  • $\begingroup$ Ammonia also is weak base and gives weak conjugate acid.So will this follow the same trend as you said for acids $\endgroup$ – Hydrous Caperilla Mar 26 '18 at 11:07

There is a widespread inconsistency in how the terms "weak" and "strong" are used for acids and bases, something I posted about here:
Is there a terminology contradiction about whether the conjugate of a strong acid is a "weak base"?
All sources agree that the strongER the acid, the weakER the conjugate base. However, some sources say that the conjugate of a strong acid is a (very) weak base. Other sources say that the conjugate of a strong acid is too weak to be considered a base, therefore when they say "the conjugate of a weak acid is a weak base", they mean that the conjugate of a strong acid is not a base at all.

Google turns up dozens of sources which say "the conjugate of a strong base is a weak acid" (or something similar), and also dozens of other sources which say "the conjugate of a weak acid is a weak base" (or something similar). Taken at face value, these statements contradict each other -- if there is at least one strong base whose conjugate is a weak acid, then it cannot be true that the conjugate of a weak acid is always a weak base.

Nonetheless, despite this inconsistency, most sources agree that a weak acid and a weak base can be conjugates of each other, e.g. the weak base $\ce{NH3}$ and the weak acid $\ce{NH4+}$.


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