If $ceHClO$ is a weak acid, that method it does not readily provide up a proton and also has a solid pull top top them. So once it becomes a conjugate base, $ceClO-$, shouldn"t the readily take protons and also therefore be a solid base in water?
ALSO,when an acid is liquified in water, and some that that acid dissociates into $ceH3O+$, is the Kw of water negligible and you only take into consideration the Ka once finding pH? however that confuses me because I believed you use 14, the exponent that Kw once finding pH.
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$K_mathrm a imes K_mathrm b = K_mathrm w$. Some teachers tell your students that the conjugate base of a weak mountain is strong but it"s not true. What is true is that the more powerful the acid, the weaker the conjugate base and vice versa.
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Yes come your second question. When calculating the pH the a solution, the hydronium ion concentration is usually managed by the strongest acid in the solution. This is the situation in the type of troubles found in lower level chem classes. In a greater level class problems v acids close enough in strength so the both acids issue may be encountered.
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Brinn BelyeaBrinn Belyea
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It"s true that together the stamin of an acid goes up, the strength of that conjugate base goes down. Because that example, hydrochloric mountain ($mathrmpK_mathrma approx -7$) is really solid and chloride anion is a yes, really weak base. On the other side the the spectrum, an alkane ($mathrmpK_mathrma approx 50$) is a an extremely weak acid, but its conjugate base will deprotonate almost anything. So in ~ the extremes it"s clear: solid acid offers weak conjugate base and also weak mountain gives strong conjugate base.
For compounds with $mathrmpK_mathrma$"s in between 0 and 14, such together hypochlorous acid with an intermediate $mathrmpK_mathrma$, both the acid and also the conjugate base room weak. We call them "weak" acids due to the fact that they don"t fully dissociate in water. However, their conjugate bases are likewise "weak" because they"re weaker than hydroxide.
It comes under to just exactly how weak carry out you average by "weak".
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A weak mountain $ceAH$ is in equilibrium through its conjugate basic $ceA-$ when liquified in water:
$$ceAH(aq) A-(aq) + H+(aq)$$
In contrast, a strong acid such together $ceHCl$ dissociates fully, i.e. The adhering to reaction goes come completion:
$$ceHCl(aq) -> Cl-(aq) + H+(aq)$$
Likewise, a solid base such as $ceNaOCH3$ accepts a proton from water, i.e. The complying with reaction goes come completion:
$$ceNaOCH3(aq) + H+(aq) -> CH3OH(aq) + Na+(aq)$$
Neither $ceCl-(aq)$ no one $ceCH3OH(aq)$ are commonly thought that as acid or bases in aqueous solution. They are spectators as far as aqueous acid/base ubraintv-jp.com is concerned.
So the principle of conjugate acid and conjugate base applies only come weak acids and also bases. Saying the a conjugate basic is strong would median that its conjugate acid is no an acid at all but rather a spectator species.
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Said in a confident way, the conjugate basic of a weak mountain is additionally weak since the reaction goes come equilibrium, no to perfect (no matter on which next you start). What you might incorrectly call "the conjugate basic of a strong acid" is really a spectator ion (or molecule).