Conjugate Acids and Bases
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Conjugate Acids and Bases
Hi, I am just confused on why a strong acid/base has a conjugate weak acid/base. Is this assumption always true?
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Re: Conjugate Acids and Bases
Yes, this assumption is always true. Strong acids must be good proton donors. Thus, their conjugate base must not readily reaccept a proton. Otherwise, the conjugate base would reverse the actions of the acid, rendering it a weak acid. Therefore, the conjugate base of a strong acid must be a weak base as it cannot readily reaccept protons. Likewise, a strong base must have a weak conjugate acid as the acid must not readily re-donate its proton.
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Re: Conjugate Acids and Bases
A strong acid is a good proton donor. A weak acid is an acid that does not dissociate so easily. The strength of a weak acid depends on how much it dissociates: the more it dissociates, the stronger the acid.
Contrastingly, a strong base is a base that breaks apart 100% in solution. a weak base does not break easily in solution.
If a compound such as HCl is considered a strong acid, it is a good proton donor. Thus, there is essentially no tendency for the conjugate base Cl- to reaccept a proton. Therefore, Cl- is a weak base.
In the Bronsted-Lowry definition of acids and bases, a conjugate acid-base pair consists of two substances that differ only by the presence of a proton (H+)
Contrastingly, a strong base is a base that breaks apart 100% in solution. a weak base does not break easily in solution.
If a compound such as HCl is considered a strong acid, it is a good proton donor. Thus, there is essentially no tendency for the conjugate base Cl- to reaccept a proton. Therefore, Cl- is a weak base.
In the Bronsted-Lowry definition of acids and bases, a conjugate acid-base pair consists of two substances that differ only by the presence of a proton (H+)
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