Why is ammonia not an arrhenius base?

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Why is ammonia not an arrhenius base?

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Answer 1 · 2018-05-27T20:36:07

Well, Arrhenius bases are conceived to be sources of the hydroxide ion in aqueous solution...

Explanation:

And since ammonia does NOT contain hydroxide ions, i.e. its chemical formula is $N H_{3}$ $NH_3$ , it does not fall under the Arrhenius' umbrella. We classify ammonia as a Bronsted-Lowry base...and its conjugate acid is ammonium ion, $N H_{4}^{+}$ $NH_4^+$ ...

$N H_{3} (a q) + H_{2} O (l) ⇌ N H_{4}^{+} + H O^{-}$ $NH_3(aq) + H_2O(l) rightleftharpoonsNH_4^+ + HO^-$

$K_{b} = 1.80 \times 10^{- 5}$ $K_b=1.80xx10^-5$

Note that this is all conceived to occur in AQUEOUS solution, i.e. in a water solvent. In liquid ammonia solvent, and use of this solvent is nowadays fairly standard and straightforward....the following acid-base regime obtains...

$2NH_3(l)rightleftharpoonsunderbrace(NH_2^(-))_"the amide ion" + NH_4^+$

Ammonia has a normal boiling point of $33.3$ $""^@C$ ...
The degree of dissociation can be measured, but I don't my text at hand right now....

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Why is ammonia not an arrhenius base?

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