Editing Ammonia solution (section)

==Basicity of ammonia in water==
In aqueous solution, ammonia [[deprotonation|deprotonates]] a small fraction of the water to give [[ammonium]] and [[hydroxide]] according to the following [[chemical equilibrium|equilibrium]]:
: NH<sub>3</sub> + H<sub>2</sub>O ⇌ {{chem|NH|4|+}} + OH<sup>−</sup>.
In a 1&nbsp;[[Molar concentration|M]] [[ammonia]] solution, about 0.42% of the ammonia is converted to ammonium, equivalent to pH = 11.63
because [{{chem|NH|4|+}}] = 0.0042&nbsp;M, [OH<sup>−</sup>] = 0.0042&nbsp;M, [NH<sub>3</sub>] = 0.9958&nbsp;M, and pH = 14 + log<sub>10</sub>[OH<sup>−</sup>] = 11.62. The [[Acid dissociation constant#Bases|base ionization constant]] is
: ''K''<sub>b</sub> = {{sfrac|[{{chem|NH|4|+}}][OH<sup>−</sup>]|[NH<sub>3</sub>]}} = 1.77{{e|−5}}.