What is the pKa of #CH_3COOH# and #H_3PO_4#?
1 Answer
Acetic acid is a monoprotic acid, so it only has one
If you are more familiar with its
You can see that phosphoric acid is not monoprotic.
It is polyprotic. It has three protons. So it has three
#"pKa"_1 = 2.16# #"pKa"_2 = 7.21# #"pKa"_3 = 12.32#
Each of its
#"H"_3"PO"_4(aq) rightleftharpoons "H"_2"PO"_4^(-)(aq) + "H"^(+)(aq)#
#"H"_2"PO"_4^(-)(aq) rightleftharpoons "HPO"_4^(2-)(aq) + "H"^(+)(aq)#
#"HPO"_4^(2-)(aq) rightleftharpoons "PO"_4^(3-)(aq) + "H"^(+)(aq)#
Combining all three reactions, we get:
#"H"_3"PO"_4(aq) rightleftharpoons cancel("H"_2"PO"_4^(-)(aq)) + "H"^(+)(aq)#
#cancel("H"_2"PO"_4^(-)(aq)) rightleftharpoons cancel("HPO"_4^(2-)(aq)) + "H"^(+)(aq)#
#cancel("HPO"_4^(2-)(aq)) rightleftharpoons "PO"_4^(3-)(aq) + "H"^(+)(aq)#
#"------------------------------------------------------"#
#color(blue)("H"_3"PO"_4(aq) rightleftharpoons "PO"_4^(3-)(aq) + 3"H"^(+)(aq))#
The full hypothetical one-step dissociation here has the
#color(blue)(K_(a,"one-step") = K_(a1)K_(a2)K_(a3))#
#= (cancel(["H"_2"PO"_4^(-)])["H"^(+)])/(["H"_3"PO"_4])(cancel(["HPO"_4^(2-)])["H"^(+)])/(cancel(["H"_2"PO"_4^(-)]))(["PO"_4^(3-)]["H"^(+)])/(cancel(["HPO"_4^(2-)]))#
#= color(blue)((["PO"_4^(3-)]["H"^(+)]^3)/(["H"_3"PO"_4]))#
#= 10^(-2.16)*10^(-7.21)*10^(-12.32) = 10^(-21.69)#
#= color(blue)(2.04xx10^(-22))#
In other words, the one-step
Hence, its