!! LONG ANSWER !!
If you want the concentration of all the species present in solution, you'll need the acid dissociation constants for phosphoric acid's second and third ionizations.
These are listed as being
K_(a2) = 6.2 * 10^(-8)Ka2=6.2⋅10−8 and K_(a3) = 4.2 * 10^(-13)Ka3=4.2⋅10−13.
As you can see, these acid dissociation constants have very, very small values, which is why only the first ionization of phophoric acid is usually taken into consideration in pH calculations.
So, the first equilibrium reaction that is established in solution will be
" "H_3PO_(4(aq)) + H_2O_((l)) rightleftharpoons H_3O_((aq))^(+) + H_2PO_(4(aq))^(-) H3PO4(aq)+H2O(l)⇌H3O+(aq)+H2PO−4(aq),
I.......0.02.........................................0......................0
C......(-x)..........................................(+x)..................(+x)
E...0.02-x.........................................x........................x
By definition, the acid dissociation constant is
K_(a1) = ([H_3O^(+)] * [H_2PO_4^(-)])/([H_3PO_4]) = (x * x)/(0.02- x) = x^2/(0.02 - x)Ka1=[H3O+]⋅[H2PO−4][H3PO4]=x⋅x0.02−x=x20.02−x
Solving for xx will produce a positive and a negative solution. Since xx represents concentration, the negative solution is automatically eliminated., which leaves x = 0.009060.
As a result, [H_3O^(+)] = [H_2PO_4^(-)] = "0.009060 M"[H3O+]=[H2PO−4]=0.009060 M
Now for the second equilibrium reaction
" "H_2PO_(4(aq))^(-) + H_2O_((l)) rightleftharpoons H_3O_((aq))^(+) + HPO_(4(aq))^(2-) H2PO−4(aq)+H2O(l)⇌H3O+(aq)+HPO2−4(aq)
I...0.009060..............................0.00906............0
C......(-x)..........................................(+x)...............(+x)
E...0.009060-x.......................0.009060+x.......x
K_(a2) = ([H_3O^(+)] * [HPO_4^(2-)])/([H2PO_4^(-)]) = [(0.009060 + x) * x]/(0.009060-x)Ka2=[H3O+]⋅[HPO2−4][H2PO−4]=(0.009060+x)⋅x0.009060−x
Because the second acid dissociation constant is so small, you can approximate 0.009060 + x and 0.009060 - x with 0.009060. The above equation becomes
6.2 * 10^(-8) = (cancel(0.009060) * x)/cancel(0.009060) = x
As a result, [HPO_4^(2-)] = 6.2 * 10^(-8)"M"
[H_3O^(+)] = 0.009060 + 6.2 * 10^(-8) ~= "0.009060 M"
Finally, the third equilibrium reaction
" "HPO_(4(aq))^(2-) + H_2O_((l)) rightleftharpoons H_3O_((aq))^(+) + PO_(4(aq))^(3-)
I...6.2 * 10^(-8)...........................0.009060.........0
C.......(-x).............................................(+x)..........(+x)
E...6.2 * 10^(-8)-x.................0.009060+x.......x
K_(a3) = ([H_3O^(+)] * [PO_4^(30)])/([HPO_4^(2-)]) = [(0.009060 +x) * x]/(6.2 * 10^(-8) - x)
Once again, you can safely approximate the above ratio with
4.2 * 10^(-13) = (0.009060 * x)/(6.2 * 10^(-8)) => x = 2.8 * 10^(-18)
As a result, [PO_4^(3-)] = 2.9 * 10^(-18)"M"
[H_3O^(+)] = 0.009060 + 2.9 * 10^(-18) ~= "0.009060 M"
Therefore, the concentration of all the species listed will be
[H_3PO_4] = 0.02 - 0.009060 = color(green)("0.01094 M")
[H_2PO_4^(-)] = color(green)("0.009060 M")
[HPO_4^(2-)] = color(green)(6.2 * 10^(-8)"M")
[PO_4^(3-)] = color(green)(2.9 * 10^(-18)"M")
[H_3O^(+)] = color(green)("0.009060 M")
