Ireally don't get this question, could someone in a 1.0× 10–2 m solution of nh4clo4(aq), identify the relative molar amounts of these species.

In this problem we need to identify the relative molar amounts of:
NH₄⁺ , ClO₄⁻ , NH₃ , HClO₄ , H₃O⁺ , H₂O, OH⁻
- The salt is completely ionized through this equation:
NH₄ClO₄ → NH₄⁺ + ClO₄⁻
0.01 M       0.01 M     0.01 M
So: 
[ClO₄⁻] = 0.01 M (conjugate base of strong acid)
[HClO₄] = 0 M
Note that: NH₄⁺ is weak acid ionized as follow:
NH₄⁺ ⇄ NH₃ + H⁺
Ka =  = 5.6 x 10⁻¹⁰
[H⁺] = [NH₃] = x  and [NH₄⁺] = 0.01 - x (because Ka is very small so x will be neglected compared to 0.01)
Ka = 5.6 x 10⁻¹⁰ = 
[H⁺] = [NH₃] = x = 2.37 x 10⁻⁶ M
[NH₄⁺] = 0.01 M
[OH⁻] =  = 4.22 X 10⁻⁹ M
because water is the solvent & this is very dilute solution:
[H₂O] =  = 55.6 M H₂O