Final answer:
To calculate the concentrations of ionic species in Asp at different pH values, pKa values and the Henderson-Hasselbalch equation are needed. The reference information provided pertains to a buffer system with calculations involving hydronium ion concentration and changes in pH after adding NaOH. Without specific pKa values for Asp, precise calculations can't be made.
Step-by-step explanation:
To calculate the concentrations of the two major ionic species present in the 0.1 M solution of Aspartic acid (Asp) at different pH values, consider the pKa values of the amino acid and the Henderson-Hasselbalch equation. Aspartic acid has three pKa values corresponding to the carboxyl groups and the amino group. At pH 4.0, the amino group is fully protonated, and the first carboxyl group is mostly protonated, while the second carboxyl group is mostly deprotonated. At pH 9.4, the amino group is mostly deprotonated, and both carboxyl groups are deprotonated.
However, to provide an accurate calculation, we need the specific pKa values of the carboxyl and amino groups of Asp which are not provided here. The question resembles a typical chemistry problem involving the calculation of ion concentrations in a buffer system or solution of a weak acid or base, which can be solved using equilibrium constants derived from the pKa values.
For the buffer system problem provided as reference, an initial calculation of the hydronium ion concentration in an acetate buffer is given. After the addition of NaOH, the buffer's capacity to resist pH changes is demonstrated through the slight change in pH despite the addition of strong base. In an unbuffered solution, the pH change would be more significant.