Question #44542

A $0.10 \text{ M}$ aqueous solution of a neutral $\alpha$-amino acid (with $pK_{a1} = 2.00$ and $pK_{a2} = 9.00$) is prepared at $300 \text{ K}$. The osmotic pressure of this initial solution is $2.46 \text{ atm}$, indicating ideal behavior and that the amino acid exists almost entirely as a single-particle zwitterion.

To $1.0 \text{ L}$ of this solution, a small volume of highly concentrated aqueous \ce{HCl} is added to adjust the pH exactly to $2.00$. Assuming the volume of the solution remains unchanged at $1.0 \text{ L}$, what is the new osmotic pressure of the solution at $300 \text{ K}$?

(Given: $R = 0.082 \text{ L atm K}^{-1} \text{mol}^{-1}$, assume all species behave ideally)