Final answer:
Calculating the pH of a solution with two weak acids requires complex equilibrium calculations. The final pH will be primarily determined by the stronger acid, which is the one with the lower pKa value. Without further information, an exact pH cannot be provided.
Step-by-step explanation:
The question is asking for the pH of a mixed weak acid solution with given concentrations and the pKa values of two different weak acids. To solve for the pH, one would typically use the Henderson-Hasselbalch equation, however, the equation is not appropriate here as we do not have an acid-base conjugate pair but rather two different weak acids. Since the two acids have significantly different pKa values (7.27 and 3.93), the acid with the lower pKa will contribute most to the acid ionization and thus primarily determine the pH of the solution. The strong acid with a pKa of 3.93 will suppress the ionization of the weaker acid with a pKa of 7.27. Therefore, the pH will be closer to the pKa of the stronger acid (the one with pKa 3.93).
To calculate the exact pH, a more complex calculation involving simultaneous equilibrium equations would need to be performed, taking into account the contribution of both acids to the hydronium ion concentration. Since the question is seeking only one answer and the relevant information for such a calculation is not provided, the response is based on the assumption that a detailed calculation might be beyond the scope of the curriculum and the fact that the lower pKa acid will dominate the pH.