Question

If you had 100 ml of a 1.00 M solution of the fully unprotonated form of this peptide, what would the pH be?

a) 1.00
b) 7.00
c) 11.00
d) 14.00

Answer 1

The pH of the solution cannot be determined without knowing the concentration of OH- ions.

Step-by-step explanation:

The pH of a solution can be calculated using the formula pH = 14.00 - pOH. In this case, since we have a solution of the fully unprotonated form of a peptide, the pOH can be calculated using the formula pOH = -log[OH-]. To find the pH, we need to know the concentration of OH- ions in the solution. However, this information is not given in the question, so it is not possible to determine the exact pH. Therefore, the correct answer to the question is none of the provided options (a, b, c, or d).