Final answer:
The pH of a 1.7L perchloric acid solution with 55.2 grams of perchloric acid (molar mass 100.46 g/mol) is approximately 0.49.
Step-by-step explanation:
The student is asking to determine the pH of a perchloric acid solution, and the question contains necessary information to calculate it, such as the mass of the acid and the volume of the solution. Perchloric acid is a strong acid that completely dissociates in water. The molar mass of perchloric acid is given as 100.46 g/mol.
First, calculate the number of moles of HClO4 (perchloric acid):
Number of moles = Mass (g) / Molar mass (g/mol)
= 55.2 g / 100.46 g/mol
= 0.549 moles
Then, we calculate the molarity (M) of the solution:
Molarity (M) = Moles of solute / Volume of solution (L)
= 0.549 moles / 1.7 L
= 0.323 M
Since perchloric acid is a strong acid, we can assume that it completely dissociates in water, so the concentration of H+ ions is equal to the molarity of the acid solution.
The pH is calculated using the formula:
pH = -log[H+]
= -log(0.323 M)
Approximately 0.49.
The pH of the perchloric acid solution is estimated to be 0.49.