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Determine the pet of a 1.7 l perchloric acid solution which contains 55.2 grams of perchloric acid (molar mass 100-46) and

User Xavinou
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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.

User Miroslava
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