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What is the pH of a solution that contains 0.1 mol of H+ in 325.7L of water?

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Answer:

The pH of the solution is 3.51.

Step-by-step explanation:

To calculate the pH of a solution containing 0.1 mol of H+ in 325.7L of water, we need to first calculate the concentration of H+ in the solution.

Concentration (in mol/L) = Number of moles / Volume (in L)

Concentration (in mol/L) = 0.1 mol / 325.7 L

Concentration (in mol/L) = 0.000307 mol/L

Now, we can use the formula for pH:

pH = -log[H+]

where [H+] is the concentration of hydrogen ions in the solution.

Substituting the value of [H+] we calculated above, we get:

pH = -log(0.000307)

pH = 3.51

Therefore, the pH of the solution is 3.51.

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