Find the pH of a solution that contains 3.25g of HCI in 2.75L of solution.

To find the pH of the solution, we need to calculate the concentration of HCl, and then use that to find the pOH and finally convert it to pH using the equation: pH = 14 - pOH.

First, we need to calculate the number of moles of HCl in the solution using the given mass and molar mass of HCl:
Number of moles = mass / molar mass
Number of moles = 3.25g / 36.46 g/mol (molar mass of HCl)
Number of moles = 0.089 moles

Next, we need to calculate the concentration of HCl in the solution using the number of moles and volume of the solution:
Concentration = moles / volume
Concentration = 0.089 moles / 2.75 L
Concentration = 0.0324 M

Now that we know the concentration of HCl, we can calculate the pOH using the equation:
pOH = -log[OH-]
But since HCl is a strong acid that completely dissociates, we can assume that all of the HCl will contribute to the concentration of H+.
Thus, the concentration of H+ is also 0.0324 M.

Using the equation pOH = -log[H+], we find:
pOH = -log(0.0324)
pOH = 1.49

Finally, we can calculate the pH using the equation:
pH = 14 - pOH
pH = 14 - 1.49
pH ≈ 12.51

Therefore, the pH of the solution is approximately 12.51.