a certain solution contains 0.35 mol of HCl in 1200 mL of water. What is the pH of the solution?

M = moles/L = 0.35 mol/1.200L = ??

pH = -log(H^+).

To determine the pH of the solution, we need to calculate the concentration of H+ ions present in the solution. We can use the formula:

pH = -log[H+]

First, we need to calculate the molarity (M) of HCl:

Molarity (M) = moles of solute / volume of solution (in liters)

Given:
Moles of HCl = 0.35 mol
Volume of solution = 1200 mL = 1.2 L

Molarity (M) = 0.35 mol / 1.2 L = 0.2917 M

Now, we can calculate the concentration of H+ ions (which is equal to HCl concentration) in the solution:

[H+] = Molarity of HCl = 0.2917 M

Finally, we can calculate the pH using the formula:

pH = -log[H+]

pH = -log(0.2917)

Using a scientific calculator, we find:

pH ≈ 0.537

Therefore, the pH of the solution containing 0.35 mol of HCl in 1200 mL of water is approximately 0.537.

To find the pH of the solution, we need to know the concentration of HCl in moles per liter. We can start by converting the volume of water to liters:

1200 mL = 1200 mL × 1 L/1000 mL = 1.2 L

Next, we can use the volume of water to calculate the molarity (M) of the HCl solution:

Molarity (M) = moles of solute / volume of solution (in liters)

Given that the solution contains 0.35 mol of HCl and the volume of solution is 1.2 L:

M = 0.35 mol / 1.2 L

M = 0.292 M

Now that we know the molarity of the HCl solution, we can calculate the pH using the formula:

pH = -log[H+]

HCl is a strong acid, so it dissociates completely in water, giving 1 H+ ion for every HCl molecule. Therefore, the [H+] concentration is equal to the HCl concentration, which is 0.292 M.

pH = -log(0.292)

Using a calculator or software, we can find:

pH ≈ 0.537