what is the pH and pOH of a solution made by adding water to 15 grams of HCl until the volume of the solution is 2500mL?

To find the pH and pOH of the solution, we need to calculate the concentration of HCl in the solution. We can use the formula:

Concentration (in moles per liter) = Amount of substance (in moles) / Volume (in liters)

First, let's find the number of moles of HCl in 15 grams. We can do this by dividing the mass by the molar mass of HCl, which is 36.46 g/mol:

Number of moles = Mass / Molar Mass = 15 g / 36.46 g/mol

Next, we need to convert the volume from milliliters (mL) to liters (L). Since 1 L = 1000 mL, we have:

Volume = 2500 mL / 1000 = 2.5 L

Now, we can calculate the concentration of HCl:

Concentration of HCl = Number of moles / Volume = (15 g / 36.46 g/mol) / 2.5 L

After calculating this, let's assume the concentration comes out to be 0.164 M.

To find the pH, we can use the fact that pH = -log[H+], where [H+] is the concentration of hydrogen ions in the solution. In this case, since HCl is a strong acid, it completely dissociates in water, resulting in the same concentration of H+ ions.

Therefore, the pH of the solution is:

pH = -log(0.164) ≈ 0.7873

To find the pOH, we can use the fact that pOH = -log[OH-], where [OH-] is the concentration of hydroxide ions in the solution.

In this case, since HCl does not contain any hydroxide ions, the concentration of OH- in the solution is negligible. Hence, the pOH of the solution is close to 0.