Determine the pH of a solution made by mixing 50,00 mL of 0,100 M nitric acid with 100 mL of 0,200 M nitric acid

To determine the pH of a solution made by mixing different concentrations of a common acid, you need to consider the principles of acid-base chemistry. In this case, the two concentrations of nitric acid can be combined to calculate the resulting pH using the following steps:

Step 1: Calculate the number of moles for each solution.
Moles = concentration (M) × volume (L)

For the first solution:
Moles of 0.100 M nitric acid = 0.100 mol/L × 0.05000 L = 0.005 moles

For the second solution:
Moles of 0.200 M nitric acid = 0.200 mol/L × 0.100 L = 0.020 moles

Step 2: Determine the total moles of nitric acid in the combined solution.
Total Moles = Moles of first solution + Moles of second solution

Total Moles = 0.005 moles + 0.020 moles = 0.025 moles

Step 3: Calculate the volume of the resulting solution.
Volume = Volume of first solution + Volume of second solution

Volume = 0.05000 L + 0.100 L = 0.150 L

Step 4: Calculate the new concentration of the combined solution.
Concentration (M) = Total Moles / Volume

Concentration = 0.025 moles / 0.150 L = 0.1667 M

Step 5: Calculate the pH using the concentration of the combined solution.
pH = -log[H+]
[H+] is the concentration of hydrogen ions.

In this case, since the nitric acid dissociates to form one hydrogen ion (H+), the concentration of hydrogen ions is the same as the concentration of nitric acid solution.

pH = -log(0.1667) ≈ 0.778

Therefore, the pH of the solution made by mixing 50.00 mL of 0.100 M nitric acid with 100 mL of 0.200 M nitric acid is approximately 0.778. Note that the answer is rounded to three decimal places.