Calculate the pH of a solution formed by mixing 50.0 mL of 0.1 M HCl and 50.0 mL of 0.1 M NaOH. (Assume complete neutralization.)
Guide On Rating System
Vote
To calculate the pH of the solution, we need to first determine the moles of HCl and NaOH that are present in the solutions.
The moles of HCl can be calculated using the formula:
moles = concentration (M) x volume (L)
For the HCl solution:
moles of HCl = 0.1 M x 0.050 L = 0.005 moles
Similarly, the moles of NaOH can be calculated:
moles of NaOH = 0.1 M x 0.050 L = 0.005 moles
Since HCl and NaOH react in a 1:1 ratio, the moles of HCl and NaOH are equal. Hence, they will completely react and neutralize each other.
Now, to determine the concentration of the resulting solution after neutralization, we need to find the total volume of the solution. Since we are adding equal volumes of HCl and NaOH, the total volume of the solution will be 50.0 mL + 50.0 mL = 100.0 mL = 0.100 L.
Since the moles of HCl and NaOH are equal and their total volume is 0.100 L, the concentration of the resulting solution can be calculated as:
concentration = moles / volume = 0.005 moles / 0.100 L = 0.05 M
Now, to calculate the pH of the resulting solution, we need to determine the concentration of H+ ions in the solution. Since HCl is a strong acid and completely dissociates in water, the concentration of H+ ions is equal to the concentration of the resulting solution, which is 0.05 M.
Using the pH formula:
pH = -log[H+]
pH = -log(0.05) = 1.30
Therefore, the pH of the solution after neutralization is 1.30.
Got a question with my answer?
Cheapmath.com is completely free!
Asking question is free.
Getting answers is free.
+99