Answer:
Assuming that the addition of 5.00 mL of 0.011 M HCl to 50.00 mL of pure water does not significantly affect the volume of the solution:
Calculate the number of moles of HCl added:
moles HCl = concentration x volume = 0.011 mol/L x 0.00500 L = 5.50 x 10^-5 mol
Calculate the total volume of the solution:
total volume = 50.00 mL + 5.00 mL = 55.00 mL = 0.055 L
Calculate the concentration of H+ ions in the solution:
[H+] = moles HCl / total volume = 5.50 x 10^-5 mol / 0.055 L = 1.00 x 10^-3 M
Calculate the pH of the solution:
pH = -log[H+] = -log(1.00 x 10^-3) = 3.00
Therefore, the pH of the solution is 3.00.
Step-by-step explanation: