As a chemist, I cannot physically use a pH meter to measure the pH of the solution. However, I can help you calculate the pH of the 0.01 M HCl solution and explain how you would use a pH meter to measure it.First, let's calculate the pH of the 0.01 M HCl solution. HCl is a strong acid, which means it dissociates completely in water to form H+ ions and Cl- ions. The concentration of H+ ions in the solution will be equal to the concentration of HCl, which is 0.01 M. To find the pH, we can use the formula:pH = -log10[H+]pH = -log10 0.01 pH = 2So, the pH of the 0.01 M HCl solution is 2.Now, let's discuss how to use a pH meter to measure the pH of the solution:1. Calibration: Before using the pH meter, you need to calibrate it using standard buffer solutions with known pH values e.g., pH 4, 7, and 10 . Rinse the electrode with distilled water and gently blot it dry with a tissue. Immerse the electrode in the first buffer solution, and adjust the pH meter to match the known pH value of the buffer. Repeat this process for the other buffer solutions to ensure accurate calibration.2. Rinse the electrode: After calibration, rinse the electrode with distilled water and gently blot it dry with a tissue to remove any residual buffer solution.3. Measure the pH of the HCl solution: Pour the 0.01 M HCl solution into a clean beaker. Immerse the electrode into the HCl solution, making sure it is fully submerged. Wait for the pH reading to stabilize on the pH meter display. The pH value should be close to 2, as calculated earlier.4. Rinse and store the electrode: After measuring the pH, rinse the electrode with distilled water, gently blot it dry, and store it according to the manufacturer's instructions.Remember that using a pH meter provides a more accurate pH measurement than our calculated value, as it accounts for any impurities or variations in the solution.