what is a titration of 25 ml of 0.15 M HCLO2 is performed with 0.15 M NaOH. What is the pH of the solution after 25 ml of naOH have been titrated? Ka = 0.011

To find the pH of the solution after 25 ml of NaOH have been titrated, we need to calculate the concentration of HClO2 at that point and use the given equilibrium constant (Ka) to determine the pH.

Here's how we can approach this problem:

Step 1: Determine the initial moles of HClO2:
The initial moles of HClO2 can be calculated using the given volume and concentration:
moles of HClO2 = volume (in liters) × concentration (in M)
moles of HClO2 = 0.025 L × 0.15 M

Step 2: Calculate the moles of NaOH added:
Since the moles of NaOH added is equal to the moles of HClO2, we can directly use the value calculated in Step 1.

Step 3: Calculate the concentration of HClO2 remaining:
Since the volume of the solution has increased by 25 ml due to the addition of NaOH, we need to calculate the new concentration of HClO2.
To do this, we need to determine the total volume of the solution after NaOH has been added. Since 25 ml of NaOH have been added to the initial 25 ml of HClO2, the total volume will be 50 ml or 0.050 L.
Now, we can calculate the new concentration of HClO2:
new concentration = moles of HClO2 / total volume

Step 4: Calculate the concentration of ClO2-:
Since the moles of HClO2 are equal to the moles of NaOH added, the concentration of ClO2- can be calculated using the moles of NaOH added and the new total volume.

Step 5: Calculate the concentration of H+:
Since the reaction between HClO2 and NaOH is a one-to-one reaction, the concentration of H+ will be equal to the concentration of ClO2-.

Step 6: Calculate the pH:
pH is defined as the negative logarithm (base 10) of the concentration of H+.
pH = -log[H+]

Using the concentration of H+ calculated in Step 5, we can find the pH using the above formula.

By following these steps and performing the calculations, the pH of the solution after 25 ml of NaOH have been titrated can be determined.