Calculate the theoretical pH after 2.50 mL and 9.50 mL of NaOH has been added in both the titration of HCl and of HC2H3O2. Indicate if the volume of NaOH is before or after the equivalence point. Compare these theoretical values with the actual values found on the titration curves created in lab. (Hint: Use total volume of titrant (the initial and final volume on the buret) in conjunction with the time required to deliver that volume to convert the volumes given above to time.) Show a sample of all necessary calculations. Calculate the percent error from the theoretical values.

PLEASE help, I've searched all over online and I can't find anything helpful for this problem =(

You must be doing a virtual titration; but without some hard data, we can't help. For example, if you can supply the molarity and volume of the reactants, I'm sure we can help.

molarity is .1 for all substances, volume of HCl and HC2H3O2 is 8.00ml each, both diluted in 100ml of water

To calculate the theoretical pH after adding NaOH in the titration of HCl and HC2H3O2, you need to perform some calculations based on the reaction equation and the principles of acid-base titrations.

First, let's break down the steps to solve this problem:

1. Convert the volumes of NaOH added (2.50 mL and 9.50 mL) to time using the total volume of titrant and the time required to deliver that volume.

2. Determine the amount in moles of HCl and HC2H3O2 based on the stoichiometry of the reaction.

3. Calculate the new concentrations of H+ and OH- ions after the addition of NaOH.

4. Use the concentrations of H+ and OH- ions to determine the pOH.

5. Convert the pOH to pH.

Now let's go through the steps in detail:

Step 1: Convert volumes to time
Since we don't have the time required to deliver the specified volumes, it's impossible to convert the volumes directly to time. Unfortunately, without this information or any further data, it is not possible to calculate the theoretical pH.

Step 2: Determine moles of HCl and HC2H3O2
Assuming that the reaction equation is:
HCl + NaOH -> NaCl + H2O
The stoichiometry tells us that for every 1 mole of HCl, 1 mole of NaOH reacts. Similarly, for every 1 mole of HC2H3O2, 1 mole of NaOH reacts. Therefore, the moles of HCl and HC2H3O2 can be calculated.

Moles of HCl = concentration of HCl x volume of HCl in liters
Moles of HC2H3O2 = concentration of HC2H3O2 x volume of HC2H3O2 in liters

Step 3: Calculate new concentrations of H+ and OH- ions
After adding NaOH, the moles of H+ ions decrease while the moles of OH- ions increase. Using the balanced equation, we know that for every 1 mole of NaOH, 1 mole of OH- ions is produced. Hence, calculate the new concentrations of H+ and OH- ions.

Step 4: Calculate pOH
pOH = -log[OH-]

Step 5: Convert pOH to pH
pH = 14 - pOH

Regarding the comparison with actual values found on titration curves in the lab, you'll need to consult the data obtained during the experiment. The actual values may differ due to experimental errors or factors that affect the accuracy of measurements.

To calculate the percent error from theoretical values, use the following formula:
Percent Error = (|Theoretical value - Actual value| / Theoretical value) x 100

Unfortunately, without additional data or information, we cannot provide the specific calculations or compare with actual values.