Complete the table below:
What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water (like it will be in the experiment you perform in lab)?
mL NaOH: 0.70
pH w/ HCl: 2.14
pH w/ HC2H3O2: ???
I got pH w/ HCl, but I can't get pH w/ HC2H3O2. Please help!!
nevermind, i got the answer
See my response above.
To determine the pH with HC2H3O2, you first need to calculate the moles of HC2H3O2. From there, you can find the concentration of HC2H3O2 in the diluted solution. Finally, you can use the concentration to find the pH using the relevant equation.
To calculate the moles of HC2H3O2, you need to use the equation:
moles = concentration * volume
Given that the volume of the acid is 8.00 mL and the concentration is 0.10 M, you can calculate the moles of HC2H3O2:
moles of HC2H3O2 = 0.10 M * 8.00 mL
Next, you need to find the concentration of HC2H3O2 in the diluted solution. This can be done by dividing the moles of HC2H3O2 by the total volume of the solution. The total volume is the sum of the volume of the acid and the volume of water added, which is 8.00 mL + 100 mL:
total volume = 8.00 mL + 100 mL = 108 mL
Now, calculate the concentration of HC2H3O2 in the diluted solution:
concentration of HC2H3O2 = moles of HC2H3O2 / total volume
Finally, you can find the pH using the concentration of HC2H3O2 in the diluted solution. The pH of HC2H3O2 can be determined using the equation:
pH = -log(concentration)
Substitute the concentration value you calculated into the equation above to find the pH with HC2H3O2.