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.
Given:
Molarity of all chemicals are 0.1 M
HCl and HC2H3O2 are 8ml prepared in 100ml water.
Im guessing I need to make and ICE chart but I'm having trouble determining the molarities that would go into the ICE chart.
To determine the theoretical pH after adding NaOH in the titration of HCl and HC2H3O2, you need to understand the stoichiometry of the reactions and the pH calculations involving acid-base titrations.
Let's start with the titration of HCl:
1. Calculate the moles of HCl in the initial solution:
moles of HCl = molarity of HCl * volume of HCl
2. Determine the stoichiometry of the reaction between HCl and NaOH:
HCl + NaOH → NaCl + H2O
From the balanced equation, we can see that it is a 1:1 ratio between HCl and NaOH.
3. Determine the moles of NaOH added:
moles of NaOH = molarity of NaOH * volume of NaOH
4. Now, determine the moles of HCl remaining after the reaction:
moles of HCl after reaction = initial moles of HCl - moles of NaOH added
5. Determine the volume of the final solution after adding NaOH:
final volume = initial volume (HCl) + volume of NaOH added
6. Calculate the new molarity of HCl after the reaction:
molarity of HCl after reaction = moles of HCl after reaction / final volume
7. Finally, calculate the pH using the formula:
pH = -log[H+]
where [H+] is the concentration of the remaining HCl.
To calculate the theoretical pH after adding NaOH in the titration of HC2H3O2, the steps are similar. You need to apply the same steps as above, but adjust the stoichiometry and replace HCl with HC2H3O2 in the equations.
Hope this helps you in determining the molarities and calculating the theoretical pH of the solutions!