What is the pH of the solution created by combining 1.20 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)?
mL NaOH pH w/ HCl pH w/ HC2H3O2
1.20 ? ?
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 pH w/ HCl pH wHC2H3O2
1.20 ? ?
Which point on the titration curve was calculated above?
3 answers
I worked this twice yesterday and once today. What do you not understand about the problem and I can help you through from there.
where do i start?
You have two problems here. The first is the combination of NaOH and HCl. Work with that one first. The second one is NaOH and HC2H3O2. Work with that one second.
For the first one,
1. Write the balanced equation.
2. Calculate moles NaOH and moles HCl. moles = M x L.
3. Determine which is in excess, if either, and prepare an ICE chart if that will help.
4. pH = -log(H^+).
The second one involves the Henderson-Hasselbalch equation.
For the first one,
1. Write the balanced equation.
2. Calculate moles NaOH and moles HCl. moles = M x L.
3. Determine which is in excess, if either, and prepare an ICE chart if that will help.
4. pH = -log(H^+).
The second one involves the Henderson-Hasselbalch equation.
1 answer