1. What is the pH of the solution created by combining 0.50 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)?

Question

1. What is the pH of the solution created by combining 0.50 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)?

2. 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)?

Okay, I solved the first one and got it right...
PH for HCl is 1.05
PH for HC2H3O2 is 3.57

but I don't understand how to do the second one? I tried adjusting the molarity with M1V1 = M2V2 but it isn't working...so could someone please explain step to step how to do it?

Answer 1

1. What is the pH of the solution created by combining 0.50 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)?

read the text book, chemistry by raymond chang chapter 14