What is the pH of the solution created by combining 12.90 mL...?

Question

What is the pH of the solution created by combining 12.90 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 wHCl pH wHC2H3O2

12.90

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 wHCl pH wHC2H3O2

12.90

Answer 1

Moles NaOH = 0.0129 L x 0.10 = 0.00129

Moles HCl = 0.0080 L x 0.10 M = 0.00080

moles OH- in excess = 0.00049

total volume = 0.0209 L

[OH-] = 0.00049 mol / 0.0209 L = 0.0234 M

pOH = 1.63

pH = 14 - 1.63 =12.4

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