Tuesday
September 16, 2014

Homework Help: Chemistry

Posted by Amphee on Monday, May 3, 2010 at 2:50pm.

What is the pH of the solution created by combining 12.20 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
12.20
===================================
my work:
0.000420 moles of NaOH / 0.020 litres = 0.0210 Molar NaOH

- log of 0.0210 Molar NaOH =
pOH of 1.68

since pOH + pH = 14

pH+ = 12.32
I did this and I got a pH of 12.32 for both NaOH and HC2H3O2.

===================================

Its the second part I'm having trouble with.

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 w/HC2H3O2
12.20

pH=pka +log(base/acid)

pka=4.75

for the base I got =0.06039602
for the acid I got = 0.02079

apparently this is wrong.
Is the pH for NaOH different than the pH of HC2H3O2? cuz for the first part they had the same pH (pH=12.32)
Thanks.

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