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Home Q & A Board Science-Related Homework Help Chemistry (Moderator: Laser_3)
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ripthekid ripthekid
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11 years ago
How many moles of sodium acetate must be added to 20 L of 0.10 M acetic acid to give a solution that has a pH equal to 5.00? Ignore the volume change due to the addition of sodium acetate.
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#1
11 years ago
Ka for acetic acid = 1.75x10^-5
The Henderson-Hasselbalch equation-
pH = pKa + log(A-/HA)
[HA] = 0.10 M
pKa = -log(1.75x10^-5) = 4.76
5.00 = 4.76 + log(A-/0.10)
log(A-/0.10) = 5.00 - 4.76 = 0.24
A-/0.10 = 10^0.24 = 1.74
[A-] = 0.174 M
20 L x 0.174 M = 3.48 moles sodium acetate
ANSWER: 3.48 moles of sodium acetate
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