A buffer solution with a pH of 4.25 is prepared with the same volumes of _________ M formic acid and 0.12 M sodium formate.
The Ka of formic acid is 1.8 ⋅ 10-4.
3.7×10−2
0.38
1.8×104
7.5×10−2
1.9×10−2
pH = 4.25
Ka = 1.8*10-4
pKa = -log Ka = -log (1.8*10-4) = 3.74
[HCOO-] = 0.12 M
[HCOOH] = ?
Using Handerson Hasselback equation:
pH = pKa + log [HCOO-]/[HCOOH]
4.25 = 3.74 + log (0.12)/[HCOOH]
log [(0.12)/[HCOOH]] = 0.51
[(0.12)/[HCOOH]] = 3.24
[HCOOH] = 0.12/3.24 = 0.037
[HCOOH] = 0.037 M = 3.7*10-2 M
1st option is correct
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