0
125.0 mg sample of unknown monoprotic acid dissolved in 100 ml of distilled h20 and titrated with a 0.050 M solution of NaOH Ph was monitored througout and data collected what is Ka the acid?
Ginger29
The total titration took 22.4 ml of alkaline, so half-way was reached at 11.2 ml:
pH at that point was (interpolated between 4.10-4.50) = 4.2
At that point half of the original amount of acid (unknown x) HA has changed to an equal amount of conjugated (coupled) base A- (0.5*x) leaving the other half of HA (also 0.5*x) unchanged
Both amounts filled in in the formula:
Henderson-Hasselbalch equation:
pH = pKa + log[base/acid]gives:4.2 = pKa + log( 0.5 / 0.5 ) = pKa + 0
So Ka = 6.3*10-5
What a nice thing to notice and remember:
half-way every thing is equal: [HA]=[A-] and pKa = pH1/2 !!
Measurements copy/pasted:
First number is the VOlume of OH- added (ml)and second number is the pH 0, 3.095, 3.6510, 4.1015, 4.5017, 4.5518, 4.7119, 4.9420, 5.1121,5.3722,5.9322.2, 6.2422.6, 9.9122.8, 10.223, 10.424, 10.825,11.030, 11.540, 11.8
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