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Carry out a serial titration of one drop of the weak base 0.05 M NH, (aka NH,OH) with 0.01 M HCI. Stir. Measure the pH valuesNOTE: Data from the computer calculation give an equivalence point pH of 5.70 at 5.0 drops of added 0.01 M HCI.Observations: Lane 1-purple (pH 12) Lane 2-purple-ish blue (pH 10) Lane 3-green-ish blue (pH 8) Lane 4-yellow (pH 5) Lane 5-oQ14. Considering Figure 14.7, what are the K, and pK, of ammonia and the K and pK, of the ammonium ion? Explain how you deter12.00 10.00 6.00 4.00 0.00 + 0.00 2.00 6.00 8.00 10.00 Drops of Added 0.01 M HCI Figure 14.7 1 drop of 0.05 M NH3 titrated wi

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Answer #1

14) NH3 is a weak base being titrated by strong acid. You can determine the pKb by looking at the graph at the midpoint of equivalence, it is half the volume necessary to reach the point of equivalence:

Average volume = 2.5 mL

pKb = 9.2

Kb is calculated:

Kb = 10 ^ -pKb = 10 ^ -9.2 = 6.31E-10

Then Ka and pKa can be calculated:

Ka = Kw / Kb = 10E-14 / 6.31E-10 = 1.58E-5

pKa = - log Ka = - log 1.58E-5 = 4.8

15) This happens because HCl can completely dissociate and offer all its H + ions, while NH3 does not completely dissociate and has fewer basic ions.

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