1) For 10mL of .50 M Morphine (pKb = 6.05) give the pH at the various points indicated when titrated with 0.30 M HNO3. Kw = 1 x10-14
a. before any HNO3 has been added
b. At 1/4 equivalence point
c. at 1/2 the equivalence point
d. at 3mL past the equivalence point
Morphine millimoles = 10 x 0.5 = 5
pKb = 6.05
Kb = 8.91 x 10^-7
a. before any HNO3 has been added
pOH = 1/2 (pKb + log C)
= 1/2 (6.05 + log 0.5)
= 2.87
pH = 11.13
c. at 1/2 the equivalence point
at half equivalence point
pOH = pKb = 6.05
pH = 7.95
d) at 3mL past the equivalence point
millimoles of base = millimoles of acid
5 = 0.3 x V
V = 16.67 mL
volume of HNO3 = 16.67 mL
3 mL past means = 16.67 + 3 = 19.67 mL
millimoles of HNO3 = 19.67 x 0.3 = 5.9
morphine + HNO3 -----------------> salt
5 5.9 0
0 0.9 5
here strong acid remained. so
[H+] = 0.9 / (19.67 + 10) = 0.0303 M
pH = -log [H+] = -log (0.0303)
= 1.52
pH = 1.52
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