Part A.) Consider that you are titrating a diprotic weak base "B" which has pKb1=4 and pKb2=8. The product of the first ionization of B is BH+ and the product of the second ionization is BH22+.
A 0.00500-mol sample of the base is dissolved in enough water to produce 100.0 mL of solution and is titrated with 0.500 M HCl.
What is the exact pH when 7.2 mL of HCl is added?
Enter your answer to three significant figures.
Part B.) 20.0 mL of 0.200 M diprotic acid (H2A) was titrated with 0.100 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10.
a. What is the pH at the first midway point?
b. What is the pH at the second midway point?
c. What is the pH at the first equivalence point?
Enter each of your answers to 3 significant figures.
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Part A.) Consider that you are titrating a diprotic weak base "B" which has pKb1=4 and...
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