Problem: The pKb values for the dibasic base B are pKb1 = 2.1 and pKb2 = 7.5. Calculate the pH at each of the following points in the titration of 50.0 mL of a 0.95 M B(aq) with 0.95 M HCl(aq).(c) after addition of 50.0 mL of HCl

FREE Expert Solution

We are asked to determine the pH of the solution. 


First, let's calculate the moles of HCl and dibasic base B

moles B = 50 mL×10-3 L1 mL× 0.95 mol1 L = 0.0475 moles

moles H+ = 50 mL×10-3 L1 mL× 0.95 mol1 L = 0.0475 moles


The moles of HCl and moles of B are equivalent. This means that we reached the equivalence point.


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Problem Details

The pKb values for the dibasic base B are pKb1 = 2.1 and pKb2 = 7.5. 

Calculate the pH at each of the following points in the titration of 50.0 mL of a 0.95 M B(aq) with 0.95 M HCl(aq).

(c) after addition of 50.0 mL of HCl

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Our tutors have indicated that to solve this problem you will need to apply the Equivalence Point concept. If you need more Equivalence Point practice, you can also practice Equivalence Point practice problems.