We’re being asked to calculate the pH of a 0.95 M B
B (aq) + H2O (l) → BH+ (aq) + OH- (aq)
From this, we can construct an ICE table for the reaction of B in a solution. Remember that liquids are ignored in the ICE table.
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).
(a) before addition of any HCl
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What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Weak Base Strong Acid Titrations concept. You can view video lessons to learn Weak Base Strong Acid Titrations. Or if you need more Weak Base Strong Acid Titrations practice, you can also practice Weak Base Strong Acid Titrations practice problems.