Write equations for the reactions of the following Bronsted bases with water: a) SeO4 2- You have 30.00 mL of a 0.250 M aqueous solution of the weak
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Write equations for the reactions of the following Bronsted bases with water:

    a) SeO4 2-

    1. You have 30.00 mL of a 0.250 M aqueous solution of the weak base (CH3)2NH (Kb = 7.40 x 10-4). This solution will be titrated with 0.250 M HCl.

    (a) How many mL of acid must be added to reach the equivalence point? solution before any acid is added?

    (c) What is the pH of the solution after 5.00 mL of acid has been added? (d) What is the pH of the solution at the equivalence point of the titration? (e) What is the pH of the solution when 35.00 mL of acid has been added?

    (b) What is the pH of the

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