You have 25.00 mL of a 0.250 M aqueous solution of the weak base CH3NH2 (Kb...

You have 25.00 mL of a 0.250 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 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?

(b) What is the pH of the 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 30.00 mL of acid has been added?

Expert Solution

queen_honey_blossom answered 4 months ago

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