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I need help for this. Im confused on how to solve the problems. thank you You...

I need help for this.

Im confused on how to solve the problems.

thank you

You have 15.00 mL of a 0.350 M aqueous solution of the weak base CH3NH2 (Kb = 5.00 x 10-4). This solution will be titrated with 0.350 M HCl.

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

(b) What is the pH of the before any acid is added?

(c) What is the pH of the solution after 10.00 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 20.00 mL of acid has been added?

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