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Consider the titration of a 50.0 mL of a .133 M NH3 (a weak base with Kb = 1.76 x 10^-5) with a 0.223 M HCl (a strong acid). Calculate the pH of the solution at each of the following points:
1. What is the pH of the solution before the titration has begun?
2. What is the pH of the solution after the addition of 15 mL of HCl?
3. What is the pH of the solution at the equivalence point?
4. What is the pH of the solution after the addition of 35 mL of HCl?
5. Sketch the form of the titration curve with important points.
Please explain every step, step by step and make clear explanations along the way
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