This question is worth 20 points and there will be only one attempt. I will grade the first attempt of this question. Number your answers 1 through 10 and type the answers in the space provided. Consider the titration of a 35.0 mL sample of 0.185 M CH3NH2 with 0.150 M HBr. Kb = 4.4 x 10-4 What is the initial pH of the solution before adding the acid? What is the pH after adding 5mL of acid (before equivalence point)? What is the concentration of hydroxide ions at equilibrium before acid is added? At the equivalence point, what ion is affecting the pH? How many moles of acid needs to be added to reach the equivalence point? How many mL of acid needs to be added to reach the equivalence point? What is the percent dissociation of the weak base? What is the pH at the equivalence point? What is the pH after the addition of 47 mL of acid to this solution? What ion is affecting the pH after the addition of 47 mL of acid?