Any help would be great, even just setting up the problem thanks

Exercise: Suppose 25mL of 0.10MNH3(aq) is titrated with 0.50MHCl(aq). Calculate the pH at the equivalence point? (We will answer this in parts.) A. Calculate the molar concentration of the product at the equivalence point. (1) Concept Check: What type of reaction is occurring between aqueous ammonia, NH3(aq), and hydrochloric acid, HCl(aq) ? What is the product of the reaction between aqueous ammonia and hydrochloric acid? (2) What is the stoichiometry of the reaction between ammonia and hydrochloric acid? Does this reaction go to completion (i.e. large Knet) ? How many milliliters of the HCl(aq) solution will it take to neutralize the ammonia? (3) Calculate the molar concentration of the product at the equivalence point (i.e. after complete neutralization of aqueous ammonia with hydrochloric acid). Assume that the volumes of the ammonia and hydrochloric acid solutions are additive. B. Calculating the pH of the solution at the equivalence point. (1) Concept Check: What type of solution is made at the equivalence point (e.g. weak acid, strong, base, etc.)? Based on our answer what would you predict the pH of this solution to be: less than 7 , equal to 7 , greater than 7 ? (2) Solution strategy: Review the appropriate sections in chapter 14 for how to calculate the pH of this type of solution. (3) Calculate the pH of the solution at the equivalence point. (4) Assessment: Is your answer consistent with your prediction in B(1)? Is your answer consistent with the information presented in the Model and Figure 1