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18 Nov 2019
titration curve
6. (17 points) In this question you are going to calculate the data that could be used to construct a titration curve (pH versus volume of titrant added) for the titration of an aqueous ammonia (NH3; weak base, pKB -4.7) cleaning solution with a strong acid (HCl). When strong acid is added to an aqueous solution, it immediately reacts and yields H30 ions; thus the titration is described by the reaction NH3(aq) + H3O+(aq) â â NH4+ + H20(1) K = 2.0x 10% The cleaning solution is produced by adding 0.02 moles of NH3 to 1.0 L of pure H20, which you later titrate with 1.0 M HCl titrant solution. To simplify matters we'll assume all activity coefficients = 1.0 for all species in this problem Utilize the ICE Table Method (show your work) to determine the pH of the system when various amounts of the strong acid (titrant) have been added. Note: when you solve the quadratic function, make sure to select the root that is positive, and if you have two positive roots, use the root that represents a realistic change; i.e. the change isn't greater than what was physically added to the system or greater than the concentration of reactant it reacts with. (4 points) Calculate pH of solution when 0 mL of titrant have been added (only the NH3 has been added) a. b. (4 points) Calculate pH of solution when 10 mL of titrant have been added c. (4 points) Calculate pH of solution when 15 mL of titrant have been added d. (4 points) Calculate pH of solution when 25 mL of titrant have been added e. (1 points) At what volume of added titrant is the equivalence point reached?
titration curve
6. (17 points) In this question you are going to calculate the data that could be used to construct a titration curve (pH versus volume of titrant added) for the titration of an aqueous ammonia (NH3; weak base, pKB -4.7) cleaning solution with a strong acid (HCl). When strong acid is added to an aqueous solution, it immediately reacts and yields H30 ions; thus the titration is described by the reaction NH3(aq) + H3O+(aq) â â NH4+ + H20(1) K = 2.0x 10% The cleaning solution is produced by adding 0.02 moles of NH3 to 1.0 L of pure H20, which you later titrate with 1.0 M HCl titrant solution. To simplify matters we'll assume all activity coefficients = 1.0 for all species in this problem Utilize the ICE Table Method (show your work) to determine the pH of the system when various amounts of the strong acid (titrant) have been added. Note: when you solve the quadratic function, make sure to select the root that is positive, and if you have two positive roots, use the root that represents a realistic change; i.e. the change isn't greater than what was physically added to the system or greater than the concentration of reactant it reacts with. (4 points) Calculate pH of solution when 0 mL of titrant have been added (only the NH3 has been added) a. b. (4 points) Calculate pH of solution when 10 mL of titrant have been added c. (4 points) Calculate pH of solution when 15 mL of titrant have been added d. (4 points) Calculate pH of solution when 25 mL of titrant have been added e. (1 points) At what volume of added titrant is the equivalence point reached?
Beverley SmithLv2
4 Jan 2019