An analytical chemist is titrating 164.9 mL of a 0.3400M solution of propylamine (C,H,NH,) with a o.3700M solution of HNO,. The pK, of propylamine is 3.46. Calculate the pH of the base solution after the chemist has added 67.7 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0

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Give the conjugate acid of each of these bases: (a) HS, (b) HCO3, (c) CO (d) H2PO,, (e) HPO;" , (f) PO " , (g) HSO,, (h) SO , (1) NO2, (j) SO?. 16.6 16.7 Give the conjugate base of each of these acids:

a buffer is prepared by adding 115 mL of .30M NH3 to 135 mL fof .15 M NH4NO3. what is the pH of the final solution?

An analytical chemist is titrating 186.4 ml of a 0.7700M solution of anilline (C,H₂NH₂) with a 0.7300M solution of HNO,. The pK, of aniline is 9.37. Calculate the pH of the base solution after the chemist has added 51.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = 0 X 2

3 7 8. 10 11 12 13 14 A chemist titrates 150.0 mL of a 0.2250M trimethylamine ((CH,),N solution with 0.3664M HCl solution at 25 °C. Calculate the pH at equivalence. ThepK, of trimethylamine is 4.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HCl solution added. pH = Submit Assignment Continue MacBook Air ►► F1 F10 吕0 F3 000 O00 FA F8 F9 esc F6 F1

1. Answer the following, use the data and plot as a reference, answer the following questions:a) What volume of 0.100 M NaOH solution is required to reach the equivalence point, at which the solution is completely neutralized?b) Briefly explain why the pH of the solution drastically increases once the titration proceeds past the equivalence point. c) The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCl titrant.  Calculate the molarity of the NaOH solution.  The titration reaction equation is:NaOH (aq)  +  HCl (aq)  →  NaCl (aq)  +  H 2O (l)

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In the laboratory, a general chemistry student measured the pH of a 0.446 M aqueous solution of hydrofluoric acid to be -0.253. Use the information she obtained to determine the K, for this acid. Ka(experiment)

A 25.000 mL aliquot of weak base that has a concentration of 0.30 M will be titrated with 0.80 M HCl. Calculate the pH of of the solution upon the addition of 9.375 mL of HCl. The Kb of the base is 4.6×10-6. Report your answer to the hundredths place.