(i) Calculate the mass of NaHCO3 (84.007 g mol) must be added to 4.00 g of K2CO3 (138.206 g mol1) to give a pH of 10.80 in 500 mL of water? H2CO3 : Ka1 = 4.45 x10-7, Ka2 = 4,69 x 10-11 %3D (ii) Determine the pH of 100 mL of 0.100 M HCl is added to the solution in (i). (iii) Determine the volume of 0.320 M HNO3 that should be added to 4.00 g K2CO3 to give a pH of 10.00 in 250 mL.

(i) Calculate the mass of NaHCO3 (84.007 g mol) must be added to 4.00 g of K2CO3 (138.206 g mol1) to give a pH of 10.80 in 500 mL of water? H2CO3 : Ka1 = 4.45 x10-7, Ka2 = 4,69 x 10-11 %3D (ii) Determine the pH of 100 mL of 0.100 M HCl is added to the solution in (i). (iii) Determine the volume of 0.320 M HNO3 that should be added to 4.00 g K2CO3 to give a pH of 10.00 in 250 mL.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.49QE: Estimate the pH that results when the following two solutions are mixed. a) 50 mL of 0.3 M CH3COOH...

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