A buffer is prepared by combining 17.6 g of H2CO3 (carbonic acid) with 220 mL of 0.18 M NAOH and diluting to 3.5 L. (K, = 4.3 x 107) (MM H2CO3 = 62 g/moll) %3D a) Calculate the initial moles of acid (before reaction) (. b) Calculate the initial moles of the OH base (before reaction) c) Calculate the moles of H2CO3 and the conjugate base HCO3 after reaction( d) Calculate the concentrations H2CO3 and the conjugate base HC03 after the reaction e) Determine the pH of the buffer H,CO, + OH 2 HCO, + H,0 Initial moles a b After reaction Concentration

A buffer is prepared by combining 17.6 g of H2CO3 (carbonic acid) with 220 mL of 0.18 M NAOH and diluting to 3.5 L. (K, = 4.3 x 107) (MM H2CO3 = 62 g/moll) %3D a) Calculate the initial moles of acid (before reaction) (. b) Calculate the initial moles of the OH base (before reaction) c) Calculate the moles of H2CO3 and the conjugate base HCO3 after reaction( d) Calculate the concentrations H2CO3 and the conjugate base HC03 after the reaction e) Determine the pH of the buffer H,CO, + OH 2 HCO, + H,0 Initial moles a b After reaction Concentration

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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