Calculate the mole fractions of SO2•H2O, HSO3- and SO3 2- in solution at a pH of 3.0, characteristic of many fogs, as well as the total concentration of S(IV) in solution for 20 ppb SO2 in the gas phase. Constants attached in table Selected Henry's Law Constants and Equilibrium Constants at 298 K.К (М)1.0 x 1014H (mole L1 atm1)EquilibriumH20 > H* + OHCO2 + H20 €> CO2·H2O3.4 x 10-2CO2·H20 > H* + HCO34.3 x 107HCO3 H* + CO3²-4.7 x 10-11SO2 + H20 → SO2·H2OSO2·H20 > H* + HSO31.231.32 x 10-2HSO3 → H* + SO3²-6.42 x 10-8NH3 + H2O > NH3·H2O62NH3-H20 > NH4* + OH1.8 x 105HNO3 + H20 A HNO3-H2O2.1 x 105HNO3-H20 €> H* + NO315.4H2O2 + H2O > H2O2•H2O7.45 x 104H2O2-H20 > H* + HO22.5 x 10-12O3 + H20 → O3·H2O0.011

Calculate the mole fractions of SO2•H2O, HSO3- and SO3 2- in solution at a pH of 3.0, characteristic of many fogs, as well as the total concentration of S(IV) in solution for 20 ppb SO2 in the gas phase. Constants attached in table

Calculate the mole fractions of SO2•H2O, HSO3- and SO3 2- in solution at a pH of 3.0, characteristic of many fogs, as well as the total concentration of S(IV) in solution for 20 ppb SO2 in the gas phase. Constants attached in table

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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Question

Selected Henry's Law Constants and Equilibrium Constants at 298 K.
К (М)
1.0 x 1014
H (mole L1 atm1)
Equilibrium
H20 > H* + OH
CO2 + H20 €> CO2·H2O
3.4 x 10-2
CO2·H20 > H* + HCO3
4.3 x 107
HCO3 H* + CO3²-
4.7 x 10-11
SO2 + H20 → SO2·H2O
SO2·H20 > H* + HSO3
1.23
1.32 x 10-2
HSO3 → H* + SO3²-
6.42 x 10-8
NH3 + H2O > NH3·H2O
62
NH3-H20 > NH4* + OH
1.8 x 105
HNO3 + H20 A HNO3-H2O
2.1 x 105
HNO3-H20 €> H* + NO3
15.4
H2O2 + H2O > H2O2•H2O
7.45 x 104
H2O2-H20 > H* + HO2
2.5 x 10-12
O3 + H20 → O3·H2O
0.011

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