Consider a system where water, buffered at pH of 6.5, is in thermodynamic equilibrium with SO2...

 

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Consider a system where water, buffered at pH of 6.5, is in thermodynamic equilibrium with SO2 gas at 10 ppb. The system is at 1 atm, 298 K. HINT: use graphs (such as the effective Henry's Law plot for SO2 vs. pH) in section 7.3 to do most of this problem. You can solve systems of equations or algebraic expressions if you like, but the problem can be solved without extensive calculations. a. What will the dominant S(IV) species in solution be under these conditions? (be sure to justify your answer) b. What will the dissolved S(IV) concentration be (answer in moles/liter)? Consider a system where water, buffered at pH of 6.5, is in thermodynamic equilibrium with SO2 gas at 10 ppb. The system is at 1 atm, 298 K. HINT: use graphs (such as the effective Henry's Law plot for SO2 vs. pH) in section 7.3 to do most of this problem. You can solve systems of equations or algebraic expressions if you like, but the problem can be solved without extensive calculations. a. What will the dominant S(IV) species in solution be under these conditions? (be sure to justify your answer) b. What will the dissolved S(IV) concentration be (answer in moles/liter)?