An organic nitro compound is electrolytically reduced in an aqueous acetate buffer solution having total acetate (HOAc+OAc-) 0.500 M and pH=5.0. 300 ml of the buffered solution containing 0.01M RNO2 was reduced completely. The dissociation constant of acetic acid is [math]1.75 \times 10^{-5}[/math] at 298 K. The reaction is

 

[math]RNO_2 + 4H^+ + 4e^- \rightarrow RNHOH + H_2O[/math]

 

Calculate the pH of the solution on completion of the reduction.

How would you approach this problem?

 

We're not here to solve your homework questions. Show us you have studied this a little bit before asking us.

If someone does find this out, and does not want to give the answer bluntly, please send it to me threw a PM with a short description of how you got it. I would really be interested to know, because im trying to learn how to work these forumla type-problems.

Calculate the pH of the solution on completion of the reduction.

 

This seems like a homework question.