hell_ever Posted December 28, 2008 Share Posted December 28, 2008 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. Link to comment Share on other sites More sharing options...
CaptainPanic Posted December 30, 2008 Share Posted December 30, 2008 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. Link to comment Share on other sites More sharing options...
Sin Posted December 30, 2008 Share Posted December 30, 2008 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. Link to comment Share on other sites More sharing options...
Genecks Posted January 2, 2009 Share Posted January 2, 2009 Calculate the pH of the solution on completion of the reduction. This seems like a homework question. Link to comment Share on other sites More sharing options...
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