Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: laddoo12 on April 24, 2012, 03:03:48 AM

H+(aq) + OH(aq)>H2O(l) deltaH = 55.8 kJ; K = 1.0 x 1014 (at 25.0 C)
Calculate the pOH of a 0.0100 M HCl solution at 50.0 C.
So i have tried the arrhenuis equation to find K2 with is 1.749e14 because we have everything we need to plug in for it but i have no clue on how to find the POH of it in relation with whats given to us please help i have a exam on tuesday!

H+(aq) + OH(aq)>H2O(l) deltaH = 55.8 kJ; K = 1.0 x 1014 (at 25.0 C)
Calculate the pOH of a 0.0100 M HCl solution at 50.0 C.
So i have tried the arrhenuis equation to find K2 with is 1.749e14 because we have everything we need to plug in for it but i have no clue on how to find the POH of it in relation with whats given to us please help i have a exam on tuesday!
Well, it's Tuesday already (and was when you posted), but anyway... Can you write an equation for K2, in terms of [H+] and [OH]?