I’m really stuck on this problem. This involves the dissolving of Borax. Na2B4O7•10H2O(s)<->2Na^+(aq) + B4O7^2-(aq) + 10H2O deltaH=109kJ/mol deltaS= 340J/mol•K Kc=0.047@25C
If the starting concentration of B4O7 is 0.17M and the sodium ions are 0.34M at 25C, which direction will the reaction proceed? I said forward because Q
At what temperature would a mixture of these same starting concentrations be a saturation solution (i.e. be at equilibrium) And that’s where I’m stuck
At what temperature would a mixture under standard conditions (B4O7=1M, Na=1M) be a saturation solution (i.e. be at equilibrium) And I’m stuck here again
I understand that crossover temperature plays a role (Tc=deltaH/deltaS) as well as equilibrium constant but I don’t understand how to work with given concentrations. Please help!
