[bmu123]

(i)Estimate the solubility of hydrogen in water at the given temperature and
pressure.

Would I use Henry's law for this? so p=1atm/101325Pa

So C = kH x p
I know kH = 1282.05 L atm mol^-1 from Wikipedia but not sure that's how I'm supposed to do it!
1282.05 x 1 = 1282.05
Think I'm definitely doing this wrong??

(ii)Given that E^o Ag+/Ag is 0.7990 V at 25°C, give the E^o of the cell and
determine the molality required to produce unit activity of H+. Give full working and reasoning in your answer, explaining any assumptions you make.

No idea what I'm doing here! So E^ocell = Eanode - Ecathode and I'm given Ecathode as 0.7990 V. Is the standard hydrogen cell always ) 0 V? Then I'm guessing when I work out Ecell I would draw a graph of molarity vs E and work out the molarity?

[mjc123]

The units of kH look wrong - multiply by P and you get something in L atm² mol^-1. Looks as if it was meant to go on the other side of the equation: p = kH*C. Try using a value of 1/1282.05 mol L^-1 atm^-1 in your equation.

[mjc123]

Standard hydrogen cell is 0V at 298K, 1 atm H₂ and a_H+ = 1
Use the Nernst equation to determine the E° of a cell with 0.001m Ag⁺ and a_H+ = 1
Use your E-m data to work out the molality at which a_H+ = 1