Hi, i'm stuck on part b) of the question below: Q: In order to perform pH determinations with a glass electrode, the cell potential was measured for threestandard solutions with the following pH values at 25 Celsius: 2.04, 7.05, and 9.20. The cell voltage readout(in mV) for each of the above solutions was 238.0, -37.5 and, -164.5, respectively. Calculate: (a) thesensitivity of the pH sensor; (b) the pH of an unknown sample yielding a cell voltage of 20.5 mV; (c) thepH deviation from the actual value if the sample temperature is 35 Celsius. My ans: So to get the sensitivity (s) I just use the nernst equation i.e. Where: R is the gas constant T is temperature in Kelvins n is the charge of a Hydrogen ion = 1 F is Faraday's constant V/pH unit But now I'm stuck on part b). My method is either to rearrange the nernst equation like so: where But this gives me a pH value of 0.96 which doesn't seem right. The other method I am using is to work out the value given the pH scale and sensitivity. i.e. If we know that the cell voltage of the unknown pH is 0.0205V, then if we find the difference between this and the the voltage for pH 7.05 (0.0375V) gives 0.058V. Then divide by the sensitivity of 0.0591V/pH unit to give a pH difference of 0.981. Then then take this value away from the reference pH value of 7.05 to give a pH of 6.068. Any thoughts on my methods, are they correct or am I way off?
It's rare to see a question about electrochemistry on this site, but hey, it's all just physics. I'm no expert, and I think there is a problem with the the text of your numbers in the post, but my first instinct is for question a), just show the relationship between the cell potential and the pH values. It's a graph of one vs the other, just to show how much one varies with respect to the other. Question b) then becomes a lookup on the graph. And question c) is where you apply the Nernst formula to compensate for temp change. Others may disagree, and I would defer to more experienced chemists.