As far as I can tell, all you need to do to solve this problem is use the Nernst equation
V_(Ca^(2+)) = (RT)/(zF) * ln(([Ca^(2+)]_"out")/([Ca^(2+)]_text(in))), where
R - the universal gas constant;
z - the valence of the ion - in your case, this will be +2;
F - Faraday's constant;
[Ca^(2+)]_"out" - the concentration of the calcium cations outside the cell (in the extracellular liquid);
[Ca^(2+)]_"in" - the concentration of the calcium cations inside the cell (intracellular liquid)
The only thing to watch out for is the fact that the concentrations of the calcium cations are not given in the same unit, so you must convert one of them to the units of the other
12.0cancel("mmol")/"L"^(-1) * ("1000"mu"mol")/(1cancel("mmol")) = 12.0 * 10^(3)mu"mol L"^(-1)
The great thing about working at 37^@"C" is that you can use the Nernst equation like this
V = (RT)/(F) * 1/z * ln(([Ca^(2+)]_"out")/([Ca^(2+)]_text(in)))
V = underbrace(2.303 * (RT)/F)_(color(blue)("61.54 mV")) * 1/z * log(([Ca^(2+)]_"out")/([Ca^(2+)]_text(in)))
This means that you'll get
V_(Ca^(2+)) = "61.55 mV" * 1/2 * log((12,000cancel(mu"mol L"^(-1)))/(100cancel(mu"mol L"^(-1))))
V_(Ca^(2+)) = color(green)("+64.0 mV")