Theory predicts that the molar conductance of a solution of a weak electrolyte should increase as the solution becomes increasingly dilute, ultimately reaching the sum of the molar conductances of the individual ions that make up the electrolyte at infinite dilution. So, for example, the molar conductance of acetic acid (vinegar) in water will approach the sum of the molar conductances of the proton and the acetate ion, H++Ac=0.039071m2mol1 as the solution is diluted. The independent variable in the theory is the square root of the concentration. The data collected in a physical chemistry lab experiment is graphed against c in the figure shown. One group, trying to earn some bonus points, fit the data using CurveExpert and found that the Weibull model yielded the best fit. The model is y=abexp(c/xd) where a= 0.00819,b=0.00775,c=0.00452,d=1.524, and x is the square root of the concentration. Even though the fit is fairly good (as shown), what is wrong with this model? Select one: a. There is nothing wrong with this fit. The instructor of this course is losing his mind. b. They should have used a model that has the square root of x. c. The model becomes singular (division by 0!) at the infinite dilution limit x0. d. The model predicts that the conductance of a concentrated solution is zero, contrary to experimental x evidence. e. The model has a singularity at x=0 and so it does not yield the desired infinite dilution behavior