We have decided on the approximate conductivities corresponding to different numbers of ionizable groups. Now we need to see how well the two theories predict conductivities which correspond with experiment.

Continue to choose which theory matches the experimental evidence. Don't be concerned if the match isn't perfect. For Co(NH3)3(H2O)Cl3, for instance, the conductivity value is 393 even though only one ionizable group is expected. We noticed a color change when this compound dissolved coupled with an increase in conductivity. We suspect that the original compound is reacting with water to form a new one with more ionizable groups.

Good. You have made the correct choices for all nine metal ammines, I think this evidence should convince you that my theory is correct. It is true that aqueous solutions of two compounds, for which I predict one ionizable groups, have very high conductivities. I think this occurs because the compounds are reacting with water, forming new and more ionizable compounds.

We have decided on the approximate conductivities corresponding to different numbers of ionizable groups. Now we need to see how well the two theories predict conductivities which correspond with experiment. I think you will see that, in some cases, neither make the correct predictions.

Continue to choose which theory fits the experimental evidence. You may see why I think the conductivities are unreliable. for Co(NH3)4Cl3 and Co(NH3)3(H2O)Cl3 the conductivities are very high, even though both theories predict only one ionizable group.

Good. You have made the correct choices for all nine metal ammines. If you look closely at the data, I think you will see that the conductivity evidence is unconvincing. There are two compounds for which neither of our predictions agree with the conductivities.