The more ions in a solution, the more conductive it will be but solubility alone does not determine the conductivity of a solution. Only the compounds that dissociate into component ions can conduct electricity, as the ions support the flow of electricity with their charges. For example, ethanol and sucrose are observed to be non-conductive, measuring 0-38 µS/cm each despite the solubility of each; this degree of conductivity matches that of distilled water. The soluble nitrate salts, KNO3, Cu(NO3)2, and AlNO3, however, are more conductive, being found experimentally to have conductivities of 1873, 2369, and 3860 µS/cm, respectively; these are strong electrolytes as they are very conductive. While the acids are all electrolytes, acetic acid is only a weak electrolyte, not completely dissociating in the water. Phosphoric acid and hydrochloric acid are strong electrolytes also, but H3PO4is more conductive than HCl, having conductivities of 2522 and 1987 µS/cm, respectively. It is important to utilize the same
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