Final answer:
To find electric conductivity between two acids, classify each one as a strong or weak electrolyte, use an ICE table for weak electrolytes like acetic acid to find ion concentration, and relate this to their electric conductivity.
Step-by-step explanation:
Understanding Conductivity and Acid Dissociation
To find the electric conductivity between two acids given their molar concentrations, one must understand how the acids dissociate in solution. Acetic acid (CH₃COOH), being a weak acid, partially dissociates in water. The dissociation of acetic acid can be analyzed using an ICE table (Initial, Change, Equilibrium) which takes into account the initial molarity of the acetic acid, the dissociation constant (Ka), and the equilibrium concentrations of the ions and the undissociated acid.
To calculate electric conductivity, classify each acid as a strong or weak electrolyte. For a strong electrolyte, the concentration of ions will be equal to its molarity, multiplied by the number of ions per formula unit. Weak electrolytes like acetic acid will have fewer ions in solution due to their incomplete dissociation. The molarity of these ions can be determined from the ICE table and the initial molarity. By understanding the concentration of the ions, one can infer the molar solubility and relate it to the electric conductivity.
Remember that conductivity measurements can provide insight into whether a substance is a strong, weak, or non-electrolyte based on how much electrical current they conduct compared to pure water and other standard electrolytes, as shown in tables such as TABLE 9.4.1.