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Solved in 2 steps
- Define conductivity and molar conductivity for the solution of an electrolyte. Discuss their Variation with change in temperature.The molar conductivity of a 1.5 M solution of an electrolyte is found to be 138.9 S cm2mol-1. Calculate the conductivity of the solution.The electrolytic conductivity of a 0.1 M solution of acetic and was found to be 503 X 104 n'cm'. Calculate the molar conductivity.
- The electrolytic conductivity of a 0.1 M solution of acetic acid was found to be 5.3x 10ʻn'cm". Calculate the molar conductivity.Describe Kohlarausch's law in mathematical terms and explain how to calculate the neural molar conductivity of a series of electrolyte solutions with known concentrations and molar conductivity.The mean activity coefficient of a 0.010 m H2SO4 solution is 0.544. What is its mean activity?
- how can the kolrausch plot be used to determine if an electrolyte is strong or weak?Describe the general features of the Debye-Huckel theory of electrolyte solutions. Which approximations limit its reliability to very low concentrations?True or False For strong electrolytes, such as hydrochloric acid, the molar conductivity decreases slightly as the concentration is increased.
- For weak electrolytes, such as acetic acid, at very low concentrations the molar conductivity drops rapidly as the concentration increases. However, at higher concentration, there’s only a slight decrease in the molar conductivity. True Falseb) In one conductivity cell, the resistance of a 0.1 M KCl solution is 1.5x102 Ω. The knownmolar conductivity of the solution is 101 Ω-1 cm2 mol-1 . Calculate the cell constant, Kcell. (Kcell unit is cm-1).Estimate the mean ionic activity coefficient and activity of a solution that is 0.015 mol kg-1 MgF2(aq) and 0.025 mol kg-1 NaCI(aq).