If you have an electrolyte solution in which you have inserted an electrode to charge it either positive or negative

If you have an electrolyte solution in which you have inserted an electrode to charge it either positive or negative - and then you remove the electrode - is it possible to then magnetize this solution by any one or several methods?

Conductivity of acetic acid KCl solutions

The conductivity of a 0.1 moldm^-3 solution of potassium chloride at298K was found to be 1.1639 x 10^-2 Scm^-1. In a separate experiment at 298K the resistance of a 0.1 moldm^-3 solution of ethanoic acid was determined as 300 ohms and the resistance of the potassium chloride solution was fond to be 33.21 ohms. Given that the specific conductivity of the water used to prepare the ethanoic acid and potassium chloride solutions was 7.6 x 10^-4 Scm^-1 at 298K, calculate the molar conductivity of the ethanoic acid solution. (Tip: The conductivity of the solutions comprises the conductivity due to the salt or acid and the conductivity due to dissociated water)

20 Thermodynamics Problems: Equilibrium Constants and LeChatelier's Principle

Please see the attached file for the fully formatted problems. Given [N2] = 0.200 M, [H2] = 0.100 M and [NH3] = 1.18 x 10-1 M for the following reaction; N2(g) + 3 H2(g) à 2 NH3(g) at 350oC calculate the equilibrium constant. A. 85.2 B. 76.4 C. 54.6 D. 69.6 E. 60.5 4. Given [CO] = 0.250 M, [H2] = 0.120 and [CH3OH] = 0.0378 for the following reaction; CO(g) + 2 H2(g) CH3OH(g) at 500ºK calculate the equilibrium constant. A. 12.9 B. 9.6 C. 7.1 D. 10.5 E. 8.4 5. Given [N2O4] = 0.351 M and [NO2] = 4.94 x 10-2 M for the following reaction; N2O4(g) à 2 NO2(g) at 30ºC calculate the equilibrium constant. A. 4.50 x 10-3 B. 7.92 x 10-3 C. 3... click for more