Limiting molar conductivity of Mg^(2+) and Cl^(-) ions in water is 106.0 and 76.3 S cm^2 "mol"^(-1) . The limiting molar conductivity of magnesium chloride (in Scm^2 " mol"^(-1) ) in water is
Molar conductivity (^^_m) is defined as conducting power of the ions produced by 1 mole of an electrolyte in a solution. ^^_m =(K)/(C) where K is conductivity (in S-cm^(-1) ), ^^_m is molar conductivity (in Scm^(2) mol^(-1) ) and C is molar concontration (in "mole"//cm^(3) ) The molar conductivity of 0.04 M solution of MgCl_2 is 200Scm^2 mol^(-1) at 298 K. A cell with electrodes that are 2.0cm^(2) in surface area and 0.50 cm apart is filled with MgCl_2 solution. The cell constant is
For an electrolytic solution of 0.05 mole "litre"^(-1) , the conductivity has been found to be 0.0110 S cm^(-1) . The molar conductivity (in Scm^(2) "mole"^(-1) ) is
The molar specific heat for solid is
The molar specific heat for water molecules
Resistance of a conductivity cell filled with a solution of an electrolyte of concentration 0.1M is 100Omega . The conductivity of this solution is 1.29 S m^(-1) . Resistance of the same cell when filled with 0.02M of the same solution is 520 Omega . The molar conductivity of 0.02M solution of the electrolyte will be
Conductors allow the passage of electric current through them. Metallic and electrolytic are the two types of conductors. Current carriers in metallic and electrolytic conductors are free electrons and free ions respectively. Specific conductance or conductivity of the electrolyte solution is given by the following relation: K= cx (l)/(A) where, c=1/R is the conductance and 1/A is the cell constant, Molar conductance (^^_m) and equivalence conductance (^^_e) of an electrolyte solution are calculated using the following similar relations: ^^_m = K xx (1000)/(M) ^^_(e) = K xx (1000)/(N) where, M and N are the molarity and normality of the solution respectively. Molar conductance of strong electrolyte depends on concentration : ^^_m = ^^_m^(0) - b sqrt(C) ^^_m^(0) = molar conductance at infinite dilution C = concentration of the solution b = constant The degrees of dissociation of weak electrolytes are calculated as alpha = (^^_m)/(^^_m^(0)) = (^^_e)/(^^_e^(0)) Which of the following decreases on dilution of electrolytic solution?
