Conductometric techniques were used to investigate solvent-solvent interactions of CoCl2 solutions with varying methanol/water compositions with and without added NaCl electrolyte. CoCl2 dissolved more in pure water, showing greater ion dissociation, while in pure methanol it formed less dissociated organo-complexes. Addition of NaCl increased conductance more as ions dissociated before complexing. More dissociation and complex formation occurred with increasing water content. Concentration, density, and viscosity were also influenced.

2.  Aroosa Shafait
 Benish Shafiq
 Naveed Sultan
 Supervised by:
 Sir, Zain-ul- abdin

3.  Condctrometric Investigation Of Solvent- Solvent
Interactions Of Transition Metal Electrolyte
(Cocl2.6h2o) In Neat Water And Methanol In
Presence Of Added Electrolyte (Nacl)

5.  During the conductrometric investigation of solvent-solvent
interaction metal Co+2 electrolyte used, NaCl and Methanol used
as solvent. In this method salvation behaviorof Co+2 in the
presence of added electrolyte (NaCl) is investigated in pure
water, in pure methanol and then different mole percentages of
Methanol. As Methanol and water both posses OH group so they
have resemblance in many physical properties. Hence increase in
conductance in pure water show great dissociation constant then
Methanol. When Electrolyte is added in CoCl2 solution of pure
water, ion salvation of Co+2 start. The ion salvations continue
until the complex formation completed. In the case of CoCl2
solution in pure Methanol, after adding electrolyte show less
degree of dissociation and complex formation. As the amount of
water increases, ion dissociates more frequently. Concentration
also effect density and viscosity values, as concentration
increases both increases (density & viscosity).

6.  The objective of the study is the conduct metric
investigation of solution containing two electrolytes in
the solvent system and comparing them with those
measured in the neat solvent containing one electrolyte.
Variation in conduction may be carried out in the
solution where the concentration of the transition metal
and the electrolyte are changed symmetrically which
leads to draw useful conclusion about ion-solvent
interactions.

7.  Definition
 Measurement of the electrical conductivity of a
solution during the course of a chemical reaction. It is
the determination of the quantity of a material present
in a mixture by measurement of its effect on the
electrical conductivity of the mixture.

8. Electrolytic conductance.
 Electronic conductance.
 Metallic conductance.

9.  Definition:
The word "viscosity" is derived from the Latin
"viscum", meaning mistletoe. A viscous glue called
birdlime was made from mistletoe berries and was used
for lime-twigs to catch birds.

10.  Definition :
 The mass density or density of a material is
its mass per unit volume. The symbol most
often used for density is ρ (the lower case
Greek letter rho). Mathematically, density is
defined as mass divided by volume:

11.  Nature of electrolyte:
 The conductance of an electrolyte depends upon the
number of ions present in the solution. Therefore, the
greater the number of ions in the solution the greater is
the conductance.
 Concentration of the solution:
 The molar conductance of electrolytic solution varies
with the concentration of the electrolyte. In general, the
molar conductance of an electrolyte increases with
decrease in concentration or increase in dilution.
 Temperature: The conductivity of an electrolyte depends
upon the temperature. With increase in temperature, the
conductivity of an electrolyte increases.

12. Solubility of Sparingly Soluble Salts
 Hydrolysis of Salts
 Rates of Reaction Solution, Diffusion
 Conductmetric Titrations

13.  Apparatus:
 Chemicals:
 Methanol
 CoCl2.6H2O
 NaCl
 KCl

26.  CO+2 has d7 configuration and a radius of
72pm.
 Cobalt is fairly soluble in neat water with
resulting light pink to rosy red color of
solution conductance measured over an
entered CoCl2 concentration range from
0.2, 0.3, 0.4, 0.6, 0.8, 0.1M.

27.  Effect of Electrolyte
When NaCl is added in Solution individually increase in
conductance show increase in ion dissociation of electrolyte.
 Solution of CoCl2 in 80% CH3OH:
 Effect of Electrolyte
When electrolyte is added in solution firstly dissociation of
ions takes place which cause increase in conductance then
equilibrium is establish.

28.  Solution of CoCl2 in 50% CH3OH:
Effect of Electrolyte
When electrolyte NaCl is added to solution it is observed
that both aqua and organo-complex is formed after
dissociation of CoCl2 into its respective ions.
Solution of CoCl2 in 20% CH3OH:
Effect of Electrolyte
When electrolyte NaCl is added to solution it show similar
behavior as complex formation takes place and after
complex formation equilibrium is established.

29.  Solution of CoCl2
 Is prepared in pure water and pure methanol along with different
concentrations of methanol as 100%, 80%, 50% and 20% to check
conductance before and after indication of electrolyte (NaCl). It is conclude
that:
 Ion dissociation takes place more in solution of CoCl2 in water.
 Co+2 form aqua-complex with water which is octahedral and it form
organo-complex with methanol which is tetrahedral.
 After addition of NaCl as electrolyte conductance increases more vigorously.
 Ions of electrolyte and methanol both solvates Co+2 but it form complex
with that legend which is stronger or greater in concentration.
 When there is no increase in conductance, it means complex formation is
completed.
 Concentration also effects viscosity and density. As concentration increases
viscosity and density also increases.