Calcium Nitrite (CA(NO3)2) is used as a corrosion inhibitor in lubricants. A sol

Question

Calcium Nitrite (CA(NO3)2) is used as a corrosion inhibitor in lubricants. A solution is prepared by dissolving 18.536g of calcium nitrite in 183.544g of distilled water. Calculate the boiling and freezing points of this solution.

Kb= 0.512 degrees C/m

Kf= 1.86 degrees c/ m

Molality of solution (m) i=(1+2)/1  ??? do not know what this part means

VON HOFFS Factor (i) ?

boiling pint elevation?

Boiling point of this solution?

Freezing point depression?

Freezing point solution?

will get full point if shown worked out step by step please

Explanation / Answer

Kf = 1.853 K kg/mol
Kb = 0.512 K kg/mol

?T = i x Kf x m

m = number of moles solute / mass of solvent (kg)



We can work out the molality of Ca(NO3)2from this

n (Ca(NO3)2) = m / MM = 18.536/ 164.088 g/mol = 0.11296 moles

We have 183.544g of solvent

molality = 0.11296mol / 0.183.544kg = 0.615mol/kg

i = 3 because Ca(NO3)2 in solution dissociates into Ca2+ and NO32- (3 ions)

?T = i x Kf x m = 3 x 1.853

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects