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Calculate the freezing point of the one molar aqueous solution (density 1.04 g L^(-1)) of KCl (k(f) for wateer = 1.86 kg mol^(-1) , atomic mass of K = 39 ,Cl = 35.5)
Calculate the heat of formation of KCl from the following data : {:((i),KOH(aq)+HCl(aq)rarr KCl(aq)+H(2)O(l)",",,Delta H=-57.3 kJ mol^(-1)),((ii),H(2)(g)+(1)/(2)O(2)(g)rarr H(2)O(l)",",,Delta H=-286.2 kJ mol^(-1)),((iii),(1)/(2)H(2)(g)+(1)/(2)Cl(2)(g)+ ...
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![A solution containing 0.5g of KCl dissolved in 100g of water and freezes at 0.24^oC . Calculate the degree of dissociation of the salt. ( Kf for water = 1.86^oC . Atomic weights [ K = 39,Cl = 35.5 ].](https://i.ytimg.com/vi/2Golq6neWdM/maxresdefault.jpg "A solution containing 0.5g of KCl dissolved in 100g of water and freezes at 0.24^oC . Calculate the degree of dissociation of the salt. ( Kf for water = 1.86^oC . Atomic weights [ K = 39,Cl = 35.5 ].")
A solution containing 0.5g of KCl dissolved in 100g of water and freezes at 0.24^oC . Calculate the degree of dissociation of the salt. ( Kf for water = 1.86^oC . Atomic weights [ K = 39,Cl = 35.5 ].
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Calculate the freezing point of a solution containing `0.5 ` g KCl (Molar mass = `74.5 ` g/mol) - YouTube
