1. A salt solution approximating ocean water would have the following ionic mola

Question

1. A salt solution approximating ocean water would have the following ionic molalities: chloride, 0.566 m; sodim, 0.485 m; magnesium,, 0.054 m; sulfate, 0.029 m; calcium 0.011 m; potassium, 0.011 m; bicarbonate, 0.002m.. At 20 0C the vapor pressure of pure water is 17.5 torr. The vapor pressure of this "ocean water solution would be about ____________% less than that of the pure water at 20 0C.

2. The melting point of KCl is less than that of NaF by some 200 0C. The primary reason for this is that:

a. potassium and chloride ions have greater charges than Na+ and F-

b. the internuclear distance in KCl is greater than that in NaF

c. the differences in electronegativity between K and Cl is greater than that between Na and F

d. KCl molecules are more polar than NaF molecules

e. the formula weight of KCl is greater than that of NaF

Explanation / Answer

Total molality = 0.566 + 0.485 0.054 0.029 + 0.011 + 0.0 11+ 0.002 = 1.158 molal

relative lowering = molality X mol wt of solvent / 1000

% less of pressure = 1.158 X 18 x 100 / 1000 = 2.08 %

2) the strenght of ionic bonds depends upon the charge on ions and size of ions

As the size of chloride ion is more than Flouride ion and it is less electronegative also.

So due to this the the internuclear distance in KCl is greater than that in NaF

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