a mixture is made by mixing 500mL of substance x, an electrolyte with a van\'t h

Question

a mixture is made by mixing 500mL of substance x, an electrolyte with a van't hoff factor of 2 ( density = 1.25 g/mL;Molar mass = 55.00g/mol) and 1000mL of water (density=1.00g/mL) at 20 degrees celsius .The density of the mixture is 1.114g/mL. express the concentration of substance x as

a) volume percent

b) molarity

c)molality

D) mole fraction

Given the vapor pressure of pure water at 20degrees celsius is 17.5 torr. what is the freezing point of the solution? (water Kf=1.86)

Chem 114 Question of the Day Chapter 12 Q. A mixture is made by mixing van 't hoff factor of2 (density = 1.25 g/mL; Mlolar Mass-55.00 g/mol) and 1000 500 mL of substance X, an electrolyte with a of water (density 1.00 g/mL) at 20°C. The density of the mixture is 1.114 g/mL. Express the concentration of substance X as Volume Percent, Molarity, Molality & Mole Fraction. Given the vapor pressure of pure water at 20°C is 17.5 Torr, what is the freezing point of the solution? (Water Kf 1.86)

Explanation / Answer

a) volume percent = vol.of solute / vol.of solution*100

                  = 500/(1000+500)*100

                  = 33.33%

b) molarity(M) = (w/M)*(1000/v)

            = ((1.25*500)/55)*(1000/1500)

            = 7.6 M

c) molality(m) = (w/M)*(1000/W)

               = ((1.25*500)/55)*(1000/(1000*1))

               = 11.364 m

d) molefraction of substance = nsubstance/ntotal

     = ((1.25*500)/55)/(((1.25*500)/55)+(1000/18))

     = 0.17
molefraction of water= 1-0.17 = 0.83

DTf = i*kf*m

(0-x) = 2*1.86*11.364

x = freezing point of the solution = -42.3 C

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