Question

1.) A 0.046 M aqueous solution of FeCl, has an osmotic pressure of 4.09 atm at 28°C. a. Calculate the percentage difference of the van't Hoff factor from the ideal value. b. What should be the concentration of this aqueous solution if this is in ideal condition?

Answer 1

Т. ₂ Bolk Saludion': The compound is feilty which disociates asi fel a Fe 3+3 a Giren, I =.409 atm c=0.046 M 2+273 R = 0.0821 lit atm molok Stou a disociating compounds i ox vant hoff factor is given as: 1 + (0-1)& where m is the number of particles formed after disociation & His the degree of disociation for fechge & ~ 100% or Utfor ionic compound ME 3+= 4 R- (a) i. Ideal rant-hoff factor 1+(4-1) 1 Lideal (+ 3 u

☺ for given data, tautual I ALE NCRT CRT u.oa atm 0.046 mol * 0 10821 il an x 3ok Qi LYC polok 3.597 2) do difference from actual value -4-3.597 x 100 4 10.07 of In ideal condition 14 ã IRT 9.09 4xo. 0821 × 301 0:0413 mit concentration of solution in ideal case)