Question

1. A solution was prepared by dissolving 2.20g of urea (H2NCONH2) in 50.00g of water. If for H2O Tb = 100C, Tf = 0C, Kb = 0.52C / m and Kf = 1.86C / m, determine the freezing and boiling point of the solution.

2. A solution is prepared by dissolving 17.41g of a substance X in 600g of benzene and the resulting solution is frozen at 4.00C. If the freezing point of pure benzene is 5.55C and its Kf is 5.10C / m, determine the molar mass of X.

3. A solution was prepared by dissolving 35.0g of hemoglobin (Hb) in 1.00L of solution. If the osmotic pressure measured at 25C was 10.0mmHg, determine the molar mass of hemoglobin.

Answer 1

kindly poat different questions separately. pleass rate

= 60.0 g/mol molar mass of urea max of uren = 2.209 moles of urea = mass molar may mass of water = 50.00g = = 2,209 = 0.0367 mol Googlmol 0.05 kg (u. 1000 g = 1kg) 0.0367 mol molality of solution = m = moles of urea mass of water 0.05 kg ml= 0.734 m la van't hoff factor 1=1 for urea boiling point of water = Too = 100°C boiling point of solution = To = ? IT= To-Too and ko= 0.52-c/m using colligative property, depo elevation in bolling point AT= (kbm To-Too = 1 kom. To - 100°C = 1 X 0.52 °C/m X 0.734m To= 100.37°C b) freezing point of water. To = 0.0°C freezing point of solution - To AT = To TF Kf = 1.860 lm using colligative property, depression in freezing point AT - l' kam → Too - Tp = 1x 1.86 Clm X 0.734m - t 0.0°C - TF = 1x1.86 Clm X 0.734m TE = -1,37°C