Determine the amount of `CaCl_2` (I = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at `27^@C`.

If N_2 gas is bubbled through water at 293K how many milliomoles of N_2 would be dissoved in 1 litre of water? Assume that N_2 exert sa partial pressure of 0.987 bar. Given that Henrey's law constant for N_2 at 293K is 76.48K bar.

Determine the osmotic pressure of a solution prepared by dissolving 25 mg of K_2SO_4 in 2 liter of water at 25^@C , assuming that it is completely dissociated.

100 mg of a protein is dissolved in just enough water to make 10.0 mL of solution. If this solution has an osmotic pressure of 13.3mm Hg at 25^@C , what is the molar mass of the protein? (R = 0.0821L atm mol^-1 K^-1 and 760mm Hg = 1atm)

Determine x if log_5 {log_3 (log_2 x)}=0

Vapour pressure of pure water at 298K is 23.8 mm Hg. 50g of urea (NH_2CONH_2) is dissolved in 850 g of water. Calculate the vapour pressure of water for this solution and its relative lowering.

0.52g of glucose (C_6H_12O_6) is dissolved in 80.2g of water calculate the boiling point of the solution. ( K_b for water is 0.52 K kg mol^-1 ).

What is the density of SO_2 gas at 27^@C at 2 atmospheric pressure?(R = 0.08219 atm K^(-1) mol^(-1)

What concentration of nitrogen should be present in a glass of water at room temperature at 25^@C , a total pressure of 1 atm and mole fraction on nitrogen in air of 0.78 [ K_H for nitrogen = 8.42xx10^(-7)M//mmHg ].

Calculate the osmotic pressure in pascal exerted by a solution prepared by dissolving 1.0g of polymer of molar mass 185,000 in 450 mL of water at 37^@C .

Compute the bulk -modulus of water from the following data: Initial volume = 100.0 litre, Pressure increase = 100.0 atm (1 atm = 1.013 xx 10^5 Pa) , Final volume = 100.5 litre. Compare the bulk modulus of water with that of air (at constant temperature). Explain in simple terms why the ratio is so large.