What mass of sucrose (C12H22O11) should be combined with 546 g of water to make a solution with an osmotic pressure of 8.80 atm at 290 K ? (Assume the density of the solution to be equal to the density of the solvent.)

The mass of sucrose required is 69.08 g

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

Or,

where,

= osmotic pressure of the solution = 8.80 atm

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (sucrose) = ?

Molar mass of sucrose = 342.3 g/mol

Volume of solution = 564 mL    (Density of water = 1 g/mL)

R = Gas constant =

T = Temperature of the solution = 290 K

Putting values in above equation, we get:

Hence, the mass of sucrose required is 69.08 g

water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.