The osmotic pressure of a solution is calculated using the formula Π=MRT where Π is the osmotic pressure in atm, M is the molarity, R is the ideal gas constant, and T is the kelvin temperature. Part A What is the osmotic pressure of a solution made by dissolving 40.0 g of glucose, C6H12O6, in enough water to form 700.0 mL of solution at 37.0 ∘C ? Express your answer to three significant figures and include the appropriate units. nothing nothing

Osmotic pressure of the solution will be 818.203 Pa.

Explanation:

Osmotic pressure of a solution is defined by the formula,

π = MRT

where π = Osmotic pressure

M = Molarity of the solution

R = Ideal gas constant

T = Temperature in °K

40 grams of glucose was dissolved in water so the Molarity of the solution will be,

M =

Moles of solute =

                          =

                          = moles

Morarity =

              = 0.3175 mole per liter

Value of ideal gas constant 'R' = 8.314

T = 37°C = (273 + 37)° K

              = 310°K

Now by substituting these values in the formula,

π =

  = 818.203 Pa

Therefore, osmotic pressure of the solution will be 818.203 Pa.

in chemistry, a solution’s concentration is how much of a dissolvable substance, known as a solute, is mixed with another substance, called the solvent. the standard formula is c = m/v, where c is the concentration, m is the mass of the solute dissolved, and v is the total volume