An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 ml of solution. the solution has an osmotic pressure of 1.2 atm at 25 °c. what is the molar mass (g/mole) of the compound?

Answer : The molar mass (g/mole) of the compound is, 2707.55 g/mole

Solution : Given,

Mass of solute = 33.2 g

Volume of solution = 250 ml = 0.250 L

Temperature of solution =

Formula used for osmotic pressure :

where,

= osmotic pressure

V = volume of solution

R = solution constant  = 0.0821 L.atm/mole.K

T= temperature of solution

M = molar mass of solute

w = mass of solute

Now put all the given values in the above formula, we get the molar mass of the compound.

Therefore, the molar mass (g/mole) of the compound is, 2707.55 g/mole

the ratio of the conjugate base to the acid required to attain the desired ph.

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.