Question

The osmotic pressure, π, of a solution of glucose is 132 atm . find the molarity of the solution at 298 k.

Answer 1

The molarity of the glucose solution at 298 K is approximately 0.00527 M.

Step-by-step explanation:

The osmotic pressure, π, of a solution can be calculated using the formula II = MRT, where M is the molarity of the solution, R is the ideal gas constant (0.08206 L atm/mol K), and T is the temperature in Kelvin. In this case, the osmotic pressure is given as 132 atm and the temperature is 298 K. We can rearrange the formula to solve for M:

M = π / (RT)

Substituting the values:

M = 132 atm / (0.08206 L atm/mol K × 298 K)

M ≈ 0.00527 M

Answer 2

The formula for osmotic pressure is:

`\Pi = iMRT`

where
`\Pi` is osmotic pressure,
`i` is van't Hoff's factor,
`M` molarity,
`R` is Ideal gas constant, and T is Temperature.

`\Pi` = 132 atm

The van't Hoff's factor for glucose,
`i` = 1

`R = 0.08206 Latmmol^(-1)K^(-1)`

`T = 298 K`

Substituting the values in the above equation we get,

`132 atm = 1* M* 0.08206 Latmmol^(-1)K^(-1)* 298`

`M = (132 atm)/(1* 0.08206 Latmmol^(-1)K^(-1)* 298) = 5.4797 molL^(-1) \simeq 5.48 molL^(-1)`

So, the molarity of the solution is
`5.48 molL^(-1)`.