Calculate the osmotic pressure (in torr) of 6.00 l of an aqueous 0.958 m solution at 30.°c, if the solute concerned is totally ionized into three ions (e. g., it could be na2so4 or mgcl2).

The osmotic pressure is 54307.94 Torr.

Explanation:

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

where,

= osmotic pressure of the solution = ?

i = Van't hoff factor = 3

C = concentration of solute = 0.958 M

R = Gas constant =

T = temperature of the solution =

Putting values in above equation, we get:

Hence, the osmotic pressure is 54307.94 Torr.

a graduated cylinder.

explanation:

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !