PLEASE SHOW STEPS Calculate the effective osmotic pressure o

PLEASE SHOW STEPS!

Calculate the effective osmotic pressure of each AND predict what will happen to cell volume if a cell is placed in each of the following solutions?

Solution

For a given problem, the osmotic pressure depends only upon the molar concentration of the solute but does not depend on its nature.

The following relation relates osmotic pressure to the number of moles of a solute

PV = nRT Van\'t Hoff \'s solution equation (p = Osmotic pressure)

or

=nv RT =nvRT

but,

nv =C nv=C

Therefore,

P = CRT

where,
C = Concentration of the solution in moles per liter ( Here C is in mM, So C will be 10 ^-3 moles/lt
R = Gas constant
T = Temperature
n = Number of moles of the solute
v = Volume of the solution in liters

Effective Pressure = C\'RT= (i*C1-C2)RT where we have taken 2*C1 as for NaCl , a strong electrolyte- i=2

Solution A -->Pa= (2*150-100)*.082*273*10 ^-3= 4.46 atm

Solution B --> Pb= (2*100-150)*.082*273*10 ^-3=1.1193 atm

Solution C --> Pc= (2*200-100)*.082*273*10 ^-3=6.67 atm

Solution D --> Pd= (2*100-50)*.082*273*10 ^-3=3.36 atm

Osmosis: Is the movement of solvent through semipermieable membrane from lower concentration towards higher concentrtion.

So according to defination :

Solution A: A solution containing 300 mOsmol/L of nonpenetrating solutes,it will be Isoosmotic and thus no cell volume change

Solution B and Solution D:A solution containing less than 300 mOsmol/L of nonpenetrating solutes,it will be Hypoosmotic and thus cell swells, increase in cell volume

Solution C: A solution containing more than 300 mOsmol/L of nonpenetrating solutes,it will be Hyperosmotic and thus cell shrinks, decrease in cell volume