Solution A contains 7g/L of MgCl2 and Solution B contains 7g/L of NaCl. At room temp, Osmotic pressure ofa)ABb)A=Bc)BAd)Insufficient informationCorrect answer is option 'C'. Can you explain this answer?

Question

Solution A contains 7g/L of MgCl2 and Solution B contains 7g/L of NaCl. At room temp, Osmotic pressure ofa)A>Bb)A=Bc)B>Ad)Insufficient informationCorrect answer is option 'C'. Can you explain this answer?

Answer

The osmotic pressure of a solution depends on the concentration of solute particles in the solution, not the identity of the solute particles. Therefore, the osmotic pressure of Solution A and Solution B would be the same if they have the same concentration of solute particles.

Since both Solution A and Solution B have a concentration of 7g/L, we can calculate their osmotic pressure using the formula:

Osmotic pressure = MRT

where M is the molarity of the solution (in moles/L), R is the gas constant (0.0821 L·atm/mol·K), and T is the temperature (in Kelvin).

To convert the concentration of Solution A and Solution B from grams/L to moles/L, we need to divide by their respective molar masses. The molar mass of MgCl2 is 95.21 g/mol, so the molarity of Solution A is:

Molarity of Solution A = (7 g/L) / (95.21 g/mol) = 0.0735 mol/L

The molar mass of NaCl is 58.44 g/mol, so the molarity of Solution B is:

Molarity of Solution B = (7 g/L) / (58.44 g/mol) = 0.1198 mol/L

Assuming room temperature is 25°C, or 298 K, we can calculate the osmotic pressure of Solution A and Solution B:

Osmotic pressure of Solution A = (0.0735 mol/L)(0.0821 L·atm/mol·K)(298 K) = 1.76 atm

Osmotic pressure of Solution B = (0.1198 mol/L)(0.0821 L·atm/mol·K)(298 K) = 2.86 atm

Therefore, the osmotic pressure of Solution A is 1.76 atm and the osmotic pressure of Solution B is 2.86 atm.

Answer

If we go acc to π= iCRT than ans should be A

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