What is the osmotic pressure in mmHg of 2.00 L of a 1.34 × 10^-3 M solution at 25 °C if four moles of ions are produced in aqueous solution for every mole of solute dissolved?

Question

Quizplus · Accepted Answer

First, we need to calculate the molarity of the solution:
1.34 × 10^-3 mol/L x 4 = 5.36 × 10^-3 mol/L
Next, we can use the formula for osmotic pressure:
π = MRT
where π is the osmotic pressure, M is the molarity of the solution, R is the gas constant (0.08206 L atm/mol K), and T is the temperature in Kelvin (25°C = 298 K).
π = (5.36 × 10^-3 mol/L)(0.08206 L atm/mol K)(298 K)
π = 0.131 atm
Finally, we convert atm to mmHg:
0.131 atm x 760 mmHg/atm = 99.6 mmHg
Therefore, the answer is C.

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