Calculate the osmotic pressure (in torr) of 5.50 L of an aqueous 0.148 M solution at 29°C if the solute concerned is totally ionized into three ions (for example, it could be Na₂SO₄ or MgCl₂). A) 8.37 * 10³ torr B) 2.71 * 10⁴torr C) 2.79 *10³ torr D) 3.52*10^-1 torr E) 8.03 *10² torr

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The correct answer is A because the osmotic pressure is given by the equation:π = MRTwhere:π is the osmotic pressure in torrM is the molarity of the solution in mol/LR is the ideal gas constant in L·torr/(mol·K)T is the temperature in KelvinIn this case, we have:M = 0.148 MR = 62.36 L·torr/(mol·K)T = 29°C + 273.15 = 302.15 KSubstituting these values into the equation, we get:π = (0.148 M)(62.36 L·torr/(mol·K))(302.15 K) = 2.79 × 10^3 torrTherefore, the osmotic pressure of the solution is 2.79 × 10^3 torr.

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