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PH of 0.1M BOH (weak base) is found to be 12.The solution at temperatureTk will display an osmotic pressure equal to A.0.01RT B.0.01(RT)2 C.0.11RT D.1.1RT Answer is C?
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PH of 0.1M BOH (weak base) is found to be 12.The solution at temperatu...

Calculation of Osmotic Pressure at Temperature Tk

- The pH of a 0.1M solution of a weak base, such as BOH, can be used to determine the concentration of hydroxide ions in the solution. In this case, a pH of 12 indicates a pOH of 2 (since pH + pOH = 14).

- Using the pOH value, we can calculate the concentration of hydroxide ions ([OH-]) in the solution. Since BOH is a weak base, we can assume that the concentration of OH- is equal to the concentration of BOH that has dissociated.

- With the concentration of OH- known, we can calculate the osmotic pressure of the solution using the formula: π = nRT, where n is the concentration of the solute in mol/L, R is the gas constant, and T is the temperature in Kelvin.

- Substituting the values into the formula, we get: π = 0.1 * R * Tk

- Since R is a constant, the osmotic pressure is directly proportional to the temperature T. Therefore, the osmotic pressure at temperature Tk will be 0.1 * R * Tk, which corresponds to option C.

Therefore, the correct answer is option C: 0.11RT.
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PH of 0.1M BOH (weak base) is found to be 12.The solution at temperatureTk will display an osmotic pressure equal to A.0.01RT B.0.01(RT)2 C.0.11RT D.1.1RT Answer is C?
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