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What is the osmotic pressure of 0.0138 M KBr at 25 degrees Celsius?

User LInsoDeTeh
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1 Answer

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Final answer:

To find the osmotic pressure of a 0.0138 M KBr solution at 25 degrees Celsius, convert the temperature to Kelvins, double the molarity for the complete ionization of KBr, and apply the osmotic pressure formula Π = MRT using the ideal gas constant.

Step-by-step explanation:

To calculate the osmotic pressure of a 0.0138 M KBr solution at 25 degrees Celsius, we need to use the osmotic pressure equation Π = MRT, where Π is the osmotic pressure, M is the molarity of the solution, R is the ideal gas constant (0.0821 L·atm/K·mol), and T is the temperature in Kelvins. First, convert the temperature from Celsius to Kelvins by adding 273.15 to the Celsius temperature, which gives us 298.15 K. As KBr is a strong electrolyte that fully dissociates into two ions, K+ and Br-, the total concentration of particles in solution is double the concentration of KBr, so we have (2)(0.0138 M) = 0.0276 M.

Now we plug these values into the formula:

Π = (0.0276 mol/L) [0.0821 (L·atm)/(K·mol)] (298.15 K)

Multiply these together to find the osmotic pressure.

User Kalyan Raghu
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