The osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25 °C. Assuming ideal solution behavior, what is the molar mass of insulin? Enter the pressure in kPa [p] and temperature in degrees Celsius [c]?
Added by Erica W.
Step 1
We know that 1 torr is approximately equal to 0.133322 kPa. So, 23 torr would be 23 * 0.133322 = 3.0664 kPa. Show more…
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