Question

3a. Calculate the molar mass (in g/mol) of an unknown 1:1 electrolyte if 0.482 g dissolved in 223.1 mL of water at 74.75 °C has an osmotic pressure of 54.4 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures.

3b. Calculate the required mass of an unknown nonelectrolyte (ℳ = 131.5599 g/mol) dissolved in 140.1 g of solvent that gives a solution that boils at 36.04 °C. The boiling point of the pure solvent is 29.40 °C and its Kb value is 3.61 °C/m. Report your answer to TWO places past the decimal.

3c. Calculate the osmotic pressure (in atm) of a solution that is made from 1.07 g of a 1:1 electrolyte (ℳ = 137.9729 g/mol) dissolved in enough water to give 604 mLof solution at 21.44 °C. R = 0.082058 L⋅atm⋅mol−1⋅K−1. Report your answer to THREE significant figures

3d. When a solution is made from 31 g of an unknown nonelectrolyte dissolved in 177.3-9.83 °C. The freezing point of the pure solvent and its Kf are -4.56 °C and 2.84 °C/m, respectively. Calculate the molar mass of the unknown electrolyte in g/mol. Report your answer to TWO places past the decimal.

3e. Calculate the molar mass (in g/mol) of an unknown nonelectrolyte if 0.227 g dissolved in 203.4 mL of water at 17 °C has an osmotic pressure of 62.5 mmHg. R = 0.082058 L⋅atm⋅mol−1⋅K−1. 1.00 atm = 760 mmHg. Report your answer to THREE significant figures.

Answer 1