Exercise 13.88 -Enhanced - with Feedback c) 70f 10 (> Constants I Periodic Table

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Exercise 13.88 -Enhanced - with Feedback c) 70f 10 (> Constants I Periodic Table Using the van't Hoff factors in the table below calculate the mass of solute required to make each aqueous solution. Part B Van't Hoff factors at 0.05 m concentration in aqueous solution Solute Calculate the mass of solute required to make 2.59-102 mL of a magnesium sulfate solution that has an osmotic pressure of 394 atm at 311 K Expected Measured Express your answer using two significant figures. Nonelectrolyte 1 NaCl MgSO, MgCl K2SO FeCls 1.9 1.3 2.7 2.6 3.4 You may want to reference Pages 569-572) Section 13.7 while completing this problem. Submit Previous Answers Request Answer

Explanation / Answer

we know,

osmotic pressure = i * c * R * T

0.94 = 2 * C * 0.0821 * 311

C = 0.0184 M

concenntration of MgSO4 = 0.0184 M

moles of MgSO4 = 0.0184 * 2.59 * 10^2 / 1000 = 4.77 * 10^-3 mole

4.77 * 10^-3 mole MgSO4 = 4.77 * 10^-3 * 120.366 = 0.57 gm (answer)

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