Chapter 13 Exercise 13.88 -Enhanced - with Feedback ) 70110 Constants I Periodic

Question

Chapter 13 Exercise 13.88 -Enhanced - with Feedback ) 70110 Constants I Periodic Table Part B Using the van't Hoff factors in the table below calculate the mass of solute required to make each aqueous solution. Calculate the mass of solute required to make 2.59x102 mL of a magnesium sulfate solution that has an osmotic pressure of 3.94 atm at 311 K Van't Hoff factors at 0.05 m concentration in aqueous solution Solute Expected Measured Express your answer using two significant figures. Nonelectrolyte 1 NaCl MgSO4 MgClh K2SO4 FeCl 1.9 1.3 2.7 2.6 3.4 You may want to reference Pages 569-572) Section 13.7 while completing Submit

Explanation / Answer

Osmotic pressure (PI)= iCRT

i= Van't Hoff factor for MgSO4, it splits into Mg+2 and SO4-2 ions i=2

C= concentration of MgSO4, R= gas constant =0.0821 L.atm/mole.K, T= 311K

Given osmotic pressure = 3.94= 2*C*0.0821*311

C= 3.94/(2*0.0821*311) =0.077 moles/L

1 liter of solution contains 0.077 moles of MgSO4, 2.59*100ml = 2.59*100/1000L =0.259L

0.259 L of solution contains 0.077*0.259/1=0.0199 moles of MgSO4

molar mass of MgSO4= 120.4 g/mole, mass of MgSO4= moles* molar mass =0.0199*120.4=2.4 gm

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