Part B Using the van\'t Hoff factors in the table below calculate the mass of so

Question

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 Solste Expected Me Express your answer using two significant figures. Expected Measured Nonelectrolyte1 NaCl MgSO4 2 MgCh K2SO4 FeCl 1.9 1.3 2.7 2.6 3.4 You may want to reference Submit (Pages 569-572) Section 13.7 while comnletinn

Explanation / Answer

B)
P = 2.94atm
T = 311 K


use:
P = i*C*R*T
2.94 = 1.3*C*0.0821*311.0
C =0.0886 M

volume , V = 259 mL
= 0.259 L


use:
number of mol,
n = Molarity * Volume
= 0.0886*0.259
= 2.294*10^-2 mol

Molar mass of MgSO4,
MM = 1*MM(Mg) + 1*MM(S) + 4*MM(O)
= 1*24.31 + 1*32.07 + 4*16.0
= 120.38 g/mol

use:
mass of MgSO4,
m = number of mol * molar mass
= 2.294*10^-2 mol * 120.38 g/mol
= 2.8 g
Answer: 2.8 g

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