Assuming the vant Hoff factors in Table 12.9 , calculate the mass of solute required to
Chapter 12, Problem 92(choose chapter or problem)
Assuming the van’t Hoff factors in Table 12.9, calculate the mass of solute required to make each aqueous solution:
a. a sodium chloride solution containing \(1.50 \times 10^{2} \mathrm{\ g}\) of water that has a melting point of \(-1.0\ ^{\circ}\mathrm{C}\)
b. \(2.50 \times 10^{2} \mathrm{\ mL}\) of a magnesium sulfate solution that has an osmotic pressure of 3.82 atm at 298 K
c. an iron(III) chloride solution containing \(2.50 \times 10^{2} \mathrm{\ g}\) of water that has a boiling point of \(102\ ^{\circ}\mathrm{C}\)
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