Chapter 13, Problem 97
Calculate the vapor pressure at 25 °C of an aqueous solution that is 5.50% NaCl by mass. (Assume complete dissociation of the solute.)
Video transcript
Use the van't Hoff factors in Table 13.9 to calculate each colligative property: a. the melting point of a 0.100 m iron(III) chloride solution
A 1.2 m aqueous solution of an ionic compound with the formula MX2 has a boiling point of 101.4 °C. Calculate the van't Hoff factor (i) for MX2 at this concentration.
A 0.100 M ionic solution has an osmotic pressure of 8.3 atm at 25 °C. Calculate the van't Hoff factor (i) for this solution.
An aqueous CaCl2 solution has a vapor pressure of 81.6 mmHg at 50 °C. The vapor pressure of pure water at this temperature is 92.6 mmHg. What is the concentration of CaCl2 in mass percent? (Assume complete dissociation of the solute.)
The solubility of carbon tetrachloride (CCl4) in water at 25 °C is 1.2 g>L. The solubility of chloroform (CHCl3) at the same temperature is 10.1 g>L. Why is chloroform almost ten times more soluble in water than carbon tetrachloride?
Sodium hydroxide (NaOH) has a lattice energy of -887 kJ>mol and a heat of hydration of -932 kJ>mol. How much solution could be heated to boiling by the heat evolved by the dissolution of 25.0 g of NaOH? (For the solution, assume a heat capacity of 4.0 J>g # °C, an initial temperature of 25.0 °C, a boiling point of 100.0 °C, and a density of 1.05 g>mL.)