Which of the following statements regarding the dilute solid-liquid solution is NOT correct? Suppose that the solution has n1 mol of liquid solvent, and n2 mol of solid solute. The molality of the solute is n2/m, where m is the mass of the solution. We usually use Raoult's law standard state for solvent, and Henry's law standard state for solute. The mole fraction of the solute is n2/(n1 + n2). The molarity (i.e., molar concentration) of the solute is n2/V , where V is the volume of the solution.

Which of the following statements regarding the dilute solid-liquid solution is NOT correct? Suppose that the solution has n1 mol of liquid solvent, and n2 mol of solid solute. The molality of the solute is n2/m, where m is the mass of the solution. We usually use Raoult's law standard state for solvent, and Henry's law standard state for solute. The mole fraction of the solute is n2/(n1 + n2). The molarity (i.e., molar concentration) of the solute is n2/V , where V is the volume of the solution.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 6RQ: In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal...

See similar textbooks

Similar questions

In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal liquid-liquid solution. lf a solution is ideal, what is true about Hsoln, T for the solution formation, and the interactive forces within the pure solute and pure solvent as compared to the interactive forces within the solution? Give an example of an ideal solution. Answer the previous two questions for solutions that exhibit either negative or positive deviations from Raoults law.
A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?
You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The freezing point of this solution is found to be 0.426C. Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.
The Henry's law constant for the solubility of radon in water at is 9.57106 M/mm Hg. Radon is present with other gases in a sample taken from an aquifer at 30C. Radon has a mole fraction of 2.7106 in the gaseous mixture. The gaseous mixture is shaken with water at a total pressure of 28 atm. Calculate the concentration of radon in the water. Express your answers using the following concentration units. (a) molarity (b) ppm (Assume that the water sample has a density of 1.00 g/mL.)
The solubility of ethylene (C2H4) in water at 20 C and 0.300 atm pressure is 1.27 104 molal. (a) Calculate the Henrys law constant for this gas in units of molal/torr. (b) How many grams of ethylene are dissolved in 1.00 kg water at 20 C if the pressure of the gas is 500 torr?
(a) If you dissolve 10.0 g (about one heaping teaspoonful) of sugar (sucrose, C12H22O11) in a cup of water (250. g), what are the mole fraction, molality, and weight percent of sugar? (b) Seawater has a sodium ion concentration of 1.08 104 ppm. If the sodium is present in the form of dissolved sodium chloride, what mass of NaCl is in each liter of seawater? Seawater is denser than pure water because of dissolved salts. Its density is 1.05 g/mL
A 2.77 M NaOH solution in water has a density of 1.109 g/mL. Express the concentration of this solution (a) mass percentage. (b) mole fraction. (c) molality.