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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is the vapor pressure if the solution is ideal, and what is the composition of acetone and chloroform in the vapor phase?
A nonvolatile solute is dissolved in benzene so that it has a mole fraction of 0.147. What is the vapor pressure of the solution in torr? (P° of benzene is 26.5 torr) 『ー F2 F3 F4 F6 F7 FB F9 F10 F11 F12 @ %23 4. 7 8. S. D J K
Please don't provide handwritten solution
You have a sucrose solution of 28°Brix or 28 grams of sugar per 100 grams solution in a ripe grape ready to be made into wine. What is the molality of the solution? Look up the freezing point depression constant KF and figure out what the new freezing temperature would be for that solution.
A solution contains 5.10 moles of water, 1.10 moles of sucrose (C12H22O11), and 1.30 moles of glucose. Sucrose and glucose are nonvolatile. What is the mole fraction of water in this solution? Assuming an ideal mixture, what is the vapor pressure of this solution at 35°C, given that the vapor pressure of pure water at 35°C is 42.2 torr? torr
At a certain temperature the vapor pressure of pure acetyl bromide (CH,COB1) is measured to be 257. mmHg. Suppose a solution is prepared by mixing 136. g of acetyl bromide and 88.2 g of chloroform (CHCI,). Calculate the partial pressure of acetyl bromide vapor above this solution. Round your answer to 3 significant digits. Note for advanced students: you may assume the solution is ideal. I| mmHg Explanation Check 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Ac stv A
A solution contains 4.50 moles of water, 1.10 moles of sucrose (C12H22O11), and 1.60 moles of glucose. Sucrose and glucose are nonvolatile. Assuming an ideal mixture, what is the vapor pressure of this solution at 35°C, given that the vapor pressure of pure water at 35°C is 42.2 torr?
Raoult’s Law states: the vapor pressure (Psolution) of a solution is proportional to the mole fraction of the solvent present in the solution. Psolution = Xsolvent P°solvent Here, P°solvent is the vapor pressure of pure solvent. Calculate the vapor pressure of a solution which is prepared by dissolving 1.00 mole of glycerol (nonvolatile) and 4.00 moles of water at 25oC. Given: the vapor pressure of water is 25.0 torr at 25oC. Group of answer choices 5.00 torr 20.0 torr 6.25 torr 15.0 torr
The ideal, theoretical, van't Hoff factor for SrCl, is 3, meaning it dissociates into 3 particles when dissolved in solution. An experiment was conducted to accurately determine the van't Hoff factor. A solution composed of 26.17 g of SrCl, was dissolved in to 475.0 mL of water at 285.2 K. The osmotic pressure was determined to be 23.04 bar. What is the experimental van't Hoff factor?
At 25°C, the vapor in equilibrium with a solution containing carbon disulfide and acetonitrile has a total pressure of 247 torr and is 85.3 mole percent carbon disulfide. What is the mole fraction of carbon disulfide in the solution? At 25°C the vapor pressure of carbon disulfide is 361 torr. Assume that the solution and vapor exhibit ideal behavior.
A solution is made by dissolving 0.603 mol of nonelectrolyte solute in 885 g of benzene. Calculate the freezing point, T, and boiling point, T,, of the solution. Constants can be found in the table of colligative constants. T = 2.012 °C T = 78 %3D °C
A solution is made up of two volatile substances: liquid 1 for which P1*= 198 Torr and Liquid 2 for which P2* = 230 Torr. What is the molar mass of 8.824 kg of liquid 1, if the total vapor pressure is 215 Torr and there’s 2.00 total moles in solution.