Match the following aqueous solutions with the appropriate letter from the column on the right. | 1. 0.16 m Zn(NO3)2 | 2. 0.15 m CuCl2 A. Highest boiling point B. Second highest boiling point 3. 0.18 m Bal2 C. Third highest boiling point 4. 0.52 m Sucrose(nonelectrolyte) D. Lowest boiling point

18) A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van't Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? Kf = 1.86 °C m-1. A) +0.80°C B)-2.66°C C) -9.97°C D) -8.85°C E) +3.06°C 18)

when 7.94 g of xylene was added to 132.5 g of cyclohexane, the freezing point of the solution was -4.9 C. what is the molar mass of xylene?

At a certain temperature the vapor pressure of pure chloroform (CHCI,) is measured to be 203. torr. Suppose a solution is prepared by mixing 54.2 g of chloroform and 106. g of acetyl bromide (CH,COBR). Calculate the partial pressure of chloroform vapor above this solution. Round your answer to 3 significant digits.

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

The increase in the boiling point of a solution is given by the equation: ДТ — Кті Where: AT = boiling point elevation K = boiling point elevation constant m = molality of the solution i van't Hoff factor NOTE: Write AT as dT (with no spaces) for the answers below. In order to solve for the van't Hoff factor, i, you must multiply both sides of the equation by the same expression: ДТ х AT x= Kmi x The resulting equation is:

7.152g of an unknown solute was dissolved in 0.049883 kg of pure water. This solution has a boiling point of 103.4oC. The Van't Hoff factor of the unknown solute is 3. What is the Molality of the unknown? What is the Molecular weight of the unknown?

True or False1.) The phase diagram of a pure solvent shows a lower freezing point compared to solutions2.) The process of freezing only lowers the kinetic energy of solute particles in a solution3.) Ionic solutes have higher van't hoff factor compared to non ionic solutes4.) The formation of intermolecular forces of attraction requires complete dissolution

A 1.00 molal aqueous solution of trichloroacetic acid (CCl3COOH) is heated to its boiling point. The solution has the boiling point of 100.18°C. Determine the van’t Hoff factor for trichloroacetic acid. (Kb for water = 0.512 K kg mol-1)

A solution is made by mixing 40.0 mL of ethanol, C, H,O, and 60.0 mL of water. Assuming ideal behavior, what is the vapor pressure of the solution at 20 °C? The relevant values at 20 °C are included in the table. Liquid Density (g/mL) Vapor Pressure, P' (Torr) ethanol 0.789 43.9 water 0.998 17.5 vapor pressure: 14.7770050376 Torr Incorrect