Table 1. Experimentally Determined Changes in Freezing Point for Aqueous SolutionsSubstanceFreezing Point Tr (°C)AT = T°r-TTrial 1-0.1°CPure WaterPure WaterTrial 2T=-04°CAverageTr= -1-5 °CNaCI/Water SolutionEthylene Glycol/Water SolutionTr= 0.2 °C-3:2°C - 3 T2Tr- A°C-49°C - 6 TSMethanol/Water Solution(Amoles (6.02X10Table 2. Three Ratios for Specifying the Composition of Aqueous Solutionsgsolute/gsolventmole,olutegsolventmoleparticles/gsolventSubstance5.029/5M •085q /sg 595-121 102NaCI/Water Solution5.05X10" L 5g. 0147 na 0.85X16) 5g.0434 /59523/5m5MEthylene Glycol/Water SolutionMethanol/Water Solution1. Might any of the ratios you calculated for Table 2 above be useful for predicting how the freezing pointof a solution would differ from that of the pure liquid? Explain.

Given that - Ratio of NaCl/water = 5.02g/5 mL The freezing point of pure liquid, water is about…

Answered: 1. Might any of the ratios you…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter13: Solutions And Their Behavior

Section: Chapter Questions

Problem 106SCQ

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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?
The lattice enthalpy of sodium chloride, H for NaCl(s)Na+(g)+Cl(g) is 787 kJ/mol; the heat of solution in making up 1 M NaCl(aq) is +4.0 kJ/mol. From these data, obtain the sum of the heats of hydration of Na+ and Cl. That is obtain the sum of H values for Na+(g)Na+(aq)Cl(g)Cl(aq) If the heat of hydration of Cl is 338 kJ/mol, what is the heat of hydration of Na+?
When KNO3 is dissolved in water, the resulting solution is significantly colder than the water was originally. (a) Is the dissolution of KNO3 an endothermic or an exothermic process? (b) What conclusions can you draw about the intermolecular attractions involved in the process? (c) Is the resulting solution an ideal solution?
A solution contains 3.75 g of a nonvolatile pure hydrocarbon in 95 g acetone. The boiling points of pure acetone and the solution are 55.95C and 56.50C, respectively. The molal boiling-point constant of acetone is 1.71 C kg/mol. What is the molar mass of the hydrocarbon?
A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
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.

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1. Might any of the ratios you calculated for Table 2 above be useful for predicting how the freezing point of a solution would differ from that of the pure liquid? Explain.