Which of the following is the reason for why water is good at dissolving ionic compounds? Water molecules can form hydrogen bonds with most ions, and since these interactions are stronger than those usually found in the lattices of ionic compounds, dissolution of these lattices tends to be favored O As an ionic compound itself, water should be able to dissolve ionic compounds as "like dissolves like" O Water molecules possess both negatively and positively charged regions, which interact with positive ions (cations) and negative ions (anions) respectively, coating ions and thus hindering their ability to form a lattice O The combination of water and ions usually forms more entropically favored lattices than just those of pure water and pure ionic compounds O Water molecules can covalently bind to each other to form "flickering clusters" which envelop ions in a hydration layer that isolate them from each other, thus making it hard for them to form a lattice and easy for lattices to dissolve

Which of the following is the reason for why water is good at dissolving ionic compounds? Water molecules can form hydrogen bonds with most ions, and since these interactions are stronger than those usually found in the lattices of ionic compounds, dissolution of these lattices tends to be favored O As an ionic compound itself, water should be able to dissolve ionic compounds as "like dissolves like" O Water molecules possess both negatively and positively charged regions, which interact with positive ions (cations) and negative ions (anions) respectively, coating ions and thus hindering their ability to form a lattice O The combination of water and ions usually forms more entropically favored lattices than just those of pure water and pure ionic compounds O Water molecules can covalently bind to each other to form "flickering clusters" which envelop ions in a hydration layer that isolate them from each other, thus making it hard for them to form a lattice and easy for lattices to dissolve

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 81QAP: Beaker A has 1.00 mol of chloroform, CHCl3, at 27C. Beaker B has 1.00 mol of carbon tetrachloride,...

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Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?
The freezing point of 0.10 M KHSO3 is -0.38C. Which of the following equations best represents what happens when KHSO3 dissolves in water? (a) KHSO3(s)KHSO3(aq) (b) KHSO3(s) K+(aq)+HSO3(aq) (c) KHSO3(s) K+(aq)+SO32(aq)+ H+(aq)
An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound gives mass percents of 31.57% C and 5.30% H. The molar mass is determined by measuring the freezing-point depression of an aqueous solution. A freezing point of 5.20C is recorded for a solution made by dissolving 10.56 g of the compound in 25.0 g water. Determine the empirical formula, molar mass, and molecular formula of the compound. Assume that the compound is a nonelectrolyte.
Beaker A has 1.00 mol of chloroform, CHCl3, at 27C. Beaker B has 1.00 mol of carbon tetrachloride, CCl4, also at 27C. Equal masses of a nonvolatile, nonreactive solute are added to both beakers. In answering the questions below, the following data may be helpful. Write , =, or more information needed in the blanks provided. (a) Vapor pressure of solvent over beaker B vapor pressure of solvent over beaker A. (b) Boiling point of solution in beaker A boiling point of solution in beaker B. (c) Vapor pressure of pure CHCl3 vapor pressure of solvent over beaker A. (d) Vapor pressure lowering of solvent in beaker A vapor pressure lowering of solvent in beaker B. (e) Mole fraction of solute in beaker A mole fraction of solute in beaker B.
Calculate the percent by mass of solute in each of the following solutions. 5.00 g of calcium chloride dissolved in 95.0 g of water 1.00 g of calcium chloride dissolved in 19.0 g of water 15.0 g of calcium chloride dissolved in 285 g of water 2.00 mg of calcium chloride dissolved in 0.0380 g of water