EBK CHEMISTRY: THE MOLECULAR NATURE OF
7th Edition
ISBN: 9781119513216
Author: HYSLOP
Publisher: JOHN WILEY+SONS INC.
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Textbook Question
Chapter 12, Problem 2RQ
Intermolecular Forces and the Formation of Solutions
When substances form liquid solutions, what two factors are involved in determining the solubility of the solute in the solvent?
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Chapter 12 Solutions
EBK CHEMISTRY: THE MOLECULAR NATURE OF
Ch. 12 - Which substances will be soluble in water? (a)...Ch. 12 - Which substances will be soluble in nonpolar...Ch. 12 - Draw an enthalpy diagram for the endothermic...Ch. 12 - When potassium hydroxide is dissolved in water,...Ch. 12 - Prob. 5PECh. 12 - When sodium hydroxide is dissolved in water, the...Ch. 12 - At 25C and standard pressure, a hydrogen sulfide...Ch. 12 - How many grams of nitrogen and oxygen are...Ch. 12 - What volume of water at 20.0C(d=0.9982gmL-1) is...Ch. 12 - Prob. 10PE
Ch. 12 - Prob. 11PECh. 12 - Water freezes at a lower temperature when it...Ch. 12 - Prob. 13PECh. 12 - Prob. 14PECh. 12 - Prob. 15PECh. 12 - Prob. 16PECh. 12 - Dibutyl phthalate, C16H22O4 (molar mass...Ch. 12 - Prob. 18PECh. 12 - At , the vapor pressure of cyclohexane, a nonpolar...Ch. 12 - Using the information from Practice Exercise...Ch. 12 - In making candy, a certain recipe calls for...Ch. 12 - How many grams of glucose (molar mass = 180.9 g...Ch. 12 - A solution made by dissolving 3.46 g of an unknown...Ch. 12 - Prob. 24PECh. 12 - What is the osmotic pressure, in mm Hg and mm H2O,...Ch. 12 - What is the osmotic pressure in torr of a 0.0115 M...Ch. 12 - Estimate the molecular mass of a protein when...Ch. 12 - Prob. 28PECh. 12 - Calculate the freezing point of aqueous 0.237mLiCl...Ch. 12 - Determine the freezing point of aqueous solutions...Ch. 12 - Prob. 31PECh. 12 - Prob. 32PECh. 12 - Intermolecular Forces and the Formation of...Ch. 12 - Intermolecular Forces and the Formation of...Ch. 12 - Intermolecular Forces and the Formation of...Ch. 12 - Intermolecular Forces and the Formation of...Ch. 12 - Intermolecular Forces and the Formation of...Ch. 12 - Intermolecular Forces and the Formation of...Ch. 12 - Prob. 7RQCh. 12 - Intermolecular Forces and the Formation of...Ch. 12 - Heats of Solution
12.9 The value of for a soluble...Ch. 12 - Heats of Solution Referring to Question 12.9,...Ch. 12 - Heats of Solution Which would be expected to have...Ch. 12 - Heats of Solution
12.12. Suggest a reason why the...Ch. 12 - Prob. 13RQCh. 12 - Prob. 14RQCh. 12 - Heat of solution When a certain solid dissolves in...Ch. 12 - Heat of solution
12.16 If the value of for the...Ch. 12 - Prob. 17RQCh. 12 - Solubility as a Function of Temperature
12.18 If a...Ch. 12 - Solubility as a Function of Temperature Anglers...Ch. 12 - Henry's Law
12.20 What is Henry’s law?
Ch. 12 - Henry's Law
12.21 Mountain streams often contain...Ch. 12 - Henry's Law Why is ammonia so much more soluble in...Ch. 12 - Prob. 23RQCh. 12 - Prob. 24RQCh. 12 - Prob. 25RQCh. 12 - Prob. 26RQCh. 12 - Concentration Units Suppose a 1.0 m solution of a...Ch. 12 - Colligative Properties What specific fact about a...Ch. 12 - Colligative Properties
12.29. What is Raoult’s...Ch. 12 - Colligative Properties Why does a nonvolatile...Ch. 12 - Prob. 31RQCh. 12 - Prob. 32RQCh. 12 - Prob. 33RQCh. 12 - Prob. 34RQCh. 12 - Prob. 35RQCh. 12 - Prob. 36RQCh. 12 - Prob. 37RQCh. 12 - Prob. 38RQCh. 12 - Colligative Properties
12.39 When a solid is...Ch. 12 - Colligative Properties
12.40 What is the...Ch. 12 - Prob. 41RQCh. 12 - Colligative Properties What is the vant Hoff...Ch. 12 - Prob. 43RQCh. 12 - Prob. 44RQCh. 12 - Prob. 45RQCh. 12 - Prob. 46RQCh. 12 - Heterogeneous Mixtures What is the Tyndall effect?Ch. 12 - Heterogeneous Mixtures
12.48 What is a micelle,...Ch. 12 - Heat of Solution For an ionic compound dissolving...Ch. 12 - Heat of solution
12.50 Consider the formation of a...Ch. 12 - Henry's Law The solubility of methane, the chief...Ch. 12 - Henry's Law If the solubility of a gas in water is...Ch. 12 - At 740 torr and 20.0C, nitrogen has a solubility...Ch. 12 - Hydrogen gas has a solubility in water of...Ch. 12 - 12.55. If 100.0 mL of water is shaken with oxygen...Ch. 12 - 12.56 Helium gas can be used to displace other...Ch. 12 - Concentration Units Muriatic acid is the...Ch. 12 - Prob. 58RQCh. 12 - What mass of a 0.853 molal solution of iron(III)...Ch. 12 - In order to conduct three experiments that...Ch. 12 - Prob. 61RQCh. 12 - A solution of acetic acid, CH3COOH, has a...Ch. 12 - Prob. 63RQCh. 12 - Botulinum toxin is one of the most acutely toxic...Ch. 12 - A solution of fructose, C6H12O6, a sugar found in...Ch. 12 - Prob. 66RQCh. 12 - Prob. 67RQCh. 12 - Prob. 68RQCh. 12 - Prob. 69RQCh. 12 - An aqueous solution of isopropyl alcohol, C3H8O,...Ch. 12 - Sodium nitrate, NaNO3, is sometimes added to...Ch. 12 - In an aqueous solution of sulfuric acid, the...Ch. 12 - Colligative Properties At 25C, the vapor pressure...Ch. 12 - Colligative Properties The vapor pressure of water...Ch. 12 - 12.75 At the vapor pressures of benzene and...Ch. 12 - Pentane (C5HI2)andheptane(C7HI6) are two...Ch. 12 - *12.77 Benzene and toluene help achieve good...Ch. 12 - The vapor pressure of pure methanol, CH3OH, at 33C...Ch. 12 - A solution containing 8.3 g of a nonvolatile,...Ch. 12 - At 21.0C, a solution of 18.26 g of a nonvolatile,...Ch. 12 - 12.81 How many grams of sucrose are needed to...Ch. 12 - Prob. 82RQCh. 12 - A solution of 12.00 g of an unknown...Ch. 12 - 12.84 A solution of 14 g of a nonvolatile,...Ch. 12 - What are the molecular mass and molecular formula...Ch. 12 - Benzene reacts with hot concentrated nitric acid...Ch. 12 - 12.87 (a) Show that the following equation is...Ch. 12 - A saturated solution is made by dissolving 0.400 g...Ch. 12 - Prob. 89RQCh. 12 - How many grams of A1C13 would have to be dissolved...Ch. 12 - 12.91 What is the osmotic pressure, in torr, of a ...Ch. 12 - Below are the concentrations of the most abundant...Ch. 12 - 12.93 What is the expected freezing point of a...Ch. 12 - Prob. 94RQCh. 12 - 12.95 The van’t Hoff factor for the solute in is...Ch. 12 - 12.96 What is the expected van’t Hoff factor for ...Ch. 12 - Prob. 97RQCh. 12 - *12.98 The “bends” is a medical emergency caused...Ch. 12 - In order for mosquitos to survive the cold winter,...Ch. 12 - The vapor pressure of a mixture of 0.400 kg of...Ch. 12 - Ethylene glycol, C2H6O2, is used in many...Ch. 12 - What is the osmotic pressure in torr of a 0.010 M...Ch. 12 - The osmotic pressure of a dilute solution of a...Ch. 12 - Prob. 104RQCh. 12 - Consider an aqueous 1.00 m solution of Na3PO4,a...Ch. 12 - A 2.50 g sample of aluminum chloride and sodium...Ch. 12 - Prob. 107RQCh. 12 - A sample containing only iron(II) nitrate and...Ch. 12 - Prob. 109RQCh. 12 - Prob. 110RQCh. 12 - How many mL of 0.223MK2Cr2O7 are needed to...Ch. 12 - Prob. 112RQCh. 12 - A certain organic substance is soluble in solvent...Ch. 12 - Prob. 114RQCh. 12 - Prob. 115RQCh. 12 - Having had some laboratory experience by now,...Ch. 12 - 12.117 This chapter focused on the physical...Ch. 12 - 12.118 Using the principles developed in this...Ch. 12 - Prob. 119RQCh. 12 - Prob. 120RQCh. 12 - Prob. 121RQCh. 12 - Consider a solution that has the maximum amount of...Ch. 12 - 12.123 When a 10.0 molar solution of sodium...
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- Temperature influences solubility. Does temperature have the same effect on all substances? Justify your answer. (Hint: Consider Le Chateliers principle.)arrow_forward. Why does the amount of excess solid solute present in a solution not affect the amount of solute that ultimately dissolves in a given amount of solvent?arrow_forwardHow are the boiling point and freezing point of water affected by the addition of solute?arrow_forward
- A solution is defined as a homogeneous mixture. Is a small sample of air a solution? Is the atmosphere a solution?arrow_forwardCalculate the concentration in (w/v) of the following solutions: a. 150.mL of solution contains 7.50g of dissolved solid Na2SO4. b. 150.mL of solution contains 7.50g of any dissolved solid solute. c. 350.mL of solution contains 30.7g of dissolved solid solute.arrow_forwardClassify each of the following solutions as saturated, unsaturated, or supersaturated based on the following observations made after adding a small piece of solid solute to the solution. a. The added solute rapidly dissolves. b. The added solute falls to the bottom of the container where it remains without any decrease in size. c. The added solute falls to the bottom of the container where it decreases in size for several hours and thereafter its size remains constant. d. The added solute causes the production of a large amount of solid white crystals.arrow_forward
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- 12.111 You have three white solids. What experiment could you carry out to rank them in order of increasing solubility?arrow_forwardEvery pure substance has a definite and fixed set of physical and chemical properties. A solution is prepared by dissolving one pure substance in another. Is it reasonable to expect that the solution will also have a definite and fixed set of properties that are different from the properties of either component? Explain your answer.arrow_forward
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY