Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Chapter 12, Problem 15RQ
Heat of solution
When a certain solid dissolves in water, the solution becomes cool. Is
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Chapter 12 Solutions
Chemistry: The Molecular Nature of Matter
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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- Simple acids such as formic acid, HCOOH, and acetic acid, CH3COOH, are very soluble in water; however, fatty acids such as stearic acid, CH3(CH2)16COOH, and palmitic acid, CH3(CH2)14COOH, are water-insoluble. Based on what you know about the solubility of alcohols, explain the solubility of these organic acids.arrow_forwardMaple syrup sap is 3% sugar (sucrose) and 97% water bymass. Maple syrup is produced by heating the sap toevaporate a certain amount of the water. (a) Describe what happens to the composition and boilingpoint of the solution as evaporation takes place. (b) A rule of thumb among maple syrup producers is thatthe finished syrup should boil about 4 C higher than theoriginal sap being boiled. Explain the chemistry behindthis guideline. (c) If the finished product boils 4 C higher than the originalsap, calculate the concentration of sugar in the finalproduct. Assume that sugar is the only solute and theoperation is done at 1 atm pressure.arrow_forwardFor each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70Carrow_forward
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