EBK STUDENT SOLUTIONS MANUAL TO ACCOMPA
7th Edition
ISBN: 9781119360902
Author: HYSLOP
Publisher: YUZU
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Textbook Question
Chapter 12, Problem 47RQ
Heterogeneous Mixtures
What is the Tyndall effect?
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Chapter 12 Solutions
EBK STUDENT SOLUTIONS MANUAL TO ACCOMPA
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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- What gas law is applicable to the fractional distillation of ethanol-water mixture?arrow_forwardWhat is meant by Reversible sols.arrow_forwardAcrylonitrile and ethyl acetate have the same boiling point: 77.20C. Which statement explains the outcome you would expect if a mixture of these two substances were distilled? * The acrylonitrile would vaporize first and the ethyl acetate would be left behinc O The ethyl acetate would vaporize first and the acrylonitrile would be left behind Both substances would vaporize at the same time so distillation would not be h Ethyl acetate is a solid so distillation would involve allowing the acrylonitrile to evaporate. Which statement best explains why structural formulas are good for depicting polymers?arrow_forward
- 9. The phrase like dissolves like refers to the fact that… a. condensed phases can only dissolve other condensed phasesb. polar solvents dissolve non-polar solutes and vice versac. solvents can only dissolve solutes of similar molar mass d. gases can only dissolve other gases e.polar solvents dissolve polar solutes and non-polar solvents dissolve non-polar solutes 10. Which of the following elements can have an extended octet? (Choose all that applies.) a.Xeb.Cc.Fd.Pe.Brf. Ar 11.picarrow_forwardA 10.00 mL sample of ethanol is added to 250.0 mL of water in order to observe the freezing point depression of the water. Consider the possible errors in this experiment, and determine whether each would cause the freezing point of the water to increase, decrease, or remain the same compared with the expected results. It is discovered that the 10.00 g ethanol sample is actually 95% ethanol and 5% water. The ethanol sample is left out for several minutes before being added to the water, allowing a significant amount to evaporate. Instead of starting the experiment with room temperature water, the experiment is started with cold water. Some of the water is splashed out of the container before the ethanol is added. Some of the ethanol and water solution is spilled out of the container during temperature measurement.arrow_forwardMiscible liquids form a homogeneous mixture when added together. Is toluene miscible with water? With ethyl alcohol?arrow_forward
- Use the graph below to solve for the following questions. The graph show a mixtures of methanol and benzene. a. What phases are present in regions 1, 2, and 3? b. Describe how you would find the boiling point of a mixture that was 20% methanol, 80% benzene c. Identify the boiling point and composition of the azeotropic mixture. Explain the meaning of the azeotropic point of this phase diagram.arrow_forwardIf a 0.890 m aqueous solution freezes at -2.10 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i =arrow_forwardWhen a substance is dissolved in water the temperature increases. Which of these statements can be inferred from this information? 1. The enthalpy change for the system in this process is negative. A 2. The enthalpy change for the system in this process is positive. 3. The interactions between the species in solution are stronger than those in the separate solute and solvent. 4. The interactions between the species in solution are weaker than those in the separate solute and solvent. O1 and 4 O2 and 3 O2 and 4 O1 and 3arrow_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