Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 12, Problem 56RQ
Helium gas can be used to displace other gases from a solvent by bubbling He through the solvent, a process called sparging, and leaving an atmosphere of helium above the solvent. At 760 torr of He, the concentration of He in water is
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
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...
Additional Science Textbook Solutions
Find more solutions based on key concepts
4. 38 Strontium has four naturally occurring isotopes, with mass numbers 84, 86, 87, arid 88.
a. Write the atom...
General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
Q3. Which change is a physical change?
a) Wood burning
b) Iron rusting
c) Dynamite exploding
d) Gasoline ev...
Chemistry: A Molecular Approach
Calculate the lattice energy of CaCl2 using a Born-Haber cycle and data from Appendices F and L and Table 7.5. ...
Chemistry & Chemical Reactivity
Determine [OH], [H+], and the pH of each of the following solutions. a. 1.0 M KCl b. 1.0 M KC2H3O2
Chemistry
The separation techniques for the separation of two colorless liquids should be predicted. Concept introduction...
Chemistry: Matter and Change
For the generic equilibrium HA(aq) ⇌ H + (aq) + A- (aq), which of these statements is true?
The equilibrium con...
Chemistry: The Central Science (14th Edition)
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- A 0.109 mol/kg aqueous solution of formic acid, HCOOH, freezes at −0.210 °C. Calculate the percent dissociation of formic acid.arrow_forwardThe vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?arrow_forwardThe freezing point of 0.109 m aqueous formic acid is 0.210C. Formic acid, HCHO2, is partially dissociated according to the equation HCHO2(aq)H+(aq)+CHO2(aq) Calculate the percentage of HCHO2 molecules that are dissociated, assuming the equation for the freezing-point depression holds for the total concentration of molecules and ions in the solution.arrow_forward
- The freezing point of a 0.21 m aqueous solution of H2SO4 is -0.796C. (a) What is i? (b) Is the solution made up primarily of (i) H2SO4 molecules only? (ii) H+ and HSO4- ions? (iii) 2H+ and 1SO42- ions?arrow_forwardThe freezing point of a 0.11 m solution of HNO2 is -0.20C. (a) What is i for the solution? (b) Is the solution made (i) of HNO2 molecules only? (ii) of H+ and NO2- only? (iii) of more HNO2 molecules than H+ ions? (iv) primarily of H+ and NO2- ions with some HNO2 molecules?arrow_forwardThe organic salt [(C4H9)4N][ClO4] consists of the ions (C4H9)4N+ and ClO4. The salt dissolves in chloroform. What mass (in grams) of the salt must have been dissolved if the boiling point of a solution of the salt in 25.0 g chloroform is 63.20 C? The normal boiling point of chloroform is 61.70 C and Kb = 3.63 C kg mol1. Assume that the salt dissociates completely into its ions in solution.arrow_forward
- 6-111 As noted in Section 6-8C, the amount of external pressure that must be applied to a more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane is known as the osmotic pressure The osmotic pressure obeys a law similar in form to the ideal gas law (discussed in Section 5-4), where Substituting for pressure and solving for osmotic pressures gives the following equation: RT MRT, where M is the concentration or molarity of the solution. (a) Determine the osmotic pressure at 25°C of a 0.0020 M sucrose (C12H22O11) solution. (b) Seawater contains 3.4 g of salts for every liter of solution. Assuming the solute consists entirely of NaCl (and complete dissociation of the NaCI salt), calculate the osmotic pressure of seawater at 25°C. (c) The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose (C6H12O6) will be isotonic with blood? (d) Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210. mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of lysozyme? (e) The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of the protein.arrow_forwardFreezing point depression is one means of determining the molar mass of a compound. The freezing point depression constant of benzene is 5.12 C/m. a. When a 0.503 g sample of the white crystalline dimer is dissolved in 10.0 g benzene, the freezing point of benzene is decreased by 0542 C. Verify that the molar mass of the dimer is 475 g/mol when determined by freezing point depression. Assume no dissociation of the dimer occurs. b. The correct molar mass of the dimer is 487 g/mol. Explain why the dissociation equilibrium causes the freezing point depression calculation to yield a lower molar mass for the dimer.arrow_forwardA forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar mass = 303.35 g/mol). She dissolves 1.22 0.01 g of the solid in 15.60 0.01 g benzene. The freezing point is lowered by 1.32 0.04C. a. What is the molar mass of the substance? Assuming that the percent uncertainty in the calculated molar mass is the same as the percent uncertainty in the temperature change, calculate the uncertainty in the molar mass. b. Could the chemist unequivocally state that the substance is cocaine? For example, is the uncertainty small enough to distinguish cocaine from codeine (C18H21NO3, molar mass = 299.36 g/mol)? c. Assuming that the absolute uncertainties in the measurements of temperature and mass remain unchanged, how could the chemist improve the precision of her results?arrow_forward
- In the 1986 Lake Nyos disaster (see the chapter introduction), an estimated 90 billion kilograms of CO2 was dissolved in the lake at the time. (a) What volume of gas is this at standard temperature and pressure? (b) Assuming that this dissolved gas was in equilibrium with the normal partial pressure of CO2 in the atmosphere (0.038%, or 0.29 torr), use the Henrys law constant for CO2 in water to estimate the volume of Lake Nyos.arrow_forwardThe freezing point of a 0.031-m solution of copper(II) sulfate in water is 0.075 C. (a) Calculate the vant Hoff factor, i, for this solution. (b) Would the vant Hoff factor be larger, smaller, or the same for a 0.050-m solution of this compound?arrow_forwardAn 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.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY