Chemistry: Atoms First
2nd Edition
ISBN: 9780073511184
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
expand_more
expand_more
format_list_bulleted
Question
Chapter 13, Problem 13.12QP
Interpretation Introduction
Interpretation:
The variation in solubility in water of given alcohol has to be explained.
Concept introduction:
Like dissolves like principle
Polar solutes dissolved in polar solvent and non polar solutes dissolved in non polar solvent. Example, Methanol and water both are polar molecule. Methanol dissolves in water but Hexane does not dissolve in water because hexane is non polar.
Compounds with same intermolecular force are soluble in one another because solute-solvent interactions are similar signification to the solute-solute interaction.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Chapter 13 Solutions
Chemistry: Atoms First
Ch. 13.2 - Determine for each solute whether the solubility...Ch. 13.2 - Predict whether iodine (I2) is more soluble in...Ch. 13.2 - Prob. 1PPBCh. 13.2 - Prob. 1PPCCh. 13.2 - Prob. 13.2.1SRCh. 13.2 - Prob. 13.2.2SRCh. 13.3 - Prob. 13.2WECh. 13.3 - Determine (a) the molality and (b) the percent by...Ch. 13.3 - Prob. 2PPBCh. 13.3 - Prob. 2PPC
Ch. 13.3 - Rubbing alcohol is a mixture of isopropyl alcohol...Ch. 13.3 - Prob. 3PPACh. 13.3 - Prob. 3PPBCh. 13.3 - Prob. 3PPCCh. 13.3 - Prob. 13.3.1SRCh. 13.3 - Prob. 13.3.2SRCh. 13.3 - Prob. 13.3.3SRCh. 13.3 - Prob. 13.3.4SRCh. 13.4 - Calculate the concentration of carbon dioxide in a...Ch. 13.4 - Calculate the concentration of CO2 in water at 25C...Ch. 13.4 - Prob. 4PPBCh. 13.4 - Prob. 4PPCCh. 13.4 - Prob. 13.4.1SRCh. 13.4 - Prob. 13.4.2SRCh. 13.5 - Prob. 13.5WECh. 13.5 - Calculate the vapor pressure of a solution made by...Ch. 13.5 - Calculate the mass of urea that should be...Ch. 13.5 - The diagrams [(i)(iv)] represent four closed...Ch. 13.5 - Ethylene glycol [CH2(OH)CH2(OH)] is a common...Ch. 13.5 - Prob. 6PPACh. 13.5 - What mass of ethylene glycol must be added to 1525...Ch. 13.5 - Prob. 6PPCCh. 13.5 - Prob. 13.7WECh. 13.5 - Prob. 7PPACh. 13.5 - Prob. 7PPBCh. 13.5 - Prob. 7PPCCh. 13.5 - Prob. 13.5.1SRCh. 13.5 - Prob. 13.5.2SRCh. 13.5 - Prob. 13.5.3SRCh. 13.5 - Prob. 13.5.4SRCh. 13.6 - Quinine was the first drug widely used to treat...Ch. 13.6 - Prob. 8PPACh. 13.6 - Prob. 8PPBCh. 13.6 - Prob. 8PPCCh. 13.6 - Prob. 13.9WECh. 13.6 - A solution made by dissolving 25 mg of insulin in...Ch. 13.6 - What mass of insulin must be dissolved in 50.0 mL...Ch. 13.6 - The first diagram represents one aqueous solution...Ch. 13.6 - Prob. 13.10WECh. 13.6 - An aqueous solution that is 0.0100 M in acetic...Ch. 13.6 - Prob. 10PPBCh. 13.6 - Prob. 10PPCCh. 13.6 - Prob. 13.6.1SRCh. 13.6 - Prob. 13.6.2SRCh. 13 - Prob. 13.1QPCh. 13 - Prob. 13.2QPCh. 13 - Prob. 13.3QPCh. 13 - Prob. 13.4QPCh. 13 - Prob. 13.5QPCh. 13 - Prob. 13.6QPCh. 13 - Explain why dissolving a solid almost always leads...Ch. 13 - Describe the factors that affect the solubility of...Ch. 13 - Prob. 13.9QPCh. 13 - Prob. 13.10QPCh. 13 - Arrange the following compounds in order of...Ch. 13 - Prob. 13.12QPCh. 13 - Prob. 13.13QPCh. 13 - Prob. 13.14QPCh. 13 - Prob. 13.15QPCh. 13 - Prob. 13.16QPCh. 13 - Prob. 13.17QPCh. 13 - Prob. 13.18QPCh. 13 - Prob. 13.19QPCh. 13 - Prob. 13.20QPCh. 13 - Prob. 13.21QPCh. 13 - Prob. 13.22QPCh. 13 - Prob. 13.23QPCh. 13 - Prob. 13.24QPCh. 13 - Fish breathe the dissolved air in water through...Ch. 13 - Prob. 13.26QPCh. 13 - Discuss the factors that influence the solubility...Ch. 13 - What is thermal pollution? Why is it harmful to...Ch. 13 - Prob. 13.29QPCh. 13 - A student is observing two beakers of water. One...Ch. 13 - A man bought a goldfish in a pet shop. Upon...Ch. 13 - A 3.20-g sample of a salt dissolves in 9.10 g of...Ch. 13 - The solubility of KNO3 is 155 g per 100 g of water...Ch. 13 - Prob. 13.34QPCh. 13 - The solubility of CO2 in water at 25C and 1 atm is...Ch. 13 - The solubility of N2 in blood at 37C and at a...Ch. 13 - The difference between water-soluble and...Ch. 13 - Predict whether each vitamin will be water soluble...Ch. 13 - Prob. 13.39QPCh. 13 - The first diagram represents an open system with...Ch. 13 - The diagrams represent an aqueous solution at two...Ch. 13 - Prob. 13.42QPCh. 13 - Prob. 13.43QPCh. 13 - Write the equation representing Raoults law, and...Ch. 13 - Prob. 13.45QPCh. 13 - Write the equations relating boiling-point...Ch. 13 - Prob. 13.47QPCh. 13 - Prob. 13.48QPCh. 13 - What is osmosis? What is a semipermeable membrane?Ch. 13 - Prob. 13.50QPCh. 13 - Prob. 13.51QPCh. 13 - Prob. 13.52QPCh. 13 - What are ion pairs? What effect does ion-pair...Ch. 13 - Prob. 13.54QPCh. 13 - Prob. 13.55QPCh. 13 - Prob. 13.56QPCh. 13 - Prob. 13.57QPCh. 13 - The vapor pressure of benzene is 100.0 mmHg at...Ch. 13 - The vapor pressures of ethanol (C2H5OH) and...Ch. 13 - The vapor pressure of ethanol (C2H5OH) at 20C is...Ch. 13 - Prob. 13.61QPCh. 13 - What arc the boiling point and freezing point of a...Ch. 13 - Prob. 13.63QPCh. 13 - How many liters of the antifreeze ethylene glycol...Ch. 13 - Prob. 13.65QPCh. 13 - Prob. 13.66QPCh. 13 - What are the normal freezing points and boiling...Ch. 13 - At 25C, the vapor pressure of pure water is 23.76...Ch. 13 - Both NaCl and CaCl2 are used to melt ice on roads...Ch. 13 - A 0.86 percent by mass solution of NaCl is called...Ch. 13 - Prob. 13.71QPCh. 13 - Calculate the osmotic pressure of a 0.0500 M MgSO4...Ch. 13 - The tallest trees known are the redwoods in...Ch. 13 - Calculate the difference in osmotic pressure (in...Ch. 13 - Prob. 13.75QPCh. 13 - Consider two aqueous solutions, one of sucrose...Ch. 13 - Arrange the following solutions in order of...Ch. 13 - Prob. 13.78QPCh. 13 - Indicate which compound in each of the following...Ch. 13 - Describe how you would use freezing-point...Ch. 13 - Prob. 13.81QPCh. 13 - The elemental analysis of an organic solid...Ch. 13 - A solution of 2.50 g of a compound having the...Ch. 13 - The molar mass of benzoic acid (C6H5COOH)...Ch. 13 - A solution containing 0.8330 g of a polymer of...Ch. 13 - Prob. 13.86QPCh. 13 - A solution of 6.S5 g of a carbohydrate m 100.0 g...Ch. 13 - A 0.036-M aqueous nitrous acid (HNO2) solution has...Ch. 13 - Prob. 13.89QPCh. 13 - Prob. 13.90QPCh. 13 - Prob. 13.91QPCh. 13 - Prob. 13.92QPCh. 13 - Prob. 13.93QPCh. 13 - Lysozyme is an enzyme that cleaves bacterial cell...Ch. 13 - The blood sugar (glucose) level of a diabetic...Ch. 13 - Trees in cold climates may be subjected to...Ch. 13 - Prob. 13.97QPCh. 13 - Two liquids A and B have vapor pressures of 76 and...Ch. 13 - Determine the van't Hoff factor of Na3PO4 in a...Ch. 13 - Prob. 13.100QPCh. 13 - Consider the three mercury manometers shown in the...Ch. 13 - A forensic chemist is given a white powder for...Ch. 13 - Prob. 13.103QPCh. 13 - A solution of 1.00 g of anhydrous aluminum...Ch. 13 - Explain why reverse osmosis is (theoretically)...Ch. 13 - What masses of sodium chloride, magnesium...Ch. 13 - The osmotic pressure of blood plasma is...Ch. 13 - Prob. 13.108QPCh. 13 - A protein has been isolated as a salt with the...Ch. 13 - A nonvolatile organic compound Z was used to make...Ch. 13 - Prob. 13.111QPCh. 13 - State which of the alcohols listed in Problem...Ch. 13 - Before a carbonated beverage bottle is sealed, it...Ch. 13 - Iodine (I2) is only sparingly soluble in water...Ch. 13 - (a) The root cells of plants contain a solution...Ch. 13 - Hemoglobin, the oxygen-transport protein, binds...Ch. 13 - Prob. 13.117QPCh. 13 - In the apparatus shown, what will happen if the...Ch. 13 - Concentrated hydrochloric acid is usually...Ch. 13 - Explain each of the following statements: (a) The...Ch. 13 - Prob. 13.121QPCh. 13 - A 1.32-g sample of a mixture of cyclohexane...Ch. 13 - How does each of the following affect the...Ch. 13 - A solution contains two volatile liquids A and B....Ch. 13 - Prob. 13.125QPCh. 13 - A mixture of ethanol and 1-propanol behaves...Ch. 13 - Ammonia (NH3) is very soluble in water, but...Ch. 13 - For ideal solutions, the volumes are additive....Ch. 13 - Acetic acid is a weak acid that ionizes in...Ch. 13 - Which vitamins (sec the given structures) do you...Ch. 13 - Calculate the percent by mass of the solute in...Ch. 13 - Acetic acid is a polar molecule and can form...Ch. 13 - Prob. 13.133QPCh. 13 - Fish in the Antarctic Ocean swim in water at about...Ch. 13 - Why are ice cubes (e.g., those you see in the...Ch. 13 - Prob. 13.136QPCh. 13 - Two beakers are placed in a closed container...Ch. 13 - (a) Derive the equation relating the molality (m)...Ch. 13 - At 27C, the vapor pressure of pure water is 23.76...Ch. 13 - A very long pipe is capped at one end with a...Ch. 13 - A mixture of liquids A and B exhibits ideal...Ch. 13 - Use Henrys law and the ideal gas equation to prove...Ch. 13 - Prob. 13.143QPCh. 13 - Prob. 13.144QPCh. 13 - The diagram here shows vapor pressure curves for...Ch. 13 - Valinomycin is an antibiotic. It functions by...Ch. 13 - Prob. 13.147QPCh. 13 - Prob. 13.148QPCh. 13 - Prob. 13.149QPCh. 13 - Explain why we cannot use osmotic pressure to...Ch. 13 - Which of the following processes is accompanied by...Ch. 13 - For each of the processes depicted here, determine...Ch. 13 - For each of the processes depicted here, determine...Ch. 13 - Prob. 13.4KSP
Knowledge Booster
Similar questions
- Predict the relative solubility of each compound in the two solvents, based on the intermolecular attractions. (a) Is potassium iodide more soluble in water or in methylene chloride (CH2Cl2)? (b) Is toluene (C6H5CH3) more soluble in benzene (C6H6) or in water? (c) Is ethylene glycol (C2H4(OH)2) more soluble in hexane (C6H14) or in ethanol (C2H5OH)?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_forward1. Vapor pressure: Arrange the following aqueous solutions in order of increasing vapor pressure at 25°C: 0.35 m C2H4(OH)2 (ethylene glycol, nonvolatile solute); 0.50 m sugar; 0.20 m KBr; and 0.20 m Na2SO4. C2H4(OH)2 < sugar < KBr < Na2SO4 Na2SO4 < sugar < KBr < C2H4(OH)2 sugar < C2H4(OH)2 < KBr < Na2SO4 KBr < sugar < Na2SO4 < C2H4(OH)2arrow_forward
- Predict the relative solubility of each compound in the two solvents, on the basis of intermolecular attractions. (a) Is NaCl more soluble in water or in carbon tetrachloride? (b) Is I2 more soluble in water or in toluene (C6H5CH3)? (c) Is ethanol (C2H5OH) more soluble in hexane or in water? (d) Is ethylene glycol (HOCH2CH2OH) more soluble in ethanol or in benzene (C6H6)?arrow_forwardTwo samples of sodium chloride solutions are brought to a boil on a stove. One of the solutions boils at 100.10C and the other at 100.15C. a Which of the solutions is more concentrated? b Which of the solutions would have a lower freezing point? c If you split the solution that boils at 100.1C into two portions, how would the boiling points of the samples compare? Which of the following statements do you agree with regarding the determination of your answer for part c? I. The question cannot be answered with certainty without knowing the volumes of each portion. II. Making the necessary assumption that the two samples have equal volumes, I was able to correctly answer the question. III. The volumes that the sample was split into are irrelevant when determining the correct answer.arrow_forwardPredict the relative solubility of each compound in the two solvents, on the basis of intermolecular attractions. (a) Is Br2 more soluble in water or in carbon tetrachloride? (b) Is CaCl2 more soluble in water or in benzene (C6H6)? (c) Is chloroform (CHCl3) more soluble in water or in diethyl ether [(C2H5)2O]? (d) Is ethylene glycol (HOCH2CH2OH) more soluble in water or in benzene (C6H6)?arrow_forward
- a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. Lattice Energy Hsoln CaCl2(s) 2247kj/mol 46kj/mol Cal2(s) 2059kj/mol 104kj/mol b. Based on your answers to part a, which ion, Cl or I, is more strongly attracted to water?arrow_forwardSamples of each of the substances listed below are dissolved in 125 g of water. Which of the solutions has the highest boiling point? (a) 3.0 g sucrose, C12H22O11 (b) 1.0 g glycerol, C3H3(OH)3 (c) 1.0 g propylene glycol, C3H6(OH)2 (d) 2.0 g glucose, C6H12(OH)2arrow_forwardIce Cream A rock salt (NaCl), ice, and water mixture isused to cool milk and cream to make homemade icecream. How many grams of rock salt must be added towater to lower the freezing point by 10.0°C?arrow_forward
- In a mountainous location, the boiling point of pure water is found to be 95C. How many grams of sodium chloride must be added to 1 kg of water to bring the boiling point back to 100C? Assume that i = 2.arrow_forwardStarch contains CC, CH, CO, and OH bonds. Hydrocarbons have only CC and CH bonds. Both starch and hydrocarbons can form colloidal dispersions in water. Which dispersion is classified as hydrophobic? Which is hydrophilic? Explain briefly.arrow_forwardA liquid solution consists of 0.30 mole fraction ethylene dibromide, C2H4Br2, and 0.70 mole fraction propylene dibromide, C2H4Br2. Both ethylene dibromide and propylene dibromide are volatile liquids; their vapor pressures at 85C are 173 mmHg and 127 mmHg, respectively. Assume that each compound follows Raoults law in the solution. Calculate the total vapor pressure of the solution.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
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 ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher: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: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher: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 Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
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: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning