Solutions for Chemistry by OpenStax (2015-05-04)
Problem 2E:
Which of the principal characteristics of solutions can we see in the solutions of K2Cr2O7 shown in...Problem 3E:
When KNO3 is dissolved in water, the resulting solution is significantly colder than the water was...Problem 4E:
Give an example of each of the following types of solutions: (a) a gas in a liquid (b) a gas in a...Problem 5E:
Indicate the most important types of intermolecular attractions in each of the following solutions:...Problem 6E:
Predict whether each of the following substances would be more soluble in water (polar solvent) or...Problem 7E:
Heat is released when some solutions form; heat is absorbed when other solutions form. Provide a...Problem 8E:
Solutions of hydrogen in palladium may be formed by exposing Pd metal to H2 gas. The concentration...Problem 9E:
Explain why the ions Na+ and CI- are strongly solvated in water but not in hexane, a solvent...Problem 10E:
Explain why solutions of HBr in benzene (a nonpolar solvent) are nonconductive, while solutions in...Problem 11E:
Consider the solutions presented: (a) Which of the following sketches best represents the ions in a...Problem 12E:
Compare the processes that occur when methanol (CH3OH), hydrogen chloride (HCI), and sodium...Problem 13E:
What is the expected electrical conductivity of the following solutions? (a) NaOH(aq) (b) HCI(aq)...Problem 14E:
Why are most solid ionic compounds electrically nonconductive, whereas aqueous solutions of ionic...Problem 15E:
Indicate the most important type of intermolecular attraction responsible for solvation in each of...Problem 16E:
Suppose you are presented with a clear solution of sodium thiosulfate, Na2S2O3. How could you...Problem 17E:
Supersaturated solutions of most solids in water are prepared by cooling saturated solutions....Problem 18E:
Suggest an explanation for the observations that ethanol, C2H5OH, is completely miscible with water...Problem 19E:
Calculate the percent by mass of KBr in a saturated solution of KBr in water at 10 °C. See Figure...Problem 20E:
Which of the following gases is expected to be most soluble in water? Explain your reasoning. (a)...Problem 21E:
At 0 C and 1.00 atm, as much as 0.70 g of O2 can dissolve in 1 L of water. At 0 C and 4.00 atm, how...Problem 22E:
Refer to Figure 11.11. (a) How did the concentration of dissolved CO2 in the beverage change when...Problem 23E:
The Henry's law constant for CO2 is 3.4102 M/atm at 25 C. What pressure of carbon dioxide is needed...Problem 24E:
The Henry's law constant for O2 is 1.3103M /atm at 25 C. What mass of oxygen would be dissolved in a...Problem 25E:
How many liters of HCI gas, measured at 30.0 C and 745 torr, are required to prepare 1.25 L of a...Problem 26E:
Which is are part of the macroscopic domain of solutions and which is are part of the microscopic...Problem 27E:
What is the microscopic explanation for the macroscopic behaviour illustrated in Figure 11.15?Problem 28E:
Sketch a qualitative graph of the pressure versus time for water vapor above a sample of pure water...Problem 29E:
A solution of potassium nitrate, an electrolyte, and a solution of glycerin (C3H5(OH)3), a...Problem 30E:
What are the mole fractions of H3PO4 and water in a solution of 14.5 g of H3PO4 in 125 g of water?...Problem 31E:
What are the mole fractions of HNO3 and water in a concentrated solution of nitric acid (68.0% HNO3...Problem 32E:
Calculate the mole fraction of each solute and solvent: (a) 583 g of H2SO4 in 1.50 kg of water—the...Problem 33E:
Calculate the mole fraction of each solute and solvent: (a) 0.710 kg of sodium carbonate (washing...Problem 34E:
Calculate the mole fractions of methanol, CH3OH; ethanol, C2H5OH; and water in a solution that is...Problem 36E:
What is the molality of phosphoric acid, H3PO4, in a solution of 14.5 of H3PO4 in 125 g of water?...Problem 37E:
What is the molality of nitric acid in a concentrated solution of nitric acid (68.0% HNO3 by mass)?...Problem 38E:
Calculate the molality of each of the following solutions: (a) 583 g of H2SO4 in 1.50 kg of...Problem 39E:
Calculate the molality of each of the following solutions: (a) 0.710 kg of sodium carbonate (washing...Problem 40E:
The concentration of glucose, C6H12O6, in normal spinal fluid is 75mg100mg. What is the molality of...Problem 41E:
A 13.0% solution of K2CO3 by mass has a density of 1.09 g/cm3. Calculate the molality of the...Problem 42E:
Why does 1 mol of sodium chloride depress the freezing point of 1 kg of water almost twice as much...Problem 43E:
What is the boiling point of a solution of 115.0 g of sucrose, C12H22O11, in 350.0 g of water? (a)...Problem 44E:
What is the boiling point of a solution of 9.04 g of I2 in 75.5 g of benzene, assuming the I2 is...Problem 45E:
What is the freezing temperature of a solution of 115.0 g of sucrose, C12H22O11, in 350.0 g of...Problem 46E:
What is the freezing point of a solution of 9.04 g of I2 in 75.5 g of benzene? (a) Outline the steps...Problem 47E:
What is the osmotic pressure of an aqueous solution of 1.64 g Ca(NO3)2 of in water at 25 C? The...Problem 48E:
What is osmotic pressure of a solution of bovine insulin (molar mass, 5700 g mol-1) at 18 C if 100.0...Problem 49E:
What is the molar mass of a solution of 5.00 g of a compound in 25.00 g of carbon tetrachloride (bp...Problem 50E:
A sample of an organic compound (a nonelectrolyte) weighing 1.35 g lowered the freezing point of...Problem 51E:
A 1.0 m solution of HCI in benzene has a freezing point of 0.4 C. Is HCI an electrolyte in benzene?...Problem 52E:
A solution contains 5.00 g of urea, CO(NH2)2, a nonvolatile compound, dissolved in 0.100 kg of...Problem 53E:
A 12.0-g sample of a nonelectrolyte is dissolved in 80.0 g of water. The solution freezes at -1.94...Problem 54E:
Arrange the following solutions in order by their decreasing freezing points: 0.1 m Na3PO4, 0.1 m...Problem 55E:
Calculate the boiling point elevation of 0.100 kg of water containing 0.010 mol of NaCl, 0.020 mol...Problem 56E:
How could you prepare a 3.08 m aqueous solution of glycerin, C3H8O3? What is the freezing point of...Problem 57E:
A sample of sulfur weighing 0.210 g was dissolved in 17.8 g of carbon disulfide, CS2 ( Kb=2.43 C/m)....Problem 58E:
In a significant experiment performed many years ago, 5.6977 g of cadmium iodide in 44.69 g of water...Problem 59E:
Lysozyme is an enzyme that cleaves cell walls. A 0.100-L sample of a solution of lysozyme that...Problem 60E:
The osmotic pressure of a solution containing 7.0 g of insulin per liter is 23 torr at 25 C. What is...Problem 61E:
The osmotic pressure of human blood is 7.6 atm at 37 C. What mass of glucose, C6H12O6, is required...Problem 62E:
What is the freezing point of a solution of dibromobenzene, C6H4Br2, in 0.250 kg of benzene, if the...Problem 63E:
What is the boiling point of a solution of NaCI in water if the solution freezes at -0.93 C?Problem 64E:
The sugar fructose contains 40.0% C, 6.7% H, and 53.3% O by mass. A solution of 11.7 g of fructose...Problem 65E:
The vapor pressure of methanol, CH3OH, is 94 torr at 20 C. The vapor pressure of ethanol, C2H5OH, is...Problem 66E:
The triple point of air-free water is defined as 273.16 K. Why is it important that the water be...Problem 67E:
Meat can be classified as fresh (not frozen) even though it is stored at -1 C. Why wouldn't meat...Problem 68E:
An organic compound has a composition of 93.46% C and 6.54% H by mass. A solution of 0.090 g of this...Problem 69E:
A sample of HgCI2 weighing 9.41 g is dissolved in 32.75 g of ethanol, C2H5OH ( Kb=1.20 C/m). The...Problem 70E:
A salt is known to be an alkali metal fluoride. A quick approximate determination of freezing point...Problem 71E:
Identify the dispersed phase and the dispersion medium in each of the following colloidal systems:...Problem 72E:
Distinguish between dispersion methods and condensation methods for preparing colloidal systems.Problem 73E:
How do colloids differ from solutions with regard to dispersed particle size and homogeneity?Problem 74E:
Explain the cleansing action of soap.Browse All Chapters of This Textbook
Chapter 1 - Essential IdeasChapter 2 - Atoms, Molecules, And IonsChapter 3 - Composition Of Substances And SolutionsChapter 4 - Stoichiometry Of Chemical ReactionsChapter 5 - ThermochemistryChapter 6 - Electronic Structure And Periodic Properties Of ElementsChapter 7 - Chemical Bonding And Molecular GeometryChapter 8 - Advanced Theories Of Covalent BondingChapter 9 - GasesChapter 10 - Liquids And Solids
Chapter 11 - Solutions And ColloidsChapter 12 - KineticsChapter 13 - Fundamental Equilibrium ConceptsChapter 14 - Acid-base EquilibriaChapter 15 - Equilibria Of Other Reaction ClassesChapter 16 - ThermodynamicsChapter 17 - ElectrochemistryChapter 18 - Representative Metals, Metalloids, And NonmetalsChapter 19 - Transition Metals And Coordination ChemistryChapter 20 - Organic ChemistryChapter 21 - Nuclear Chemistry
Book Details
Chemistry is designed for the two-semester general chemistry course. For many students, this course provides the foundation to a career in chemistry, while for others, this may be their only college-level science course. As such, this textbook provides an important opportunity for students to learn the core concepts of chemistry and understand how those concepts apply to their lives and the world around them. The text has been developed to meet the scope and sequence of most general chemistry courses. At the same time, the book includes a number of innovative features designed to enhance student learning. A strength of Chemistry is that instructors can customize the book, adapting it to the approach that works best in their classroom. This is a full-color textbook.
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More Editions of This Book
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Chemistry (OER)
19th Edition
ISBN: 9781947172623
Chemistry (OER)
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ISBN: 9781947172616
WEBASSIGN FOR GENERAL CHEMISTRY
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ISBN: 9781337799867
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18th Edition
ISBN: 9781506696805
CHEMISTRY
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ISBN: 9781593995782
EBK CHEMISTRY
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ISBN: 9781947172098
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