Chemistry Atoms First2e2nd EditionOpenStax Publisher: OpenStax CollegeISBN: 9781947172647
Chemistry Atoms First2e
Solutions for Chemistry Atoms First2e
Problem 2E:
Which of the principal characteristics of solutions are evident 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 10C. 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 11.10. (a) How did the concentration of dissolved CO2 in the beverage change when...Problem 23E:
The Henrys law constant for CO2 is 3.4102 M/atm at 25 C. Assuming ideal solution behavior, what...Problem 24E:
The Henrys law constant for O2 is 1.3103 M/ atm at 25C. Assuming ideal solution behavior, what mass...Problem 25E:
Assuming ideal solution behavior, how many liters of HC1 gas, measured at 30.0 C and 745 torr, are...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 behavior illustrated in Figure 11.14? Figure...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:
Assuming ideal solution behavior what is the boiling point of a solution of 115.0 g of nonvolatile...Problem 44E:
Assuming ideal solution behavior, what is the boiling point of a solution of 9.04 g of I2 in 75.5 g...Problem 45E:
Assuming ideal solution behavior, what is the freezing temperature of a solution of 115.0 g of...Problem 46E:
Assuming ideal solution behavior, what is the freezing point of a solution of 9.04gofI2 in 75.5 g of...Problem 47E:
Assuming ideal solution behavior, what is the osmotic pressure of an aqueous solution of 1.64 g of...Problem 48E:
Assuming ideal solution behavior, what is osmotic pressure of a solution of bovine insulin (molar...Problem 49E:
Assuming ideal solution behavior, what is the molar mass of a solution of 5.00 g of a compound in...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.O-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 rnol of NaCI, 0.020 mol...Problem 56E:
How could you prepare a 3.08m aqueous solution of glycerin, C3H8O3? Assuming ideal solution...Problem 57E:
A sample of sulfur weighing 0.210 g was dissolved in 17.8 g of carbon disulfide, CS2(Kb=2.43C/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....Problem 61E:
The osmotic pressure of human blood is 7.6 atm at 37 C. What mass of glucose, C6H12O6 , is required...Problem 62E:
Assuming ideal solution behavior, what is the freezing point of a solution of dibromobenzene,...Problem 63E:
Assuming ideal solution behavior, what is the boiling point of a solution of NaC1 in water if the...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 - Electronic Structure And Periodic Properties Of ElementsChapter 4 - Chemical Bonding And Molecular GeometryChapter 5 - Advanced Theories Of BondingChapter 6 - Composition Of Substances And SolutionsChapter 7 - Stoichiometry Of Chemical ReactionsChapter 8 - GasesChapter 9 - ThermochemistryChapter 10 - Liquids And Solids
Chapter 11 - Solutions And ColloidsChapter 12 - ThermodynamicsChapter 13 - Fundamental Equilibrium ConceptsChapter 14 - Acid-base EquilibriaChapter 15 - Equilibria Of Other Reaction ClassesChapter 16 - ElectrochemistryChapter 17 - KineticsChapter 18 - Representative Metals, Metalloids, And NonmetalsChapter 19 - Transition Metals And Coordination ChemistryChapter 20 - Nuclear ChemistryChapter 21 - Organic Chemistry
Sample Solutions for this Textbook
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More Editions of This Book
Corresponding editions of this textbook are also available below:
CHEMISTRY: ATOMS FIRST
18th Edition
ISBN: 9781947172180
Chemistry: Atoms First
1st Edition
ISBN: 9781630182151
Chemistry: Atoms First
18th Edition
ISBN: 9781938168154
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