Chemistry

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
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Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
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ISBN: 9780321910417
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Chapter: Problem: 27E

Chemistry: The Central Science 13
Saturated Solutions; Factors Affecting Solubility (Sections) Consider water and glycerol, . (a) Would you expect them to be miscible in all proportions? Explain, (b) List the intermolecular attractions that occur between a water molecule and a glycerol molecule.

Chapter: Problem: 28E

Chemistry: The Central Science 13
Saturated Solutions; Factors Affecting Solubility (Sections) Oil and water are immiscible. Which is the most likely reason? (a) Oil molecules are denser than water, (b) Oil molecules are composed mostly of carbon and hydrogen, (c) Oil molecules have higher molar masses than water, (d) Oil molecules h

Chapter: Problem: 29E

Chemistry: The Central Science 13
Problem 29E Saturated Solutions; Factors Affecting Solubility (Sections) Common laboratory solvents include acetone (CH3COCH3), methanol (CH3OH), toluene (C6H5CH3), and water. Which of these is the best solvent for nonpolar solutes?

Chapter: Problem: 30E

Chemistry: The Central Science 13
Would you expect alanine (an amino acid) to be more soluble in water or in hexane? Explain.

Chapter: Problem: 31E

Chemistry: The Central Science 13
(a) Would you expect stearic acid, \(\mathrm{CH}_{3}\left(\mathrm{CH}_{2}\right)_{16} \mathrm{COOH}\), to be more soluble in water or in carbon tetrachloride? Explain. (b) Which would you expect to be more soluble in water, cyclohexane or dioxane? Explain. Equation Transcription:

Chapter: Problem: 32E

Chemistry: The Central Science 13
Ibuprofen, widely used as a pain reliever, has a limited solubility in water, less than 1 mg>mL. Which part of the molecules structure (gray, white, red) contributes to its water solubility? Which part of the molecule (gray, white, red) contributes to its water insolubility?

Chapter: Problem: 33E

Chemistry: The Central Science 13
Saturated Solutions; Factors Affecting Solubility (Sections) Which of the following in each pair is likely to be more soluble in hexane, : (a) , (b) benzene or glycerol, , (c) octanoic acid, , or acetic acid, ? Explain your answer in each case.

Chapter: Problem: 34E

Chemistry: The Central Science 13
Writing Condensed Structural Formulas Write the condensed structural formula for 3-ethyl-2-methylpentane How many hydrogen atoms are in 2.2-dimethylhexane? (a) 6. (b) 8. (c) 16. (d) 18. (e) 20.

Chapter: Problem: 35E

Chemistry: The Central Science 13
Positron emission from , occurs with release of per mole of 11C. What is the mass change per mole of 11C in this nuclear reaction? The masses of are 11.009305 and 11.011434 arnu, respectively.

Chapter: Problem: 36E

Chemistry: The Central Science 13
Drawing Isomers Draw all the structural and geometric isomers of pentene. . It has an unbranched hydrocarbon chain. Which compound does not exist? (a) 1,2.3.4.5.6.7-octaheptaene. (b) cis-2-butane. (c) trans-3-hexene. (d) 1-propene. (e)cis-4-decene.

Chapter: Problem: 37E

Chemistry: The Central Science 13
Drawing Isomers How many straight-chain isomers are there of hexene. ?

Chapter: Problem: 38E

Chemistry: The Central Science 13
The partial pressure of \(\mathrm{O}_{2}\) in air at sea level is 0.21 atm. Using the data in Table 13.1, together with Henrys law, calculate the molar concentration of \(\mathrm{O}_{2}\) in the surface water of a mountain lake saturated with air at \(20\ ^{\circ} \mathrm{C}\) and an atmospheric pres

Chapter: Problem: 39E

Chemistry: The Central Science 13
Draw the condensed Structural formula for 4-methyl-2-pentyne.

Chapter: Problem: 40E

Chemistry: The Central Science 13
What product is formed from the hydrogenation of 2-methylpropene? (a) propane, (b) butane, (c) 2-methylbutane. (d) 2-methylpropane, (e) 2-methylpropyne

Chapter: Problem: 41E

Chemistry: The Central Science 13
Problem 41E Concentrations of Solutions (Section) A solution is made containing 14.6 g of CH30H in 184 g of H2O. Calculate (a) the mole fraction of CH3OH, (b) the mass percent of CH3OH, (c) the molality of CH3OH.

Chapter: Problem: 42E

Chemistry: The Central Science 13
Concentrations of Solutions (Section) A solution is made containing 20.8 g of phenol in 425 g of ethanol . Calculate (a) the mole fraction of phenol, (b) the mass percent of phenol, (c) the molality of phenol.

Chapter: Problem: 43E

Chemistry: The Central Science 13
Problem 43E Concentrations of Solutions (Section) Calculate the molarity of the following aqueous solutions: (a) 0.540 g of Mg(N03)2 in 250.0 ml of solution, (b) 22.4 g of LiCIO4.3 H2O in 125 mL of solution, (c) 25.0 ml of 3.50 M HNO3 diluted to 0.250 L.

Chapter: Problem: 44E

Chemistry: The Central Science 13
Problem 44E Concentrations of Solutions (Section) What is the molarity of each of the following solutions: (a) 15.0 g of AI2(SO4)3 in 0.250 ml solution, (b) 5.25 g of Mn(NO3)2*2 H20 in 175 ml of solution (c) 35.0 ml of 9.00 MH2SO4 diluted to 0.500 L?

Chapter: Problem: 45E

Chemistry: The Central Science 13
Problem 45E Concentrations of Solutions (Section) Calculate the molality of each of the following solutions: (a) 8.66 g of benzene (C6H6) dissolved in 23.6 g of carbon tetrachloride (CCI4), (b) 4.80 g of NaCI dissolved in 0.350 L of water.

Chapter: Problem: 46E

Chemistry: The Central Science 13
Problem 46E Concentrations of Solutions (Section) (a) What is the molality of a solution formed by dissolving 1.12 mol of KCI in 16.0 mol of water? (b) How many grams of sulfur (S8) must be dissolved in 100.0 g of naphthalene (C10H8) to make a 0.12 m solution?

Chapter: Problem: 47E

Chemistry: The Central Science 13
Concentrations of Solutions (Section) A sulfuric acid solution containing 571.6 g of per liter of solution has a density of . Calculate (a) the mass percentage, (b) the mole fraction, (c) the molality, (d) the molarity of in this solution.

Chapter: Problem: 48E

Chemistry: The Central Science 13
Concentrations of Solutions (Section) Ascorbic acid (vitamin C, ) is a water-soluble vitamin. A solution containing 80.5 g of ascorbic acid dissolved in 210 g of water has a density of 1.22 g/mL at 55 C. Calculate (a) the mass percentage, (b) the mole fraction, (c) the molality, (d) the molarity of

Chapter: Problem: 49E

Chemistry: The Central Science 13
Problem 49E Concentrations of Solutions (Section) The density of acetonitrile (CH3CN) is 0.786 g/mL and the density of methanol (CH3OH) is 0.791 g/mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (a) What is the mole fraction of methanol in the solution? (b) What is the

Chapter: Problem: 50E

Chemistry: The Central Science 13
Problem 50E Concentrations of Solutions (Section) The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/ml. A solution is made by dissolving 8.10 g of thiophene in 250.0 ml of toluene, (a) Calculate the mole fraction of thiophene in the solution, (b) Calcula

Chapter: Problem: 51E

Chemistry: The Central Science 13
Concentrations of Solutions (Section) Calculate the number of moles of solute present in each of the following aqueous solutions: (a) 600 ml of 0.250 M , (b) 86.4 g of 0.180 m , (c) 124.0 g of a solution that is 6.45% glucose by mass.

Chapter: Problem: 52E

Chemistry: The Central Science 13
Problem 52E Concentrations of Solutions (Section) Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 MHNO3(ag), (b) 50.0 mg of an aqueous solution that is 1.50 m NaCI, (c) 75.0 g of an aqueous solution that is 1.50% sucrose (C12H22O11) by mass.

Chapter: Problem: 53E

Chemistry: The Central Science 13
Problem 53E Concentrations of Solutions (Section) Describe how you would prepare each of the following aqueous solutions, starting with solid KBr: (a) 0.75 L of 1.5 x 10-2 M KBr, (b) 125 g of 0.180 m KBr, (c) 1.85 L of a solution that is 12.0% KBr by mass (the density of the solution is 1.10 g/mL

Chapter: Problem: 54E

Chemistry: The Central Science 13
Problem 54E Concentrations of Solutions (Section) Describe how you would prepare each of the following aqueous solutions: (a) 1.50 L of 0.110 M(NH4)2SO4 solution, starting with solid (NH4)2SO4; (b) 225 g of a solution that is 0.65 m in Na2CO3, starting with the solid solute; (c) 1.20 L of a solut

Chapter: Problem: 55E

Chemistry: The Central Science 13
Problem 55E Commercial aqueous nitric acid has a density of 1.42 g/mL and is 16 M. Calculate the percent HNaO3 by mass in the solution.

Chapter: Problem: 56E

Chemistry: The Central Science 13
Commercial concentrated aqueous ammonia is 28% by mass and has a density of 0.90 g/mL. What is the molarity of this solution?

Chapter: Problem: 57E

Chemistry: The Central Science 13
Problem 57E Concentrations of Solutions (Section) Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of 80.0% Cu and 20.0% Zn by mass has a density of 8750 kg/m3. (a) What is the molality of Zn in the solid solution? (b) What i

Chapter: Problem: 58E

Chemistry: The Central Science 13
Caffeine \(\left(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{~N}_{4} \mathrm{O}_{2}\right)\) is a stimulant found in coffee and tea. If a solution of caffeine in the solvent chloroform \(\left(\mathrm{CHCl}_{3}\right)\) has a concentration of 0.0500 m, calculate (a) the percentage of caffeine by mass, (b)

Chapter: Problem: 60E

Chemistry: The Central Science 13
Problem 60E Concentrations of Solutions (Section) Breathing air that contains 4.0% by volume CO2 over time causes rapid breathing, throbbing headache, and nausea, among other symptoms. What is the concentration of CO2 in such air in terms of (a) mol percentage, (b) molarity, assuming 1 atm pressu

Chapter: Problem: 59E

Chemistry: The Central Science 13
Problem 59E Concentrations of Solutions (Section) During a person's typical breathing cycle, the CO2 concentration in the expired air rises to a peak of 4.6% by volume, (a) Calculate the partial pressure of the CO2 in the expired air at its peak, assuming 1 atm pressure and a body temperature of

Chapter: Problem: 61E

Chemistry: The Central Science 13
Problem 61E Colligative Properties (Section) You make a solution of a nonvolatile solute with a liquid solvent. Indicate whether each of the following statements is true or false, (a) The freezing point of the solution is higher than that of the pure solvent, (b) The freezing point of the solutio

Chapter: Problem: 62E

Chemistry: The Central Science 13
Problem 62E You make a solution of a nonvolatile solute with a liquid solvent. Indicate if each of the following statements is true or false, (a) The freezing point of the solution is unchanged by addition of the solvent, (b) The solid that forms as the solution freezes is nearly pure solute, (c)

Chapter: Problem: 63E

Chemistry: The Central Science 13
Problem 63E Colligative Properties (Section) Consider two solutions, one formed by adding 10 g of glucose (C6H12O6) to 1 L of water and the other formed by adding 10 g of sucrose (C12H22O11) to 1 L of water. Calculate the vapour pressure for each solution at 20 C; the vapor pressure of pure wat

Chapter: Problem: 64E

Chemistry: The Central Science 13
Problem 64E Colligative Properties (Section) (a) What is an ideal solution? (b) The vapor pressure of pure water at 60 C is 149 torr. The vapor pressure of water over a solution at 60 C containing equal numbers of moles of water and ethylene glycol (a nonvolatile solute) is 67 torr. Is the solu

Chapter: Problem: 65E

Chemistry: The Central Science 13
Problem 65E Colligative Properties (Section) (a) Calculate the vapor pressure of water above a solution prepared by adding 22.5 g of lactose (C12H22011) to 200.0 g of water at 338 K. (Vapor-pressure data for water are given in Appendix B.) (b) Calculate the mass of propylene glycol (C3H802) that

Chapter: Problem: 66E

Chemistry: The Central Science 13
Problem 66E Colligative Properties (Section) (a) Calculate the vapor pressure of water above a solution prepared by dissolving 28.5 g of glycerin (C3H8O3) in 125 g of water at 343 K. (The vapor pressure of water is given in Appendix B.) (b) Calculate the mass of ethylene glycol (C2H6O2) that must b

Chapter: Problem: 67E

Chemistry: The Central Science 13
Problem 67E Colligative Properties (Section) At 63.5 C, the vapor pressure of H20 is 175 torr, and that of ethanol (C2H5OH) is 400 torr. A solution is made by mixing equal masses of H2O and C2H5OH. (a) What is the mole fraction of ethanol in the solution? (b) Assuming ideal-solution behavior, wha

Chapter: Problem: 68E

Chemistry: The Central Science 13
Problem 68E Colligative Properties (Section) At 20 C, the vapor pressure of benzene (C6H6) is 75 torr, and that of toluene (C7H8) is 22 torr. Assume that benzene and toluene form an ideal solution, (a) What is the composition in mole fraction of a solution that has a vapor pressure of 35 torr at

Chapter: Problem: 69E

Chemistry: The Central Science 13
Problem 69E Colligative Properties (Section) (a) Does a 0.10 m aqueous solution of NaCI have a higher boiling point, a lower boiling point, or the same boiling point as a 0.10 m aqueous solution of C6H12O6? (b) The experimental boiling point of the NaCI solution is lower than that calculated assu

Chapter: Problem: 70E

Chemistry: The Central Science 13
Problem 70E Colligative Properties (Section) Arrange the following aqueous solutions, each 10% by mass in solute, in order of increasing boiling point: glucose (C6H12O6), sucrose (C12H22O11), sodium nitrate (NaNO3).

Chapter: Problem: 71E

Chemistry: The Central Science 13
Problem 71E Colligative Properties (Section) List the following aqueous solutions in order of increasing boiling point: 0.120 m glucose, 0.050 m LiBr, 0.050 m Zn(NO3)2.

Chapter: Problem: 72E

Chemistry: The Central Science 13
Problem 72E Colligative Properties (Section) List the following aqueous solutions in order of decreasing freezing point: 0.040 m glycerin (C3H8O3), 0.020 m KBr, 0.030 m phenol (C6H5OH).

Chapter: Problem: 73E

Chemistry: The Central Science 13
Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.22 m glycerol \(\mathrm {\left(C_{3} H_{8} O_{3}\right)}\) in ethanol, (b) 0.240 mol of naphthalene \(\mathrm {\left(C_{10} H_{8}\right)}\) in 2.45 mol of chloroform, (c) 1.50 g NaCl in 0.2

Chapter: Problem: 74E

Chemistry: The Central Science 13
Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.25 m glucose in ethanol; (b) 20.0 g of decane, \(\mathrm{C}_{10} \mathrm{H}_{22}\), in 50.0 g \(\mathrm{CHCl}_{3}\);(c) 3.50 g NaOH in 175 g of water, (d) 0.45 mol ethylene glycol and 0.15

Chapter: Problem: 75E

Chemistry: The Central Science 13
Problem 75E Colligative Properties (Section) How many grams of ethylene glycol (C2H602) must be added to 1.00 kg of water to produce a solution that freezes at -5.00 C?

Chapter: Problem: 76E

Chemistry: The Central Science 13
Problem 76E Colligative Properties (Section) What is the freezing point of an aqueous solution that boils at 105.0 C?

Chapter: Problem: 78E

Chemistry: The Central Science 13
Problem 78E Colligative Properties (Section) Seawater contains 3.4 g of salts for every liter of solution. Assuming that the solute consists entirely of NaCI (in fact, over 90% of the salt is indeed NaCI), calculate the osmotic pressure of seawater at 20 C.

Chapter: Problem: 77E

Chemistry: The Central Science 13
Problem 77E Colligative Properties (Section) What is the osmotic pressure formed by dissolving 44.2 mg of aspirin (C9H8O4) in 0.358 L of water at 25 C?

Chapter: Problem: 79E

Chemistry: The Central Science 13
Adrenaline is the hormone that triggers the release of extra glucose molecules in times of stress or emergency. A solution of 0.64 g of adrenaline in 36.0 g of \(\mathrm{CCl}_{4}\) elevates the boiling point by \(0.49\ { }^{\circ} \mathrm{C}\). Calculate the approximate molar mass of adrenaline from

Chapter: Problem: 80E

Chemistry: The Central Science 13
Problem 80E Lauryl alcohol is obtained from coconut oil and is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1 C. What is the molar mass of lauryl alcohol from this data?

Chapter: Problem: 81E

Chemistry: The Central Science 13
Problem 81E 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?

Chapter: Problem: 82E

Chemistry: The Central Science 13
Problem 82E A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L of solution. The resulting solution has an osmotic pressure of 0.605 atm at 25 C. Assuming that the organic compound is a nonelectrolyte, what is its

Chapter: Problem: 83E

Chemistry: The Central Science 13
Problem 83E The osmotic pressure of a 0.010 M aqueous solution of CaCI2 is found to be 0.674 atm at 25 C. (a) Calculate the van't Hoff factor, /, for the solution, (b) How would you expect the value of / to change as the solution becomes more concentrated? Explain.

Chapter: Problem: 84E

Chemistry: The Central Science 13
Based on the data given in Table 13.4, which solution would give the larger freezing-point lowering, a 0.030 m solution of NaCl or a 0.020 m solution of \(\mathrm{K}_{2} \mathrm{SO}_{4}\)? How do you explain the departure from ideal behavior and the differences observed between the two salts?

Chapter: Problem: 85E

Chemistry: The Central Science 13
Problem 85E Colloids (Section) (a) Do colloids made only of gases exist? Why or why not? (b) In the 1850's, Michael Faraday prepared ruby-red colloids of gold nanoparticles in water that are still stable today. These brightly colored colloids look like solutions. What experiment(s) could you do t

Chapter: Problem: 86E

Chemistry: The Central Science 13
Problem 86E Colloids (Section) Choose the best answer: A colloidal dispersion of one liquid in another is called (a) a gel, (b) an emulsion, (c) a foam, (d) an aerosol.

Chapter: Problem: 87E

Chemistry: The Central Science 13
Problem 87E An emulsifying agent' is a compound that helps stabilize a hydrophobic colloid in a hydrophilic solvent (or a hydrophilic colloid in a hydrophobic solvent). Which of the following choices is the best emulsifying agent? (a) CH3COOH, (b) CH3CH2CH2COOH, (c) CH3(CH2)11COOH, (d) CH3(CH2)11

Chapter: Problem: 88E

Chemistry: The Central Science 13
Problem 88E Aerosols are important components of the atmosphere. Does the presence of aerosols in the atmosphere increase or decrease the amount of sunlight that arrives at the Earth's surface, compared to an aerosol-free' atmosphere? Explain your reasoning.

Chapter: Problem: 89E

Chemistry: The Central Science 13
Problem 89E Proteins can be precipitated out of aqueous solution by the addition of an electrolyte; this process is called salting out'the protein, (a) Do you think that all proteins would be precipitated out to the same extent by the same concentration of the same electrolyte? (b) If a protein h

Chapter: Problem: 90E

Chemistry: The Central Science 13
Problem 90E Explain how (a) a soap such as sodium stearate stabilizes a colloidal dispersion of oil droplets in water; (b) milk curdles upon addition of an acid.

Chapter: Problem: 92AE

Chemistry: The Central Science 13
Problem 92AE A saturated solution of sucrose (C12H22011) is made by dissolving excess table sugar in a flask of water. There are 50 g of undissolved sucrose crystals at the bottom of the flask in contact with the saturated solution. The flask is stoppered and set aside. A year later a single large

Chapter: Problem: 91AE

Chemistry: The Central Science 13
Butylated hydroxytoluene (BHT) has the following molecular structure: It is widely used as a preservative in a variety of foods, including dried cereals. Based on its structure, would you expect BHT to be more soluble in water or in hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)\)? Explai

Chapter: Problem: 93AE

Chemistry: The Central Science 13
Problem 93AE Most fish need at least 4 ppm dissolved 02 in water for survival, (a) What is this concentration in mol/L? (b) What partial pressure of 02 above water is needed to obtain 4 ppm 02 in water at 10 C? (The Henry's law constant for 02 at this temperature is 1.71 * 10-3 mol/L-atm.)

Chapter: Problem: 94AE

Chemistry: The Central Science 13
Problem 94AE The presence of the radioactive gas radon (Rn) in well water presents a possible health hazard in parts of the United States, (a) Assuming that the solubility of radon in water with 1 atm pressure of the gas over the water at 30 C is 7.27 * 10-3 M, what is the Henry's law constant for

Chapter: Problem: 95AE

Chemistry: The Central Science 13
Problem 95AE Glucose makes up about 0.10% by mass of human blood. Calculate this concentration in (a) ppm, (b) molality, (c) What further information would you need to determine the molarity of the solution?

Chapter: Problem: 96AE

Chemistry: The Central Science 13
Problem 96AE The concentration of gold in seawater has been reported to be between 5 ppt (parts per trillion) and 50 ppt. Assuming that seawater contains 13 ppt of gold, calculate the number of grams of gold contained in 1.0 * 103 gal of seawater.

Chapter: Problem: 97AE

Chemistry: The Central Science 13
Problem 97AE The maximum allowable concentration of lead in drinking water is 9.0 ppb. (a) Calculate the molarity of lead in a 9.0-ppb solution, (b) How many grams of lead are in a swimming pool containing 9.0 ppb lead in 60 m3 of water?

Chapter: Problem: 98AE

Chemistry: The Central Science 13
Problem 98AE Acetonitrile (CH3CN) is a polar organic solvent that dissolves a wide range of solutes, including many salts. The density of a 1.80 M LiBr solution in acetonitrile is 0.826 g/cm3. Calculate the concentration of the solution in (a) molality, (b) mole fraction of LiBr, (c) mass percentag

Chapter: Problem: 99AE

Chemistry: The Central Science 13
Problem 99AE A canned heat' product used to warm buffet dishes consists of a homogeneous mixture of ethanol (C2H5OH) and paraffin, which has an average formula of C24H5O. What mass of C2H5OH should be added to 620 kg of the paraffin to produce 8 torr of ethanol vapor pressure at 35 C? The vapor pre

Chapter: Problem: 100AE

Chemistry: The Central Science 13
Problem 100AE A solution contains 0.115 mol H2O and an unknown number of moles of sodium chloride. The vapor pressure of the solution at 30 C is 25.7 torr. The vapor pressure of pure water at this temperature is 31.8 torr. Calculate the number of grams of sodium chloride in the solution. (Hint Reme

Chapter: Problem: 101AE

Chemistry: The Central Science 13
Problem 101AE Two beakers are placed in a sealed box at 25 C. One beaker contains 30.0 ml of a 0.050 M aqueous solution of a non-volatile nonelectrolyte. The other beaker contains 30.0 ml of a 0.035 M aqueous solution of NaCI. The water vapor from the two solutions reaches equilibrium, (a) In which

Chapter: Problem: 102AE

Chemistry: The Central Science 13
Problem 102AE A car owner who knows no chemistry has to put antifreeze in his car's radiator. The instructions recommend a mixture of 30% ethylene glycol and 70% water. Thinking he will improve his protection he uses pure ethylene glycol, which is a liquid at room temperature. He is saddened to fin

Chapter: Problem: 104AE

Chemistry: The Central Science 13
Problem 104AE Carbon disulfide (CS2) boils at 46.30 C and has a density of 1.261 g/ml. (a) When 0.250 mol of a nondissociating solute is dissolved in 400.0 ml_ of CS2, the solution boils at 47.46 C. What is the molal boiling-point-elevation constant for CS2? (b) When 5.39 g of a nondissociating unk

Chapter: Problem: 103AE

Chemistry: The Central Science 13
Calculate the freezing point of a 0.100 m aqueous solution of \(\mathrm{K}_{2} \mathrm{SO}_{4}\), (a) ignoring interionic attractions, and (b) taking interionic attractions into consideration by using the vant Hoff factor (Table 13.4).

Chapter: Problem: 105AE

Chemistry: The Central Science 13
Problem 105AE A lithium salt used in lubricating grease has the formula LiCnH2n + 102. The salt is soluble in water to the extent of0.036 g per 100 g of water at 25 C. The osmotic pressure of this solution is found to be 57.1 torr. Assuming that molality and molarity in such a dilute solution are t

Chapter: Problem: 106AE

Chemistry: The Central Science 13
Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at \(25\ ^{\circ} \mathrm{C}\), and their solubilities in water at \(25\ ^{\circ} \mathrm{C}\) and 1 atm fluorocarbon pressure are give

Chapter: Problem: 108AE

Chemistry: The Central Science 13
Consider the following values for enthalpy of vaporization (kJ/mol) of several organic substances: (a) Account for the variations in heats of vaporization for these substances, considering their relative intermolecular forces. (b) How would you expect the solubilities of these sub- stances to v

Chapter: Problem: 109AE

Chemistry: The Central Science 13
Problem 109AE A textbook on chemical thermodynamics states, "The heat of solution represents the difference between the lattice energy of the crystalline solid and the solvation energy of the gaseous ions.' (a) Draw a simple energy diagram to illustrate this statement, (b) A salt such ? as NaBr is

Chapter: Problem: 110AE

Chemistry: The Central Science 13
Problem 110AE (a) A sample of hydrogen gas is generated in a closed container by reacting 2.050 g of zinc metal with 15.0 ml of 1.00 M sulfuric acid. Write the balanced equation for the reaction, and calculate the number of moles of hydrogen formed, assuming that the reaction is complete.

Chapter: Problem: 107AE

Chemistry: The Central Science 13
Problem 107AE At ordinary body temperature (37 C), the solubility of N2 in water at ordinary atmospheric pressure (1.0 atm) is 0.015 g/L. Air is approximately 78 mol % N2. (a) Calculate the number of moles of N2 dissolved per liter of blood, assuming blood is a simple aqueous solution, (b) At a dep

Chapter: Problem: 112IE

Chemistry: The Central Science 13
Problem 112IE A small cube of lithium (density = 0.535 g/cm3) measuring 1.0 mm on each edge is added to 0.500 L of water. The following reaction occurs: 2 Li(s) + 2 H20(l). 2 LiOH(aq) + H2(g) What is the freezing point of the resultant solution, assuming that the reaction goes to completion?

Chapter: Problem: 111IE

Chemistry: The Central Science 13
The following table presents the solubilities of several gases in water at \(25^{\circ} \mathrm{C}\) under a total pressure of gas and water vapor of 1 atm. (a) What volume of \(\mathrm{CH}_{4}(\mathrm{~g})\) under standard conditions of temperature and pressure is contained in 4.0 L of a saturated s

Chapter: Problem: 113IE

Chemistry: The Central Science 13
At \(35\ ^{\circ} \mathrm{C}\) the vapor pressure of acetone, \(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO}\), is 360 torr, and that of chloroform, \(\mathrm{CHCl}_{3}\), is 300 torr. Acetone and chloroform can form very weak hydrogen bonds between one another; the chlorines on the carbon give the c

Chapter: Problem: 114IE

Chemistry: The Central Science 13
Compounds like sodium stearate, called surfactants in general, can form structures known as micelles in water, once the solution concentration reaches the value known as the critical micelle concentration (cmc). Micelles contain dozens to hundreds of molecules. The cmc depends on the substance, the s

Chapter: Problem: 1DE

Chemistry: The Central Science 13
Based on Figure 13.18, you might think that the reason volatile solvent molecules in a solution are less likely to escape to the gas phase, compared to the pure solvent, is because the solute molecules are physically blocking the solvent molecules from leaving at the surface. This is a common misconc

Chapter: Problem: 1E

Chemistry: The Central Science 13
Visualizing Concepts Rank the contents of the following containers in order of increasing entropy: [Section 13.1]

Chapter: Problem: 2E

Chemistry: The Central Science 13
This figure shows the interaction of a cation with surrounding water molecules. (a) Which atom of water is associated with the cation? Explain. (b) Which of the following explanations accounts for the fact that the ion-solvent interaction is greater for \(\mathrm{Li}^{+}\) than for \(\mathrm{K}

Chapter: Problem: 3E

Chemistry: The Central Science 13
Problem 3E Visualizing Concepts Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies, (a) Will the solids have the same solubility in water? (b) If not, which solid will be more soluble in water, the one with the larger lattice energy or the one wi

Chapter: Problem: 4E

Chemistry: The Central Science 13
Problem 4E Visualizing Concepts Are gases always miscible with each other? Explain. [Section]

Chapter: Problem: 5E

Chemistry: The Central Science 13
Which of the following is the best representation of a saturated solution? Explain your reasoning. [Section 13.2]

Chapter: Problem: 6E

Chemistry: The Central Science 13
The solubility of Xe in water at 1 atm pressure and \(20\ ^{\circ} \mathrm{C}\) is approximately \(5 \times 10^{-3}\ M\). (a) Compare this with the solubilities of Ar and Kr in water (Table 13.1). (b) What properties of the rare gas atoms account for the variation in solubility? [Section 13.3]

Chapter: Problem: 7E

Chemistry: The Central Science 13
The structures of vitamins E and \(\mathrm{B}_{6}\) are shown below. Predict which is more water soluble and which is more fat soluble. Explain. [Section 13.3] Equation Transcription: Text Transcription: B_6 B_6

Chapter: Problem: 8E

Chemistry: The Central Science 13
Problem 8E Visualizing Concepts You take a sample of water that is at room temperature and in contact with air and put it under a vacuum. Right away, you see bubbles leave the water, but after a little while, the bubbles stop. As you keep applying the vacuum, more bubbles appear. A friend tells you

Chapter: Problem: 9E

Chemistry: The Central Science 13
The figure shows two identical volumetric flasks containing the same solution at two temperatures. 1. Does the molarity of the solution change with the change in temperature? Explain. 2. Does the molality of the solution change with the change in temperature? Explain. [Section 13.4]

Chapter: Problem: 10E

Chemistry: The Central Science 13
This portion of a phase diagram shows the vapor-pressure curves of a volatile solvent and of a solution of that solvent containing a nonvolatile solute. (a) Which line represents the solution? (b) What are the normal boiling points of the solvent and the solution? [Section 13.5]

Chapter: Problem: 11E

Chemistry: The Central Science 13
Suppose you had a balloon made of some highly flexible semi-permeable membrane. The balloon is filled completely with a 0.2 M solution of some solute and is submerged in a 0.1 M solution of the same solute: Initially, the volume of solution in the balloon is 0.25 L. Assuming the volume outside

Chapter: Problem: 12E

Chemistry: The Central Science 13
The molecule n-octylglucoside, shown here, is widely used in biochemical research as a nonionic detergent for solubilizing large hydrophobic protein molecules. What characteristics of this molecule are important for its use in this way? [Section 13.6]

Chapter: Problem: 13E

Chemistry: The Central Science 13
Problem 13E The Solution Process (Section) Indicate whether each statement is true or false: (a) A solute will dissolve in a solvent if solute-solute interactions are stronger than solute-solvent interactions. (b) In making a solution, the enthalpy of mixing is always a positive num

Chapter: Problem: 14E

Chemistry: The Central Science 13
Indicate whether each statement is true or false: (a) NaCl dissolves in water but not in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) because benzene is denser than water. (b) NaCl dissolves in water but not in ben- zene because water has a large dipole moment and benzene has zero dipole mo

Chapter: Problem: 16E

Chemistry: The Central Science 13
Problem 16E The Solution Process (Section) Indicate the principal type of solute-solvent interaction in each of the following solutions and rank the solutions from weakest to strongest solute-solvent interaction: (a) KCI in water, (b) CH2CI2 in benzene (C6H6), (c) methanol (CH3OH) in water.

Chapter: Problem: 15E

Chemistry: The Central Science 13
Problem 15E The Solution Process (Section) Indicate the type of solute-solvent interaction (Section) that should be most important in each of the following solutions: (a) CCI4 in benzene (C6H6), (b) methanol (CH30H) in water, (c) KBr in water, (d) HCI in acetonitrile (CH3CN).

Chapter: Problem: 17E

Chemistry: The Central Science 13
Problem 17E The Solution Process (Section) An ionic compound has a very negative ?Hsoln in water. (a) Would you expect it to be very soluble or nearly insoluble in water? (b) Which term would you expect to be the largest negative number: ?Hsolvent, ?Hsolute, or ?Hmix?

Chapter: Problem: 18E

Chemistry: The Central Science 13
Problem 18E The Solution Process (Section) When ammonium chloride dissolves in water, the solution becomes colder, (a) Is the solution process exothermic or endothermic? (b) Why does the solution form?

Chapter: Problem: 19E

Chemistry: The Central Science 13
Problem 19E (a) In Equation, which of the enthalpy terms for dissolving an ionic solid would correspond to the lattice energy? (b) Which energy term in this equation is always exothermic? ?Hsoln = ?Hsolute + ?Hsolvent + ?Hmix

Chapter: Problem: 20E

Chemistry: The Central Science 13
Problem 20E The Solution Process (Section) For the dissolution of LiCl in water, ?Hsoln = -37 kJ/mol. Which term would you expect to be the largest negative number: ?Hsolvent, ?Hsolute, or ?Hmix?

Chapter: Problem: 21E

Chemistry: The Central Science 13
Two nonpolar organic liquids, hexane \(\left(\mathrm{C}_{6} \mathrm{H}_{14}\right)\) and heptane \(\left(\mathrm{C}_{7} \mathrm{H}_{16}\right)\), are mixed. (a) Do you expect \(\Delta H_{\mathrm{soln}}\) to be a large positive number, a large negative number, or close to zero? Explain. (b) Hexane and

Chapter: Problem: 22E

Chemistry: The Central Science 13
Problem 22E The Solution Process (Section) The enthalpy of solution of KBr in water is about +198 kJ/mol. Nevertheless, the solubility of KBr in water is relatively high. Why does the solution process occur even though it is endothermic?

Chapter: Problem: 23E

Chemistry: The Central Science 13
Problem 23E Saturated Solutions; Factors Affecting Solubility (Sections) The solubility of Cr(N03)3*9 H20 in water is 208 g per 100 g of water at 15 C. A solution of Cr(NO3)3*9 H2O in water at 35 C is formed by dissolving 324 g in 100 g of water. When this solution is slowly cooled to 15 C, no prec

Chapter: Problem: 24E

Chemistry: The Central Science 13
The solubility of \(\mathrm{MnSO}_{4} \cdot \mathrm{H}_{2} \mathrm{O}\) in water at \(20\ ^{\circ} \mathrm{C}\) is 70 g per 100 mL of water. (a) Is a 1.22 M solution of \(\mathrm{MnSO}_{4} \cdot \mathrm{H}_{2} \mathrm{O}\) in water at \(20\ ^{\circ} \mathrm{C}\) saturated, supersaturated, or unsatura

Chapter: Problem: 25E

Chemistry: The Central Science 13
By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at \(40^{\circ} \mathrm{C}\) will lead to a saturated solution: (a) \(\mathrm{NaNO}_{3}\), (b) KCl, (c) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\), (d) \(\mathrm{~Pb}\

Chapter: Problem: 26E

Chemistry: The Central Science 13
By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at \(30\ ^{\circ} \mathrm{C}\): (a) \(\mathrm{KClO}_{3}\), (b) \(\mathrm{~Pb}\left(\mathrm{NO}_{3}\right)_{2}\), (c) \(\mathrm{Ce}_{2}(\mathrm{SO} 4)_{3}\).

Chapter: Problem: 13.1

Chemistry: The Central Science 13
Rank the contents of the following containers in order of increasing entropy: [Section 13.1] (a) (b) (c)

Chapter: Problem: 13.2

Chemistry: The Central Science 13
This figure shows the interaction of a cation with surrounding water molecules. + (a) Which atom of water is associated with the cation? Explain. (b) Which of the following explanations accounts for the fact that the ion-solvent interaction is greater for Li + than for K+? a. Li + is of lower mass th

Chapter: Problem: 13.3

Chemistry: The Central Science 13
Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies. (a) Will the solids have the same solubility in water? (b) If not, which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assum

Chapter: Problem: 13.4

Chemistry: The Central Science 13
Are gases always miscible with each other? Explain. [Section 13.1]

Chapter: Problem: 13.5

Chemistry: The Central Science 13
Which of the following is the best representation of a saturated solution? Explain your reasoning. [Section 13.2] (a) (b) (c)

Chapter: Problem: 13.6

Chemistry: The Central Science 13
The solubility of Xe in water at 1 atm pressure and 20 C is approximately 5 * 10-3 M. (a) Compare this with the solubilities of Ar and Kr in water (Table 13.1). (b) What properties of the rare gas atoms account for the variation in solubility? [Section 13.3]

Chapter: Problem: 13.7

Chemistry: The Central Science 13
The structures of vitamins E and B6 are shown below. Predict which is more water soluble and which is more fat soluble. Explain. [Section 13.3] Vitamin B6 Vitamin E

Chapter: Problem: 13.8

Chemistry: The Central Science 13
You take a sample of water that is at room temperature and in contact with air and put it under a vacuum. Right away, you see bubbles leave the water, but after a little while, the bubbles stop. As you keep applying the vacuum, more bubbles appear. A friend tells you that the first bubbles were water

Chapter: Problem: 13.9

Chemistry: The Central Science 13
The figure shows two identical volumetric flasks containing the same solution at two temperatures. (a) Does the molarity of the solution change with the change in temperature? Explain. (b) Does the molality of the solution change with the change in temperature? Explain. [Section 13.4] 25 C 55 C

Chapter: Problem: 13.10

Chemistry: The Central Science 13
This portion of a phase diagram shows the vapor-pressure curves of a volatile solvent and of a solution of that solvent containing a nonvolatile solute. (a) Which line represents the solution? (b) What are the normal boiling points of the solvent and the solution? [Section 13.5] 40 1.0 50 60 70 T (C)

Chapter: Problem: 13.11

Chemistry: The Central Science 13
Suppose you had a balloon made of some highly flexible semipermeable membrane. The balloon is filled completely with a 0.2 M solution of some solute and is submerged in a 0.1 M solution of the same solute: 0.1 M 0.2 M Initially, the volume of solution in the balloon is 0.25 L. Assuming the volume out

Chapter: Problem: 13.12

Chemistry: The Central Science 13
The molecule n-octylglucoside, shown here, is widely used in biochemical research as a nonionic detergent for solubilizing large hydrophobic protein molecules. What characteristics of this molecule are important for its use in this way? [Section 13.6]

Chapter: Problem: 13.13

Chemistry: The Central Science 13
Indicate whether each statement is true or false: (a) A solute will dissolve in a solvent if solutesolute interactions are stronger than solute-solvent interactions.(b) In making a solution, the enthalpy of mixing is always a positive number. (c) An increase in entropy favors mixing.

Chapter: Problem: 13.14

Chemistry: The Central Science 13
Indicate whether each statement is true or false: (a) NaCl dissolves in water but not in benzene 1C6H62 because benzene is denser than water. (b) NaCl dissolves in water but not in benzene because water has a large dipole moment and benzene has zero dipole moment. (c) NaCl dissolves in water but not

Chapter: Problem: 13.15

Chemistry: The Central Science 13
Indicate the type of solutesolvent interaction (Section 11.2) that should be most important in each of the following solutions: (a) CCl4 in benzene 1C6H62, (b) methanol 1CH3OH2 in water, (c) KBr in water, (d) HCl in acetonitrile 1CH3CN2.

Chapter: Problem: 13.16

Chemistry: The Central Science 13
Indicate the principal type of solutesolvent interaction in each of the following solutions and rank the solutions from weakest to strongest solutesolvent interaction: (a) KCl in water, (b) CH2Cl2 in benzene 1C6H62, (c) methanol 1CH3OH2 in water.

Chapter: Problem: 13.17

Chemistry: The Central Science 13
An ionic compound has a very negative Hsoln in water. (a) Would you expect it to be very soluble or nearly insoluble in water? (b) Which term would you expect to be the largest negative number: Hsolvent, Hsolute, or Hmix?

Chapter: Problem: 13.18

Chemistry: The Central Science 13
When ammonium chloride dissolves in water, the solution becomes colder. (a) Is the solution process exothermic or endothermic? (b) Why does the solution form?

Chapter: Problem: 13.19a

Chemistry: The Central Science 13
(a) In Equation 13.1, which of the enthalpy terms for dissolving an ionic solid would correspond to the lattice energy?

Chapter: Problem: 13.19b

Chemistry: The Central Science 13
(b) Which energy term in this equation is always exothermic?

Chapter: Problem: 13.20

Chemistry: The Central Science 13
For the dissolution of LiCl in water, Hsoln = -37 kJ>mol. Which term would you expect to be the largest negative number: Hsolvent, Hsolute, or Hmix?

Chapter: Problem: 13.21

Chemistry: The Central Science 13
Two nonpolar organic liquids, hexane 1C6H142 and heptane 1C7H162, are mixed. (a) Do you expect Hsoln to be a large positive number, a large negative number, or close to zero? Explain. (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy

Chapter: Problem: 13.22

Chemistry: The Central Science 13
The enthalpy of solution of KBr in water is about +198 kJ>mol. Nevertheless, the solubility of KBr in water is relatively high. Why does the solution process occur even though it is endothermic?

Chapter: Problem: 13.23

Chemistry: The Central Science 13
The solubility of Cr1NO323 # 9 H2O in water is 208 g per 100 g of water at 15 C. A solution of Cr1NO323 # 9 H2O in water at 35 C is formed by dissolving 324 g in 100 g of water. When this solution is slowly cooled to 15 C, no precipitate forms. (a) What term describes this solution? (b) What action m

Chapter: Problem: 13.24

Chemistry: The Central Science 13
The solubility of MnSO4 # H2O in water at 20 C is 70 g per 100 mL of water. (a) Is a 1.22 M solution of MnSO4 # H2O in water at 20 C saturated, supersaturated, or unsaturated? (b) Given a solution of MnSO4 # H2O of unknown concentration, what experiment could you perform to determine whether the new

Chapter: Problem: 13.25

Chemistry: The Central Science 13
The solubility of MnSO4 # H2O in water at 20 C is 70 g per 100 mL of water. (a) Is a 1.22 M solution of MnSO4 # H2O in water at 20 C saturated, supersaturated, or unsaturated? (b) Given a solution of MnSO4 # H2O of unknown concentration, what experiment could you perform to determine whether the new

Chapter: Problem: 13.26

Chemistry: The Central Science 13
By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 C: (a) KClO3, (b) Pb1NO322, (c) Ce21SO423.

Chapter: Problem: 13.27

Chemistry: The Central Science 13
Consider water and glycerol, CH21OH2CH1OH2CH2OH. (a) Would you expect them to be miscible in all proportions? Explain. (b) List the intermolecular attractions that occur between a water molecule and a glycerol molecule.

Chapter: Problem: 13.28

Chemistry: The Central Science 13
Oil and water are immiscible. Which is the most likely reason? (a) Oil molecules are denser than water. (b) Oil molecules are composed mostly of carbon and hydrogen. (c) Oil molecules have higher molar masses than water. (d) Oil molecules have higher vapor pressures than water. (e) Oil molecules have

Chapter: Problem: 13.29

Chemistry: The Central Science 13
Common laboratory solvents include acetone 1CH3COCH32, methanol 1CH3OH2, toluene 1C6H5CH32, and water. Which of these is the best solvent for nonpolar solutes?

Chapter: Problem: 13.30

Chemistry: The Central Science 13
Would you expect alanine (an amino acid) to be more soluble in water or in hexane? Explain. Alanine

Chapter: Problem: 13.31a

Chemistry: The Central Science 13
(a) Would you expect stearic acid, CH31CH2216COOH, to be more soluble in water or in carbon tetrachloride? Explain.

Chapter: Problem: 13.31b

Chemistry: The Central Science 13
(b) Which would you expect to be more soluble in water, cyclohexane or dioxane? Explain. H2C H2C CH2 CH2 O O Dioxane H2C H2C CH2 CH2 CH2 CH2 Cyclohexane

Chapter: Problem: 13.32

Chemistry: The Central Science 13
Ibuprofen, widely used as a pain reliever, has a limited solubility in water, less than 1 mg>mL. Which part of the molecules structure (gray, white, red) contributes to its water solubility? Which part of the molecule (gray, white, red) contributes to its water insolubility? Ibuprofen

Chapter: Problem: 13.33

Chemistry: The Central Science 13
Which of the following in each pair is likely to be more soluble in hexane, C6H14: (a) CCl4 or CaCl2, (b) benzene 1C6H62 or glycerol, CH21OH2CH1OH2CH2OH, (c) octanoic acid, CH3CH2CH2CH2CH2CH2CH2COOH, or acetic acid, CH3COOH? Explain your answer in each case

Chapter: Problem: 13.34

Chemistry: The Central Science 13
Which of the following in each pair is likely to be more soluble in water: (a) cyclohexane 1C6H122 or glucose 1C6H12O62, (b) propionic acid 1CH3CH2COOH2 or sodium propionate 1CH3CH2COONa2, (c) HCl or ethyl chloride 1CH3CH2Cl2? Explain in each case.

Chapter: Problem: 13.35a

Chemistry: The Central Science 13
(a) Explain why carbonated beverages must be stored in sealed containers.

Chapter: Problem: 13.35b

Chemistry: The Central Science 13
(b) Once the beverage has been opened, why does it maintain more carbonation when refrigerated than at room temperature?

Chapter: Problem: 13.36

Chemistry: The Central Science 13
Explain why pressure substantially affects the solubility of O2 in water but has little effect on the solubility of NaCl in water.

Chapter: Problem: 13.37

Chemistry: The Central Science 13
The Henrys law constant for helium gas in water at 30 C is 3.7 * 10-4 M>atm and the constant for N2 at 30 C is 6.0 * 10-4 M>atm. If the two gases are each present at 1.5 atm pressure, calculate the solubility of each gas.

Chapter: Problem: 13.38

Chemistry: The Central Science 13
The partial pressure of O2 in air at sea level is 0.21 atm. Using the data in Table 13.1, together with Henrys law, calculate the molar concentration of O2 in the surface water of a mountain lake saturated with air at 20 C and an atmospheric pressure of 650 torr.

Chapter: Problem: 13.39a

Chemistry: The Central Science 13
(a) Calculate the mass percentage of Na2SO4 in a solution containing 10.6 g of Na2SO4 in 483 g of water.

Chapter: Problem: 13.39b

Chemistry: The Central Science 13
(b) An ore contains 2.86 g of silver per ton of ore. What is the concentration of silver in ppm?

Chapter: Problem: 13.40a

Chemistry: The Central Science 13
(a) What is the mass percentage of iodine in a solution containing 0.035 mol I2 in 125 g of CCl4?

Chapter: Problem: 13.40b

Chemistry: The Central Science 13
(b) Seawater contains 0.0079 g of Sr 2+ per kilogram of water. What is the concentration of Sr 2+ in ppm?

Chapter: Problem: 13.41

Chemistry: The Central Science 13
A solution is made containing 14.6 g of CH3OH in 184 g of H2O. Calculate (a) the mole fraction of CH3OH, (b) the mass percent of CH3OH, (c) the molality of CH3OH.

Chapter: Problem: 13.42

Chemistry: The Central Science 13
A solution is made containing 20.8 g of phenol 1C6H5OH2 in 425 g of ethanol 1CH3CH2OH2. Calculate (a) the mole fraction of phenol, (b) the mass percent of phenol, (c) the molality of phenol.

Chapter: Problem: 13.43

Chemistry: The Central Science 13
Calculate the molarity of the following aqueous solutions: (a) 0.540 g of Mg1NO322 in 250.0 mL of solution, (b) 22.4 g of LiClO4 # 3 H2O in 125 mL of solution, (c) 25.0 mL of 3.50 M HNO3 diluted to 0.250 L.

Chapter: Problem: 13.44

Chemistry: The Central Science 13
What is the molarity of each of the following solutions: (a) 15.0 g of Al21SO423 in 0.250 mL solution, (b) 5.25 g of Mn1NO322 # 2 H2O in 175 mL of solution, (c) 35.0 mL of 9.00 M H2SO4 diluted to 0.500 L?

Chapter: Problem: 13.45

Chemistry: The Central Science 13
Calculate the molality of each of the following solutions: (a) 8.66 g of benzene 1C6H62 dissolved in 23.6 g of carbon tetrachloride 1CCl42, (b) 4.80 g of NaCl dissolved in 0.350 L of water

Chapter: Problem: 13.46a

Chemistry: The Central Science 13
(a) What is the molality of a solution formed by dissolving 1.12 mol of KCl in 16.0 mol of water?

Chapter: Problem: 13.46b

Chemistry: The Central Science 13
(b) How many grams of sulfur 1S82 must be dissolved in 100.0 g of naphthalene 1C10H82 to make a 0.12 m solution?

Chapter: Problem: 13.47

Chemistry: The Central Science 13
A sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution has a density of 1.329 g>cm3 . Calculate A sulfuric acid solution containing 571.6 g of H2SO4 perliter of solution has a density of 1.329 g>cm3 .

Chapter: Problem: 13.48

Chemistry: The Central Science 13
Ascorbic acid 1vitamin C, C6H8O62 is a water-soluble vitamin. A solution containing 80.5 g of ascorbic acid dissolved in 210 g of water has a density of 1.22 g>mL at 55 C. Calculate (a) the mass percentage, (b) the mole fraction, (c) the molality, (d) the molarity of ascorbic acid in this solution.

Chapter: Problem: 13.49

Chemistry: The Central Science 13
The density of acetonitrile 1CH3CN2 is 0.786 g>mL and the density of methanol 1CH3OH2 is 0.791 g>mL. A solution is made by dissolving 22.5 mL of CH3OH in 98.7 mL of CH3CN. (a) What is the mole fraction of methanol in the solution? (b) What is the molality of the solution? (c) Assuming that the volume

Chapter: Problem: 13.50

Chemistry: The Central Science 13
The density of toluene 1C7H82 is 0.867 g>mL, and the density of thiophene 1C4H4S2 is 1.065 g>mL. A solution is made by dissolving 8.10 g of thiophene in 250.0 mL of toluene. (a) Calculate the mole fraction of thiophene in the solution. (b) Calculate the molality of thiophene in the solution. (c) Assu

Chapter: Problem: 13.51

Chemistry: The Central Science 13
Calculate the number of moles of solute present in each of the following aqueous solutions: (a) 600 mL of 0.250 M SrBr2, (b) 86.4 g of 0.180 m KCl, (c) 124.0 g of a solution that is 6.45% glucose 1C6H12O62 by mass.

Chapter: Problem: 13.52

Chemistry: The Central Science 13
Calculate the number of moles of solute present in each of the following solutions: (a) 255 mL of 1.50 M HNO31aq2, (b) 50.0 mg of an aqueous solution that is 1.50 m NaCl, (c) 75.0 g of an aqueous solution that is 1.50% sucrose 1C12H22O112 by mass.

Chapter: Problem: 13.53

Chemistry: The Central Science 13
Describe how you would prepare each of the following aqueous solutions, starting with solid KBr: (a) 0.75 L of 1.5 * 10-2 M KBr, (b) 125 g of 0.180 m KBr, (c) 1.85 L of a solution that is 12.0% KBr by mass (the density of the solution is 1.10 g>mL), (d) a 0.150 M solution of KBr that contains just en

Chapter: Problem: 13.54

Chemistry: The Central Science 13
Describe how you would prepare each of the following aqueous solutions: (a) 1.50 L of 0.110 M 1NH422SO4 solution, starting with solid 1NH422SO4; (b) 225 g of a solution that is 0.65 m in Na2CO3, starting with the solid solute; (c) 1.20 L of a solution that is 15.0% Pb1NO322 by mass (the density of th

Chapter: Problem: 13.55

Chemistry: The Central Science 13
Commercial aqueous nitric acid has a density of 1.42 g>mL and is 16 M. Calculate the percent HNO3 by mass in the solution.

Chapter: Problem: 13.56

Chemistry: The Central Science 13
Commercial concentrated aqueous ammonia is 28% NH3 by mass and has a density of 0.90 g>mL. What is the molarity of this solution?

Chapter: Problem: 13.57

Chemistry: The Central Science 13
Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of 80.0% Cu and 20.0% Zn by mass has a density of 8750 kg>m3 . (a) What is the molality of Zn in the solid solution? (b) What is the molarity of Zn in the solution?

Chapter: Problem: 13.58

Chemistry: The Central Science 13
Caffeine 1C8H10N4O22 is a stimulant found in coffee and tea. If a solution of caffeine in the solvent chloroform 1CHCl32 has a concentration of 0.0500 m, calculate (a) the percentage of caffeine by mass, (b) the mole fraction of caffeine in the solution. Caffeine

Chapter: Problem: 13.59

Chemistry: The Central Science 13
During a persons typical breathing cycle, the CO2 concentration in the expired air rises to a peak of 4.6% by volume. (a) Calculate the partial pressure of the CO2 in the expired air at its peak, assuming 1 atm pressure and a body temperature of 37 C. (b) What is the molarity of the CO2 in the expire

Chapter: Problem: 13.60

Chemistry: The Central Science 13
Breathing air that contains 4.0% by volume CO2 over time causes rapid breathing, throbbing headache, and nausea, among other symptoms. What is the concentration of CO2 in such air in terms of (a) mol percentage, (b) molarity, assuming 1 atm pressure and a body temperature of 37 C?

Chapter: Problem: 13.61

Chemistry: The Central Science 13
You make a solution of a nonvolatile solute with a liquid solvent. Indicate whether each of the following statements is true or false. (a) The freezing point of the solution is higher than that of the pure solvent. (b) The freezing point of the solution is lower than that of the pure solvent. (c) The

Chapter: Problem: 13.62

Chemistry: The Central Science 13
You make a solution of a nonvolatile solute with a liquid solvent. Indicate if each of the following statements is true or false. (a) The freezing point of the solution is unchanged by addition of the solvent. (b) The solid that forms as the solution freezes is nearly pure solute. (c) The freezing po

Chapter: Problem: 13.63

Chemistry: The Central Science 13
Consider two solutions, one formed by adding 10 g of glucose 1C6H12O62 to 1 L of water and the other formed by adding 10 g of sucrose 1C12H22O112 to 1 L of water. Calculate the vapor pressure for each solution at 20 C; the vapor pressure of pure water at this temperature is 17.5 torr

Chapter: Problem: 13.64a

Chemistry: The Central Science 13
(a) What is an ideal solution?

Chapter: Problem: 13.64b

Chemistry: The Central Science 13
(b) The vapor pressure of pure water at 60 C is 149 torr. The vapor pressure of water over a solution at 60 C containing equal numbers of moles of water and ethylene glycol (a nonvolatile solute) is 67 torr. Is the solution ideal according to Raoults law? Explain.

Chapter: Problem: 13.65a

Chemistry: The Central Science 13
(a) Calculate the vapor pressure of water above a solution prepared by adding 22.5 g of lactose 1C12H22O112 to 200.0 g of water at 338 K. (Vapor-pressure data for water are given in Appendix B.)

Chapter: Problem: 13.65b

Chemistry: The Central Science 13
(b) Calculate the mass of propylene glycol 1C3H8O22 that must be added to 0.340 kg of water to reduce the vapor pressure by 2.88 torr at 40 C.

Chapter: Problem: 13.66a

Chemistry: The Central Science 13
(a) Calculate the vapor pressure of water above a solution prepared by dissolving 28.5 g of glycerin 1C3H8O32 in 125 g of water at 343 K. (The vapor pressure of water is given in Appendix B.)

Chapter: Problem: 1366b

Chemistry: The Central Science 13
(b) Calculate the mass of ethylene glycol 1C2H6O22 that must be added to 1.00 kg of ethanol 1C2H5OH2 to reduce its vapor pressure by 10.0 torr at 35 C. The vapor pressure of pure ethanol at 35 C is 1.00 * 102 torr.

Chapter: Problem: 13.67

Chemistry: The Central Science 13
At 63.5 C, the vapor pressure of H2O is 175 torr, and that of ethanol 1C2H5OH2 is 400 torr. A solution is made by mixing equal masses of H2O and C2H5OH. (a) What is the mole fraction of ethanol in the solution? (b) Assuming ideal-solution behavior, what is the vapor pressure of the solution at 63.5 C

Chapter: Problem: 13.68

Chemistry: The Central Science 13
At 20 C, the vapor pressure of benzene 1C6H62 is 75 torr, and that of toluene 1C7H82 is 22 torr. Assume that benzene and toluene form an ideal solution. (a) What is the composition in mole fraction of a solution that has a vapor pressure of 35 torr at 20 C? (b) What is the mole fraction of benzene in

Chapter: Problem: 13.69a

Chemistry: The Central Science 13
(a) Does a 0.10 m aqueous solution of NaCl have a higher boiling point, a lower boiling point, or the same boiling point as a 0.10 m aqueous solution of C6H12O6?

Chapter: Problem: 13.69b

Chemistry: The Central Science 13
(b) The experimental boiling point of the NaCl solution is lower than that calculated assuming that NaCl is completely dissociated in solution. Why is this the case?

Chapter: Problem: 13.70

Chemistry: The Central Science 13
Arrange the following aqueous solutions, each 10% by mass in solute, in order of increasing boiling point: glucose 1C6H12O62, sucrose 1C12H22O112, sodium nitrate 1NaNO32.

Chapter: Problem: 13.71

Chemistry: The Central Science 13
List the following aqueous solutions in order of increasing boiling point: 0.120 m glucose, 0.050 m LiBr, 0.050 m Zn1NO322.

Chapter: Problem: 13.72

Chemistry: The Central Science 13
List the following aqueous solutions in order of decreasing freezing point: 0.040 m glycerin 1C3H8O32, 0.020 m KBr, 0.030 m phenol 1C6H5OH2.

Chapter: Problem: 13.73

Chemistry: The Central Science 13
Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.22 m glycerol 1C3H8O32 in ethanol, (b) 0.240 mol of naphthalene 1C10H82 in 2.45 mol of chloroform, (c) 1.50 g NaCl in 0.250 kg of water, (d) 2.04 g KBr and 4.82 g glucose 1C6H12O62 in 188 g

Chapter: Problem: 13.74

Chemistry: The Central Science 13
Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (a) 0.25 m glucose in ethanol; (b) 20.0 g of decane, C10H22, in 50.0 g CHCl3;(c) 3.50 g NaOH in 175 g of water, (d) 0.45 mol ethylene glycol and 0.15 mol KBr in 150 g H2O.

Chapter: Problem: 13.75

Chemistry: The Central Science 13
How many grams of ethylene glycol 1C2H6O22 must be added to 1.00 kg of water to produce a solution that freezes at -5.00 C?

Chapter: Problem: 13.76

Chemistry: The Central Science 13
What is the freezing point of an aqueous solution that boils at 105.0 C?

Chapter: Problem: 13.77

Chemistry: The Central Science 13
What is the osmotic pressure formed by dissolving 44.2 mg of aspirin 1C9H8O42 in 0.358 L of water at 25 C?

Chapter: Problem: 13.78

Chemistry: The Central Science 13
Seawater contains 3.4 g of salts for every liter of solution. Assuming that the solute consists entirely of NaCl (in fact, over 90% of the salt is indeed NaCl), calculate the osmotic pressure of seawater at 20 C.

Chapter: Problem: 13.79

Chemistry: The Central Science 13
Adrenaline is the hormone that triggers the release of extra glucose molecules in times of stress or emergency. A solution of 0.64 g of adrenaline in 36.0 g of CCl4 elevates the boiling point by 0.49 C. Calculate the approximate molar mass of adrenaline from this data. Adrenaline

Chapter: Problem: 13.80

Chemistry: The Central Science 13
Lauryl alcohol is obtained from coconut oil and is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1 C. What is the molar mass of lauryl alcohol from this data?

Chapter: Problem: 13.81

Chemistry: The Central Science 13
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?

Chapter: Problem: 13.82

Chemistry: The Central Science 13
A dilute aqueous solution of an organic compound soluble in water is formed by dissolving 2.35 g of the compound in water to form 0.250 L of solution. The resulting solution has an osmotic pressure of 0.605 atm at 25 C. Assuming that the organic compound is a nonelectrolyte, what is its molar mass?

Chapter: Problem: 13.83

Chemistry: The Central Science 13
The osmotic pressure of a 0.010 M aqueous solution of CaCl2 is found to be 0.674 atm at 25 C. (a) Calculate the vant Hoff factor, i, for the solution. (b) How would you expect the value of i to change as the solution becomes more concentrated? Explain.

Chapter: Problem: 13.84

Chemistry: The Central Science 13
Based on the data given in Table 13.4, which solution would give the larger freezing-point lowering, a 0.030 m solution of NaCl or a 0.020 m solution of K2SO4? How do you explain the departure from ideal behavior and the differences observed between the two salts?

Chapter: Problem: 13.85a

Chemistry: The Central Science 13
(a) Do colloids made only of gases exist? Why or why not?

Chapter: Problem: 13.85b

Chemistry: The Central Science 13
(b) In the 1850s, Michael Faraday prepared ruby-red colloids of gold nanoparticles in water that are still stable today. These brightly colored colloids look like solutions. What experiment(s) could you do to determine whether a given colored preparation is a solution or colloid?

Chapter: Problem: 13.86

Chemistry: The Central Science 13
Choose the best answer: A colloidal dispersion of one liquid in another is called (a) a gel, (b) an emulsion, (c) a foam, (d) an aerosol.

Chapter: Problem: 13.87

Chemistry: The Central Science 13
An emulsifying agent is a compound that helps stabilize a hydrophobic colloid in a hydrophilic solvent (or a hydrophilic colloid in a hydrophobic solvent). Which of the following choices is the best emulsifying agent? (a) CH3COOH, (b) CH3CH2CH2COOH, (c) CH31CH2211COOH, (d) CH31CH2211COONa.

Chapter: Problem: 13.88

Chemistry: The Central Science 13
Aerosols are important components of the atmosphere. Does the presence of aerosols in the atmosphere increase or decrease the amount of sunlight that arrives at the Earths surface, compared to an aerosol-free atmosphere? Explain your reasoning.

Chapter: Problem: 13.89

Chemistry: The Central Science 13
roteins can be precipitated out of aqueous solution by the addition of an electrolyte; this process is called salting out the protein. (a) Do you think that all proteins would be precipitated out to the same extent by the same concentration of the same electrolyte? (b) If a protein has been salted ou

Chapter: Problem: 13.90

Chemistry: The Central Science 13
Explain how (a) a soap such as sodium stearate stabilizes a colloidal dispersion of oil droplets in water; (b) milk curdles upon addition of an acid.

Chapter: Problem: 13.91

Chemistry: The Central Science 13
Butylated hydroxytoluene (BHT) has the following molecular structure: H3C C CH3 CH3 OH CH3 BHT CH3 C CH3 CH3 It is widely used as a preservative in a variety of foods, including dried cereals. Based on its structure, would you expect BHT to be more soluble in water or in hexane 1C6H142? Explain.

Chapter: Problem: 13.92

Chemistry: The Central Science 13
A saturated solution of sucrose 1C12H22O112 is made by dissolving excess table sugar in a flask of water. There are 50 g of undissolved sucrose crystals at the bottom of the flask in contact with the saturated solution. The flask is stoppered and set aside. A year later a single large crystal of mass

Chapter: Problem: 13.93

Chemistry: The Central Science 13
Most fish need at least 4 ppm dissolved O2 in water for survival. (a) What is this concentration in mol>L? (b) What partial pressure of O2 above water is needed to obtain 4 ppm O2 in water at 10 C? (The Henrys law constant for O2 at this temperature is 1.71 * 10-3 mol>L@atm.)

Chapter: Problem: 13.94

Chemistry: The Central Science 13
The presence of the radioactive gas radon (Rn) in well water presents a possible health hazard in parts of the United States. (a) Assuming that the solubility of radon in water with 1 atm pressure of the gas over the water at 30 C is 7.27 * 10-3 M, what is the Henrys law constant for radon in water a

Chapter: Problem: 13.95

Chemistry: The Central Science 13
Glucose makes up about 0.10% by mass of human blood. Calculate this concentration in (a) ppm, (b) molality. (c) What further information would you need to determine the molarity of the solution?

Chapter: Problem: 13.96

Chemistry: The Central Science 13
The concentration of gold in seawater has been reported to be between 5 ppt (parts per trillion) and 50 ppt. Assuming that seawater contains 13 ppt of gold, calculate the number of grams of gold contained in 1.0 * 103 gal of seawater.

Chapter: Problem: 13.97

Chemistry: The Central Science 13
The maximum allowable concentration of lead in drinking water is 9.0 ppb. (a) Calculate the molarity of lead in a 9.0- ppb solution. (b) How many grams of lead are in a swimming pool containing 9.0 ppb lead in 60 m3 of water?

Chapter: Problem: 13.98

Chemistry: The Central Science 13
Acetonitrile 1CH3CN2 is a polar organic solvent that dissolves a wide range of solutes, including many salts. The density of a 1.80 M LiBr solution in acetonitrile is 0.826 g>cm3 . Calculate the concentration of the solution in (a) molality, (b) mole fraction of LiBr, (c) mass percentage of CH3CN

Chapter: Problem: 13.99

Chemistry: The Central Science 13
A canned heat product used to warm buffet dishes consists of a homogeneous mixture of ethanol 1C2H5OH2 and paraffin, which has an average formula of C24H50. What mass of C2H5OH should be added to 620 kg of the paraffin to produce 8 torr of ethanol vapor pressure at 35 C? The vapor pressure of pure et

Chapter: Problem: 13.100

Chemistry: The Central Science 13
A solution contains 0.115 mol H2O and an unknown number of moles of sodium chloride. The vapor pressure of the solution at 30 C is 25.7 torr. The vapor pressure of pure water at this temperature is 31.8 torr. Calculate the number of grams of sodium chloride in the solution. (Hint: Remember that sodiu

Chapter: Problem: 13.101

Chemistry: The Central Science 13
Two beakers are placed in a sealed box at 25 C. One beaker contains 30.0 mL of a 0.050 M aqueous solution of a nonvolatile nonelectrolyte. The other beaker contains 30.0 mL of a 0.035 M aqueous solution of NaCl. The water vapor from the two solutions reaches equilibrium. (a) In which beaker does the

Chapter: Problem: 13.102

Chemistry: The Central Science 13
A car owner who knows no chemistry has to put antifreeze in his cars radiator. The instructions recommend a mixture of 30% ethylene glycol and 70% water. Thinking he will improve his protection he uses pure ethylene glycol, which is a liquid at room temperature. He is saddened to find that the soluti

Chapter: Problem: 13.103

Chemistry: The Central Science 13
Calculate the freezing point of a 0.100 m aqueous solution of K2SO4, (a) ignoring interionic attractions, and (b) taking interionic attractions into consideration by using the vant Hoff factor (Table 13.4).

Chapter: Problem: 13.104

Chemistry: The Central Science 13
Carbon disulfide 1CS22 boils at 46.30 C and has a density of 1.261 g>mL. (a) When 0.250 mol of a nondissociating solute is dissolved in 400.0 mL of CS2, the solution boils at 47.46 C. What is the molal boiling-point-elevation constant for CS2? (b) When 5.39 g of a nondissociating unknown is dissolved

Chapter: Problem: 13.105

Chemistry: The Central Science 13
A lithium salt used in lubricating grease has the formula LiCnH2n + 1O2. The salt is soluble in water to the extent of 0.036 g per 100 g of water at 25 C. The osmotic pressure of this solution is found to be 57.1 torr. Assuming that molality and molarity in such a dilute solution are the same and tha

Chapter: Problem: 13.106

Chemistry: The Central Science 13
Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 C, and their solubilities in water at 25 C and 1 atm fluorocarbon pressure are given as mass percentages. (a) For each fluorocarb

Chapter: Problem: 13.107

Chemistry: The Central Science 13
At ordinary body temperature 137 C2, the solubility of N2 in water at ordinary atmospheric pressure (1.0 atm) is 0.015 g>L. Air is approximately 78 mol % N2. (a) Calculate the number of moles of N2 dissolved per liter of blood, assuming blood is a simple aqueous solution. (b) At a depth of 100 ft in

Chapter: Problem: 13.108

Chemistry: The Central Science 13
Consider the following values for enthalpy of vaporization 1kJ>mol2 of several organic substances: CH3C H 30.4 O Acetaldehyde H2C CH2 28.5 O Ethylene oxide CH3CCH3 32.0 O Acetone H2C CH2 CH2 24.7 Cyclopropane (a) Account for the variations in heats of vaporization for these substances, considering th

Chapter: Problem: 13.109

Chemistry: The Central Science 13
A textbook on chemical thermodynamics states, The heat of solution represents the difference between the lattice energy of the crystalline solid and the solvation energy of the gaseous ions. (a) Draw a simple energy diagram to illustrate this statement. (b) A salt such as NaBr is insoluble in most po

Chapter: Problem: 13.110a

Chemistry: The Central Science 13
(a) A sample of hydrogen gas is generated in a closed container by reacting 2.050 g of zinc metal with 15.0 mL of 1.00 M sulfuric acid. Write the balanced equation for the reaction, and calculate the number of moles of hydrogen formed, assuming that the reaction is complete.

Chapter: Problem: 13.110b

Chemistry: The Central Science 13
(b) The volume over the solution in the container is 122 mL. Calculate the partial pressure of the hydrogen gas in this volume at 25 C, ignoring any solubility of the gas in the solution. (c) The Henrys law constant for hydrogen in water at 25 C is 7.8 * 10-4 mol>L@atm. Estimate the number of moles o

Chapter: Problem: 13.111

Chemistry: The Central Science 13
The following table presents the solubilities of several gases in water at 25 C under a total pressure of gas and water vapor of 1 atm. (a) What volume of CH41g2 under standard conditions of temperature and pressure is contained in 4.0 L of a saturated solution at 25 C? (b) Explain the variation in s

Chapter: Problem: 13.112

Chemistry: The Central Science 13
A small cube of lithium 1density = 0.535 g/cm3 2 measuring 1.0 mm on each edge is added to 0.500 L of water. The following reaction occurs: 2 Li1s2 + 2 H2O1l2 2 LiOH1aq2 + H21g2 What is the freezing point of the resultant solution, assuming that the reaction goes to completion?

Chapter: Problem: 13.113

Chemistry: The Central Science 13
At 35 C the vapor pressure of acetone, 1CH322CO, is 360 torr, and that of chloroform, CHCl3, is 300 torr. Acetone and chloroform can form very weak hydrogen bonds between one another; the chlorines on the carbon give the carbon a sufficient partial positive charge to enable this behavior: CH3 CH3 C H

Chapter: Problem: 13.114

Chemistry: The Central Science 13
Compounds like sodium stearate, called surfactants in general, can form structures known as micelles in water, once the solution concentration reaches the value known as the critical micelle concentration (cmc). Micelles contain dozens to hundreds of molecules. The cmc depends on the substance, the s

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