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All Textbook Solutions for Introductory Chemistry: A Foundation

92QAP What volume does a mixture of 14.2gof He and 21.6gof H2Occupy at 28Cand 0.985atm?94QAP 95QAP The volume of a gas-filled balloon is 50.0 L at 20. °C and 742 torr. What volume will it occupy at STP?97QAP 98QAP Consider the following unbalanced chemical equation for the combination reaction of sodium metal and chlorine gas: msp;Na(s)+Cl2(g)NaCl(s) at volume of chlorine gas. measured at STP, is necessary for the complete reaction of 4.81gof sodium metal?100QAP 101QAP 102QAP 103AP 104AP 105AP onsider the flasks in the following diagrams. mg src=Images/HTML_99425-13-106AP_image001.jpg alt="" align="top"/> suming the connecting tube has negligible volume, draw what each diagram will look like after the stopcock between the two flasks is opened. Also, solve for the final pressure in each case. in terms of the original pressure. Assume temperature is constant.107AP helium tank contains 25.2Lof helium m 8.40atm pressure. Determine how many 1.50Lballoons at 755mmHgcan be inflated with the gas in the tank, assuming that the tank will also have to contain He at 755mmHgafter the balloons are filled (that is, it is not possible to empty the tank completely). The temperature is 25Cin all cases.109AP 110AP 111AP 112AP 113AP 114AP 115AP 116AP 117AP 118AP 119AP 120AP 121AP 122AP 123AP 124AP 125AP 126AP f 5.l2gof oxygen gas occupies a volume of 6.21Lat a certain temperature and pressure, what volume will 25.0gof oxygen gas occupy under the same conditions?128AP 129AP 130AP 131AP Suppose three 100.-L tanks are to be filled separately with the gases CH4. N2, and CO?. respectively. What mass of each gas is needed to produce a pressure of 120. atm in its tank at 27 °C?t what temperature does 4.00gof helium gas have a pressure of 1.00atm in a msp;22.4Lvessel?134AP f 3.20gof nitrogen gas occupies a volume of 1.71Lat 0Cand a pressure of 1.50atm, what would the volume become if 8.80gof nitrogen gas were added at constant conditions of temperature and pressure?136AP 137AP A mixture at 33 °C contains H2at 325 torr. N;at 475 tore and O2at 650. torr. What is the total pressure of the gases in the system? Which gas contains the greatest number of moles?139AP 140AP Consider the following unbalanced chemical equation: 6H12O6(s) + O2(g) -> CO,(g) + H2O(g) What volume of oxygen gas. measured at 28 °C and 0.976 atm. is needed to react with 5.00 g of C*H|2O6? What volume of each product is produced under the same conditions?Consider the following unbalanced chemical equation: ^Sfr) + O2(g) —? Cu2O(s) + SO2(g) What volume of oxygen gas, measured at 27.5 °C and 0.998 atm. is required to react with 25 g of copper!I) sulfide? What volume of sulfur dioxide gas is produced under the same conditions?143AP 144AP 145AP 146AP 147AP 148AP 149AP 150AP omplete the following table for an ideal gas. mg src=Images/HTML_99425-13-150CP_image001.jpg alt="" align="top"/>152CP 153CP certain flexible weather balloon contains helium gas at a volume of 855L. Initially, the balloon is at sea level where the temperature is 25 °C and the barometric pressure is 730torr. The balloon men rises to an altitude of 6000 ft, where the pressure is 605torr and the temperature is 15C. What is the change in volume of the balloon as it ascends from sea level to 6000ft?155CP 156CP 157CP 158CP trong>Exercise 14.1 Calculate the total energy required to melt 15gof ice at 0C, heat the water to 100C, and vaporize it to steam at 100C.1CT trong>Exercise 14.2 Name the type of crystalline solid formed by each of the following substances: sulfur trioxide barium oxide gold ou seal a container half-filled with water. Which best describes what occurs in the container? Water evaporates until the air becomes saturated with water vapor; at this point, no more water evaporates. Water evaporates until the air becomes overly saturated (supersaturated) with water, and most of this water recondenses; this cycle continues until a certain amount of water vapor is present, and then the cycle ceases. The water does not evaporate because the container sealed. Water evaporates, and thou water evaporates and recondenses simultaneously and continuously. The water evaporates until it is eventually all in vapor form. stify your choice, and for choices you did not pick, explain what is wrong with them.xplain the following: You add 100mLof water to a 500mLround-bottomed flask and heat the water until it is boiling. You remove the heat and stopper me flask, and the boiling stops. You then run cool water over the neck of the flask, and me boiling begins again. It seems as though you are boiling water by cooling it.3ALQ 4ALQ 5ALQ 6ALQ 7ALQ ow do the following physical properties depend on the strength of intermolecular forces? Explain. melting point . baiting point . vapor pressure ook at Fig. 14.2. Why doesn't temperature increase continuously ever time? That is, why does the temperature stay constanl for periods of time?10ALQ 11ALQ 12ALQ 13ALQ 14ALQ 15ALQ True or false? Methane (CH4) is more likely In form stronger hydrogen bonding than is water because each methane molecule has twice as many hydrogen alums. Provide a concise explanation of hydrogen bonding to go with your answer.17ALQ 18ALQ 19ALQ Which would you predict should be larger for a given substance: HvaporHfus? Explain why.21ALQ 22ALQ 23ALQ ases have (higher/lower) densities than liquids or solids.2QAP 3QAP he enthalpy (H)of vaporization of water is about seven times larger than water’s enthalpy fusion(41kJ/molvs.6kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous states of water?5QAP 6QAP 7QAP 8QAP 9QAP 10QAP 11QAP What does the molar heat of fusion of a substance represent?The following data have ban collected for substance X. Construct. a heating curve for substance X. (The drawing does not need to be absolutely to scale, but it should clearly show relative differences.) rmal melting point :math>15C lar heat of fusion :math>2.5KJ/mol rmal boiling point :math>134C lar heat of vaporization :math>55.3KJ/mol The molar heat of fusion of aluminum metal is 10.79Kj/mol, whereas its heat of vaporization is 293.4Kj/mol. Why is the heat of fusion of aluminum so much smaller than the ham of vaporization? What quantity of heat would be required to vaporize 1.00gof aluminum at its normal boiling point? What quantity of ham would he evolved if 5.00gof liquid aluminum freezes at its normal freezing point? What quantity of heat would be required to melt 0.105mole of aluminum at its normal melting point?15QAP 16QAP The molar heats of fusion and vaporization for water are 6.02kJ/moland 40.6kJ/molrespectively, and The specific heat capacity of liquid water is 4.18J/gC. What quantity of heat energy is required to melt 25.0gof ice at 0C? What quantity of heat is required for vaporize 37.5gof liquid water at 100C? What quantity of heat is required to warm 55.2gof liquid water from 0Cto 100C?It requires 113Jto melt 1.00gof sodium metal at its normal melting point of 98C. Calculate the molar hear of fusion of sodium Consider the iodine monochloride molecule, ICI. Because chlorine is more electronegative than iodine, this molecule is a dipole. How would you expect iodine monochloride molecules in the gaseous state to orient themselves with respect to each other as the sample is cooled and the molecules begin to aggregate? Sketch the orientation you would expect.20QAP 21QAP 22QAP 23QAP 24QAP What type of intermolecular forces is active in the liquid state of each of the following substances? msp;a.Neb.COC.CH3OHd.Cl2 26QAP 27QAP The heats of fusion of three substances are listed below. Explain the trend this list reflects. msp;HI2.87kJ/molHBr2.41kJ/molHCl1.99kJ/mol When dry ammonia gas (NH3)is bubbled into a msp;125mLsample of water, the volume of the sample (initially, at least) decreases slightly. Suggest a reason for this.30QAP 31QAP If you've ever opened a bottle of rubbing alcohol or other solvent on a warm day, you may have heard a little “whoosh” as the vapor that had built up above the liquid escapes. Describe on a microscopic basis how a vapor pressure builds up in a closed container above a liquid. What processes in the container give rise to this phenomenon?33QAP 34QAP Which substance in each pair would be expected to have a lower boiling point? Explain your reasoning. msp;a.CH3OHorCH3CH2CH2OHb.CH3CH30rCH3CH2OHc.H2OorCH4 Which substance in each pair would be expected to be more volatile at a particular temperature? Explain your reasoning. mg src=Images/HTML_99425-14-36QAP_image001.jpg alt="" align="top"/>37QAP Two molecules that contain the same number of each kind of atom but [hat have different molecular structures are said to he isomers of each other. For example, both ethyl alcohol and dimethyl ether (shown below} have the formula C2H6Oand are isomers; Based on considerations of intermolecular forces. which substance would you expect to be more volatile? Which would you expect 10have the higher boiling point? Explain. methyl ether hyl alcohol msp;CH3OCH3CH3CH2OH 39QAP 40QAP How do ionic solids differ in structure from molecular solids? What are the fundamental panicles in each? Give two examples of each type of solid and indicate the individual particles that make up the solids in each of your examples.A common prank on college campuses is to switch the salt and sugar on dining hall tables. which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties because one is a molecular solid and the other is an ionic solid. How do the properties differ and why?43QAP What types of forces exist between the individual particles in an ionic solid? Are these threes relatively strong or relatively weak?45QAP 46QAP 47QAP 48QAP 49QAP 50QAP 51AP 52AP 53AP 54AP 55AP 56AP 57AP 58AP 59AP 60AP Given the densities and conditions of ice, liquid water, and steam listed in Table 14.1, calculate the volume of 1.0gof water under each of these circumstances.62AP Which of the substances in each of the following sets would be Expected to have the highest boiling point? Explain why. msp;a.Ga,KBr,O2b.Hg,NaCl,Hec.H2,O2,H2O 64AP 65AP 66AP 67AP 68AP Describe, on both a microscopic and a macroscopic basis, what happens to a sample of water as it is cooled from room temperture to 50Cbelow its normal freezing point.Cake mixes and other packaged foods that require cooking often contain special directions for use at high elevations. Typically these directions indicate that the food should be cooked longer above 5000ft. Explain why it takes longer to cook something at higher elevations.71AP 72AP The molar heat of vaporization of carbon disulfide, CS2, is 28.4kJ/molat its normal boiling point of 46C. How much energy (heat) is required to vaporize 1.0gof CS2at46C? How much heat is evolved when 50.gofCS2is condensed from the vapor to the liquid form at 46 °C?74AP 75AP 76AP 77AP 78AP 79AP 80AP 81AP 82AP 83AP 84AP Describe in detail the microscopic processes that take place when a liquid boils. What kind of forces must be overcome? Are any chemical bonds broken during these processes?86AP 87AP 88AP 89AP Describe, on a microscopic basis, the processes of evaporation and condensation. Which process requires an input of energy? Why?91AP 92AP Which of the following compound(s) exhibit only London dispersion intermolecular forces? Which compound(s) exhibit hydrogen-bonding forces? Considering only the compounds without hydrogen-bonding interactions. which compounds have dipole-dipole intermolecular forces? msp;a.SF4d.HF msp;b.CO2e.IC15 msp;c.CH3CH2OHf.XeF4 Which of the following statements about intermolecular forces is(are) true? London dispersion forces are the only type of intermolecular force that nonpnlar molecules exhibit. Molecules that have only London dispersion forms will always be gases at room temperature (25C). The hydrogen-bonding forces in NH3are stronger than those in H2O. The molecules in SO2(g)exhibit dipole-dipole intermolecular interactions. CH3CH2CH3has stronger London dispersion forces than does CH4.95CP 96CP 97CP Which of the following statements is(are) true? LiFwill have a higher vapor pressure at 25Cthan H2S. HFwill have a lower vapor pressure at -50 °C than HBr. Cl2will have a higher boiling point than Ar. HClis more soluble in water than in CCl4. MgOwill have a higher vapor pressure at 25Cthan CH3CH2OH.ercise 15.1 A 1 35-g sample of seawater is evaporated to dryness, leaving 4.73 g of solid residue (the salts formerly dissolved in the seawater). Calculate the mass percent of solute present in the original seawater.15.2SC ercise 15.3 Calculate the molarity of a solution prepared by dissolving I .00 g of ethanol. C2HOH. in enough water to give a final volume of 101 mL.ercise 15.4 Give the concentrations of the ions in each of the following solutions: 10 M Na2CO3 0 10 M Al2(SO4) 3 ercise 15.5 Calculate the number of moles of Cl ions in 1.75 L of 1.0 X 10 M AICl3.ercise 15.6 Formalin is an aqueous solution of formaldehyde, HCHO, used as a preservative for biologic specimens. How many grams of formaldehyde must be used to prepare 2.5 L of 12.3 M formalin?ercise 15.7 What volume of 12 M HCI must be taken to prepare 0.75 L of 0.25 M HCl?at if all ionic solids were soluble in water? How would this affect stoichiometry calculations for reactions in aqueous solution?Exercise 15.8 When aqueous solutions of Na2SO3 and Pb(NO3)2 are mixed, PbSO4 precipitates. Calculate the mass of PbSO4 formed when 1.25 L of 0.0500 M Pb(NO3)2 and 2.00 L of 0.0250 M NaSO4 are mixed.ercise 15.9 Calculate the volume of 0.10 M HNO3 needed to neutralize 125 mL of 0.050 M KOH.ercise 15.10 Calculate the normality of a solution containing 23.6 g of KOH in 755 mL of solution.15.11SC ou have a solution of table sail in water. What happens to the salt concentration (increases, decreases, or stays the same) as the solution boils? Draw pictures to explain your answer.onsider a sugar solution (solution A) with concentration x. You pour one-third of this solution into a beaker, and add an uivalent volume of water (solution B). What is the ratio of sugar in solutions A and B? Compare the volumes of solutions A and B. m>c. What is the ratio of the concentrations of sugar in solutions A and 13?You need to make 150.0 mL of a 0.10 M NaCI solution. You have solid NaCl, and your lab partner has a 2.5 M NaC1 solution. Explain how you each independently make the solution you need.ou have two solutions containing solute A. To determine which solution has the highest concentration of A in molarity, which of the following must you know? (There may be more than one answer.) the mass in grams of A in each solution the molar mass of A the volume of’ water added to each solution the total volume of the solution plain your answer.m>5. Which of the following do you need to know to calculate the molarity of a salt solution? (There may be more than one answer.) the mass of salt added the molar mass of the salt the volume of water added the total volume of the solution plain your answer.onsider separate aqueous solutions of HCI and H2S04 with the same concentrations in terms of molarity. You wish to neutralize au aqueous solution of’ NaOH. For which acid solution would you need to add more volume (in mL) to neutralize the base? The HCI solution. The H2SO4 solution. You need to know the acid concentrations to answer this question. You need to know the volume and concentration of’ the NaOH solution to answer this question. c and d plain your answer.7ALQ an one solution have a greater concentration than another in terms of weight percent, but a lower concentration in terms of molarity? Explain.9ALQ You have equal masses of different solutes dissolved in equal volumes of solution. Which of the solutes listed below would make the solution with the highest concentration measured in molarity? Defend your answer. CI, MgSO4, LiF, KNO3 Which of the following solutions contains the greatest number of particles? Support your answer. .0 mL of 0 10 M sodium chloride .0 mL of 0.10 M calcium chloride .0 mL of 0.10 M iron(III) chloride .0 mL of 0.10 M potassium bromide .0 mL of 0.10 M sucrose (table sugar)As with all quantitative problems in chemistry, make sure not to get “lost in the math.” In particular, work on visualizing solutions at a molecular level. For example, consider the following. U have two separate beakers with aqueous solutions, one with 4 units of potassium sulfate and one with 3 “units” of barium nitrate. Draw molecular-level diagrams of both solutions. Draw a molecular-level diagram of the mixture of the two solutions before a reaction has taken place. Draw a molecular-level diagram of the product and solution formed after the reaction has taken place.13ALQ 14ALQ solution is a homogeneous mixture. Can you give an example of a gaseous homogeneous mixture? A liquid homogeneous mixture? A solid homogeneous mixture?ow do the properties of a nonhomogeneous (heterogeneous) mixture differ from those of a solution? Give two examples of nonhomogeneous mixtures.3QAP 4QAP n Chapter 14. you learned that the bonding forces in ionic solids such as NaCl are very strong, yet many ionic solids dissolve readily in water. Explain.n oil spill spreads out on the surface of water, rather than dissolving in the water. Explain why.. The “Chemistry in Focus” segment Water, Water Everywhere, Bu . . . discusses the desalinization of ocean water. Explain why many sails are soluble in water. Include molecular-level diagrams in your answer.8QAP 9QAP 10QAP A solution is a homogeneous mixture and, unlike a compound, has composition.12QAP How do we define the mass percent composition of a solution? Give an example of a solution, and explain the relative amounts of solute and solvent present in the solution in terms of the mass percent composition.14QAP Calculate the percent by mass of solute in each of the following solutions. 14 g of potassium chloride dissolved in 12.5 g of water 14 g of potassium chloride dissolved in 25.0 g of water 14 g of potassium chloride dissolved in 37.5 g of water 14 g of potassium chloride dissolved in 50.0 g of water Calculate the percent by mass of solute in each of the following solutions. 5.00 g of calcium chloride dissolved in 95.0 g of water 1.00 g of calcium chloride dissolved in 19.0 g of water 15.0 g of calcium chloride dissolved in 285 g of water 2.00 mg of calcium chloride dissolved in 0.0380 g of water 17QAP 18QAP A sample of an iron alloy contains 92.1 g Fe. 2.59 g C. and Cr. Calculate the percent by mass of each component present in the alloy sample.Consider the iron alloy described in Question 19. Suppose it is desired to prepare 1.00 kg of this alloy, what mass of each component would be necessary?An aqueous solution is to be prepared that will be 7.51% by mass ammonium nitrate. What mass of NH4NO3 and what mass of water will be needed to prepare 1.25 kg of the solution?22QAP A solution is to be prepared that will be 4.50% by mass calcium chloride. To prepare 175 g of the solution, what mass of calcium chloride will be needed?24QAP 25QAP Hydrogen peroxide solutions sold in drugstores as an antiseptic typically contain 3.0% of the active ingredient, Hydrogen peroxide decomposes into water and oxygen gas when applied to a wound according to the balanced chemical equation 2H2O2(aq)2H2O(l)+O2(g) What approximate mass of hydrogen peroxide solution would be needed to produce 1.00 g of oxygen gas?27QAP A solvent sold for use in the laboratory contains 0.95% of a stabilizing agent that prevents the solvent from reacting with the air. What mass of the stabilizing agent is present in 1.00 kg of the solvent?29QAP 30QAP What is a standard solution? Describe the steps involved in preparing a standard solution.32QAP 33. For each of the following solutions, the number of moles of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 0.521 mol NaCl; 125 mL b. 0.521 mol NaCl; 250. mL c. 0.521 mol NaCl; 500. mL d. 0.521 molNaCl; 1.00 L 34. For each of the following solutions, the number of moles of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 0.754 mol KNO; 225 mL b. 0.0105 in of CaCl; 10.2 mL c. 3.15 mol NaCl; 5.00 L d. 0.499 mol NaBr; 100. mL 35. For each of the following solutions, the mass of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 3.51 g NaCl: 25 mL c. 3.51 g NaCl: 75 mL b. 3.51 g NaCl; 50. mL d. 3.51 g NaCl; l.00 L 36QAP 37. A laboratory assistant needs to prepare 225 mL of 0.150 M CaCl2 solution. How many grams of calcium chloride will she need?38QAP 39. Standard solutions of calcium ion used to test for water hardness are prepared by dissolving pure calcium carbonate. CaCO3, in dilute hydrochloric acid. A 1.745-g sample of CaCO3 is placed in a 250.O-mL volumetric flask and dissolved in HCI. Then the solution is diluted to the calibration mark of the volumetric flask. Calculate the resulting molarity of calcium ion.40QAP 41. If 42.5 g of NaOH is dissolved in water and diluted to a final volume of 225 mL, calculate the molanty of the solution.42. Standard silver nitrate solutions are used in the analysis of samples containing chloride ion. How many grams of silver nitrate are needed to prepare 250. mL of a 0.100 M AgNO3 solution?43QAP 44QAP 45QAP 46QAP 47QAP 48. What mass of solute is present in 225 mL of 0.355 M KBr solution?49QAP 50QAP 51QAP Strong acid solutions may have their concentration determined by reaction with measured quantities of standard sodium carbonate solution. What mass of Na2CO3 is needed to prepare 250. mL of 0.0500 M Na2CO, solution?53QAP 54QAP 55QAP 56QAP 57QAP 58QAP 59QAP 60. Suppose 325 in L of 0.150 M NaOH is needed for your experiment. How would you prepare this if all that is available is a 1.01 M NaOH solution?61. How much water must be added w 500. mL of 0.200 M HCI to produce a 0.150 M solution? (Assume that the volumes are additive.)An experiment calls for 100. mL of 1.25 M HC1. All that is available in the lab is a bottle of concentrated HC1, whose label indicates that it is 12.1 M. How much of the concentrated HC1 would be needed to prepare the desired solution?63QAP 64. Generally only the carbonates of the Group I elements and the ammonium ion are soluble in water: most other carbonates are insoluble. How many milliliters of 0.1 25 M sodium carbonate solution would be needed to precipitate the calcium ion from 37.2 mL of 0.105 M CaC12 solution? Na2CO3(aq)+CaCl2(aq)CaCO3(s)+2NaCI(aq)65. Many metal ions are precipitated from solution by the sulfide ion. As an example, consider treating a solution of copper(II) sulfate with sodium sulfide solution: CuSO4(aq)+Na2S(aq)CuS(s)+Na2SO4(aq) What Volume of 0.105 M Na2S solution would be required to precipitate all of the copper( II) ion from 27.5 mL of 0.121 M CuSO4solution?66. Calcium oxalate, CaCO4, is very insoluble in water. What mass of sodium oxalate, Na2C2O4, is required to precipitate the calcium ion from 37.5 mL of 0.104 M CaCl2 solution?67. When aqueous solutions of lead(II) ion are treated with potassium chromate solution, a bright yellow precipitate of lead(II) chromate, PbCrO4, forms. How many grains of lead chromate form when a 1.00-g sample of Pb(NO3)2 is added to 25.0 mL of 1 .00 M K2CrO4 solution?68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?69. What volume of 0.502 M NaOH solution would be required to neutralize 27.2 mL of 0.491 M HNO3 solution?70. What volume of a 0.500 M NaOH solution would be required to neutralize 40.0 mL of a 0.400 M H2SO4 solution?71. A sample of sodium hydrogen carbonate solid weighing 0.1015 g requires 47.21 ml. of a hydrochloric acid solution to react completely. HCl(aq)+NaHCO3(s)NaCl(aq)+H2O(l)+CO2(g) Calculate the molarity of the hydrochloric acid solution.72. The total acidity in water samples can be determined by neutralization with standard sodium hydroxide solution. What is the total concentration of hydrogen ion, H+, present in a water sample if 100. mL of the sample requires 7.2 mL of 2.5103M NaOH to be neutralized?73QAP 74QAP 75QAP 76QAP 77. Explain why the equivalent weight of H2SO4 is half the molar mass of this substance. How many hydrogen ions does each H2SO4 molecule produce when reacting with an excess of OH ions?78QAP 79QAP 80QAP 81QAP 82QAP 83QAP

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