Chemistry 10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
1 Chemical Foundations 2 Atoms, Molecules, And Ions 3 Stoichiometry 4 Types Of Chemical Reactions And Solution Stoichiometry 5 Gases 6 Thermochemistry 7 Atomic Structure And Periodicity 8 Bonding: General Concepts 9 Covalent Bonding: Orbitals 10 Liquids And Solids 11 Properties Of Solutions 12 Chemical Kinetics 13 Chemical Equilibrium 14 Acids And Bases 15 Acid-base Equilibria 16 Solubility And Complex Ion Equilibria 17 Spontaneity, Entropy, And Free Energy 18 Electrochemistry 19 The Nucleus: A Chemist's View 20 The Representative Elements 21 Transition Metals And Coordination Chemistry 22 Organic And Biological Molecules Chapter11: Properties Of Solutions
Chapter Questions Section: Chapter Questions
Problem 1RQ Problem 2RQ: Using KF as an example, write equations that refer to Hsoln and Hhyd Lattice energy was defined in... Problem 3RQ Problem 4RQ Problem 5RQ: Define the terms in Raoults law. Figure 10-9 illustrates the net transfer of water molecules from... Problem 6RQ: In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal... Problem 7RQ: Vapor-pressure lowering is a colligative property, as are freezing-point depression and... Problem 8RQ: What is osmotic pressure? How is osmotic pressure calculated? Molarity units are used in the osmotic... Problem 9RQ: Distinguish between a strong electrolyte, a weak electrolyte, and a nonelectrolyte. How can... Problem 10RQ Problem 1ALQ Problem 2ALQ: Once again, consider Fig. 10-9. Suppose instead of having a nonvolatile solute in the solvent in one... Problem 3ALQ Problem 4ALQ Problem 5ALQ: You have read that adding a solute to a solvent can both increase the boiling point and decrease the... Problem 6ALQ: You drop an ice cube (made from pure water) into a saltwater solution at 0C. Explain what happens... Problem 7ALQ: Using the phase diagram for water and Raoults law, explain why salt is spread on the roads in winter... Problem 8ALQ: You and your friend are each drinking cola from separate 2-L bottles. Both colas are equally... Problem 9ALQ Problem 10ALQ Problem 11ALQ: If a solution shows positive deviations from Raoults law, would you expect the solution to have a... Problem 12ALQ Problem 13SR: Rubbing alcohol contains 585 g isopropanol (C3H7OH) per liter (aqueous solution). Calculate the... Problem 14SR Problem 15SR Problem 16SR Problem 17SR: Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of... Problem 18SR: Write equations showing the ions present after the following strong electrolytes are dissolved in... Problem 19Q: Rationalize the temperature dependence of the solubility of a gas in water in terms of the kinetic... Problem 20Q: The weak electrolyte NH3(g) does not obey Henrys law. Why? O2(g) obeys Henrys law in water but not... Problem 21Q: The two beakers in the sealed container illustrated below contain pure water and an aqueous solution... Problem 22Q: The following plot shows the vapor pressure of various solutions of components A and B at some... Problem 23Q: When pure methanol is mixed with water, the resulting solution feels warm. Would you expect this... Problem 24Q Problem 25Q: For an acid or a base, when is the normality of a solution equal to the molarity of the solution and... Problem 26Q Problem 27Q Problem 28Q Problem 29Q Problem 30Q: Table sugar (C12H22O11) or urea [(NH2)2CO] can be used by road crews to melt ice on roads, but... Problem 31Q: If two different aqueous solutions of proteins have the same boiling point, what other physical... Problem 32Q: An extremely important application of dialysis is the use of artificial kidney machines to purify... Problem 33Q: Explain the terms isotonic solution, crenation, and hemolysis. Problem 34Q Problem 35E Problem 36E: A typical IV used in hospitals is dextrose 5% in water (called D5W). This solution is injected into... Problem 37E Problem 38E Problem 39E: Common commercial acids and bases are aqueous solutions with the following properties: Density... Problem 40E: In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would... Problem 41E Problem 42E Problem 43E Problem 44E: Calculate the molarity and mole fraction of acetone in a 1.00-m solution of acetone (CH3COCH3) in... Problem 45E Problem 46E Problem 47E Problem 48E: a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium... Problem 49E: Although Al(OH)3 is insoluble in water, NaOH is very soluble. Explain in terms of lattice energies. Problem 50E Problem 51E Problem 52E Problem 53E: For each of the following pairs, predict which substance would be more soluble in water. a. or b. or... Problem 54E: Which ion in each of the following pairs would you expect to be more strongly hydrated? Why? a. Na+... Problem 55E: Rationalize the trend in water solubility for the following simple alcohols: Alcohol Solubility... Problem 56E: In flushing and cleaning columns used in liquid chromatography to remove adsorbed contaminants, a... Problem 57E: The solubility of nitrogen in water is 8.21 104 mol/L at 0C when the N2 pressure above water is... Problem 58E: Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25C. The Henrys... Problem 59E: The vapor pressure of a solution containing 53.6 g glycerin (C3H8O3) in 133.7 g ethanol (C2H5OH) is... Problem 60E: An aqueous solution containing glucose has a vapor pressure of 19.6 torr at 25C. What would be the... Problem 61E: The normal boiling point of diethyl ether is 34.5C. A solution containing a nonvolatile solute... Problem 62E: At a certain temperature, the vapor pressure of pure benzene (C6H6) is 0.930 atm. A solution was... Problem 63E Problem 64E: A solution is prepared by mixing 0.0300 mole of CH2Cl2 and 0.0500 mole of CH2Br2 at 25C. Assuming... Problem 65E: What is the composition of a methanol (CH3OH)-propanol (CH3CH2CH2OH) solution that has a vapor... Problem 66E: Benzene and toluene form an ideal solution. Consider a solution of benzene and toluene prepared at... Problem 67E: Which of the following will have the lowest total vapor pressure at 25C? a. pure water (vapor... Problem 68E Problem 69E: Match the vapor pressure diagrams with the solute-solvent combinations and explain your answers. a.... Problem 70E: The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various... Problem 71E: A solution is prepared by dissolving 27.0 g urea, (NH2)CO, in 150.0 g water. Calculate the boiling... Problem 72E: A 2.00-g sample of a large biomolecule was dissolved in 15.0 g carbon tetrachloride. The boiling... Problem 73E: What mass of glycerin (C3H8O3), a nonelectrolyte, must be dissolved in 200.0 g water to give a... Problem 74E: The freezing point of 1-butanol is 25.50C and Kf is 9.1C kg/mol. Usually t-butanol absorbs water on... Problem 75E Problem 76E: What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 15.0 L water to produce... Problem 77E: Reserpine is a natural product isolated from the roots of the shrub Rauwolfia serpenlina. It was... Problem 78E: A solution contains 3.75 g of a nonvolatile pure hydrocarbon in 95 g acetone. The boiling points of... Problem 79E: a. Calculate the freezing-point depression and osmotic pressure at 25C of an aqueous solution... Problem 80E: Erythrocytes are red blood cells containing hemoglobin. In a saline solution they shrivel when the... Problem 81E Problem 82E Problem 83E Problem 84E Problem 85E: Consider the following solutions: 0.010 m Na3PO4 in water 0.020 m CaBr2 in water 0.020 m KCl in... Problem 86E: From the following: pure water solution of C12H22O11 (m = 0.01) in water solution of NaCl (m = 0.01)... Problem 87E Problem 88E Problem 89E Problem 90E: Consider the following representations of an ionic solute in water. Which flask contains MgSO4, and... Problem 91E Problem 92E Problem 93E: Use the following data for three aqueous solutions of CaCl2 to calculate the apparent value of the... Problem 94E: The freezing-point depression of a 0.091-m solution of CsCl is 0.320C. The freezing-point depression... Problem 95E Problem 96E: A 0.500-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This... Problem 97AE: The solubility of benzoic acid (HC7H5O2), is 0.34 g/100 mL in water at 25C and is 10.0 g/100 mL in... Problem 99AE Problem 100AE Problem 101AE Problem 102AE: In Exercise 96 in Chapter 8, the pressure of CO2 in a bottle of sparkling wine was calculated... Problem 103AE: Explain the following on the basis of the behavior of atoms and/or ions. a. Cooking with water is... Problem 104AE: The term proof is defined as twice the percent by volume of pure ethanol in solution. Thus, a... Problem 105AE Problem 106AE Problem 107AE: A solution is made by mixing 50.0 g acetone (CH3COCH3) and 50.0 g methanol (CH3OH). What is the... Problem 108AE Problem 109AE: Thyroxine, an important hormone that controls the rate of metabolism in the body, can be isolated... Problem 110AE Problem 111AE: An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound... Problem 112AE Problem 113AE Problem 115AE Problem 117AE: Patients undergoing an upper gastrointestinal tract laboratory test are typically given an X-ray... Problem 118CWP Problem 119CWP: The lattice energy of NaCl is 786 kJ/mol, and the enthalpy of hydration of 1 mole of gaseous Na+ and... Problem 120CWP: For each of the following pairs, predict which substance is more soluble in water. a. CH3NH2 or NH3... Problem 121CWP: The normal boiling point of methanol is 64.7C. A solution containing a nonvolatile solute dissolved... Problem 122CWP: A solution is prepared by mixing 1.000 mole of methanol (CH3OH) and 3.18 moles of propanol... Problem 123CWP Problem 124CWP: A 4.7 102 mg sample of a protein is dissolved in water to make 0.25 mL of solution. The osmotic... Problem 125CWP: A solid consists of a mixture of NaNO3 and Mg(NO3)2. When 6.50 g of the solid is dissolved in 50.0 g... Problem 126CP: The vapor pressure of pure benzene is 750.0 torr and the vapor pressure of toluene is 300.0 torr at... Problem 127CP Problem 128CP: Plants that thrive in salt water must have internal solutions (inside the plant cells) that are... Problem 129CP: You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The... Problem 130CP Problem 131CP: The vapor in equilibrium with a pentane-hexane solution at 25C has a mole fraction of pentane equal... Problem 132CP: A forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar... Problem 133CP: A 1.60-g sample of a mixture of naphthalene (C10H8) and anthracene (C14H10) is dissolved in 20.0 g... Problem 134CP Problem 135CP Problem 136CP: You have a solution of two volatile liquids, A and B (assume ideal behavior). Pure liquid A has a... Problem 137CP: In some regions of the southwest United States, the water is very hard. For example, in Las Cruces,... Problem 138CP: Specifications for lactated Ringers solution, which is used for intravenous (IV) injections, are as... Problem 140IP: Creatinine, C4H7N3O, is a by-product of muscle metabolism, and creatinine levels in the body are... Problem 141IP: An aqueous solution containing 0.250 mole of Q, a strong electrolyte, in 5.00 102 g water freezes... Problem 142IP: Anthraquinone contains only carbon, hydrogen, and oxygen. When 4.80 mg anthraquinone is burned, 14.2... Problem 105AE
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help find initial concentration/rate reaction of data thank you includ sig figs.
Transcribed Image Text: Trial 1
Concentration of iodide solution (mM)
100.0
Concentration of thiosulfate solution (mM)
31.5
Concentration of hydrogen peroxide solution (mM)
176.5
Temperature of iodide solution (°C)
25.0
Volume of iodide solution (1") used (mL)
10.0
Volume of thiosulfate solution (S203²) used (mL)
1.0
Volume of DI water used (mL)
2.5
Volume of hydrogen peroxide solution (H202) used (mL)
7.5
Time (s)
17.8
change of color
Observations
Initial concentration of iodide in reaction (mM)
Initial concentration of thiosulfate in reaction (mM)
Initial concentration of hydrogen peroxide in reaction (mM)
Initial Rate (mM/s)
Definition Definition Study of the speed of chemical reactions and other factors that affect the rate of reaction. It also extends toward the mechanism involved in the reaction.
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