Chemistry 9th Edition
ISBN: 9781133611097
Author: Steven S. Zumdahl
Publisher: Steven S. Zumdahl
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 11SR: Rubbing alcohol contains 585 g isopropanol (C3H7OH) per liter (aqueous solution). Calculate the... Problem 12SR Problem 13SR Problem 14SR Problem 15SR: Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of... Problem 16SR: Write equations showing the ions present after the following strong electrolytes are dissolved in... Problem 17Q: Rationalize the temperature dependence of the solubility of a gas in water in terms of the kinetic... Problem 18Q: The weak electrolyte NH3(g) does not obey Henrys law. Why? O2(g) obeys Henrys law in water but not... Problem 19Q: The two beakers in the sealed container illustrated below contain pure water and an aqueous solution... Problem 20Q: The following plot shows the vapor pressure of various solutions of components A and B at some... Problem 21Q: When pure methanol is mixed with water, the resulting solution feels warm. Would you expect this... Problem 22Q Problem 23Q: For an acid or a base, when is the normality of a solution equal to the molarity of the solution and... Problem 24Q Problem 25Q Problem 26Q Problem 27Q: Explain the terms isotonic solution, crenation, and hemolysis. Problem 28Q Problem 29E Problem 30E Problem 31E: Common commercial acids and bases are aqueous solutions with the following properties: Density... Problem 32E: In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would... Problem 33E Problem 34E Problem 35E Problem 36E: Calculate the molarity and mole fraction of acetone in a 1.00-m solution of acetone (CH3COCH3) in... Problem 37E Problem 38E Problem 39E Problem 40E: a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium... Problem 41E: Although Al(OH)3 is insoluble in water, NaOH is very soluble. Explain in terms of lattice energies. Problem 42E Problem 43E Problem 44E Problem 45E: For each of the following pairs, predict which substance would be more soluble in water. a. or b. or... Problem 46E: Which ion in each of the following pairs would you expect to be more strongly hydrated? Why? a. Na+... Problem 47E: Rationalize the trend in water solubility for the following simple alcohols: Alcohol Solubility... Problem 48E: In flushing and cleaning columns used in liquid chromatography to remove adsorbed contaminants, a... Problem 49E: The solubility of nitrogen in water is 8.21 104 mol/L at 0C when the N2 pressure above water is... Problem 50E: Calculate the solubility of O2 in water at a partial pressure of O2 of 120 torr at 25C. The Henrys... Problem 51E: Glycerin, C3H8O3, is a nonvolatile liquid. What is the vapor pressure of a solution made by adding... Problem 52E: The vapor pressure of a solution containing 53.6 g glycerin (C3H8O3) in 133.7 g ethanol (C2H5OH) is... Problem 53E: The normal boiling point of diethyl ether is 34.5C. A solution containing a nonvolatile solute... Problem 54E: At a certain temperature, the vapor pressure of pure benzene (C6H6) is 0.930 atm. A solution was... Problem 55E: A solution is made by dissolving 25.8 g urea (CH4N2O), a nonelectrolyte, in 275 g water. Calculate... Problem 56E: A solution of sodium chloride in water has a vapor pressure of 19.6 torr at 25C. What is the mole... Problem 57E Problem 58E: A solution is prepared by mixing 0.0300 mole of CH2Cl2 and 0.0500 mole of CH2Br2 at 25C. Assuming... Problem 59E: What is the composition of a methanol (CH3OH)-propanol (CH3CH2CH2OH) solution that has a vapor... Problem 60E: Benzene and toluene form an ideal solution. Consider a solution of benzene and toluene prepared at... Problem 61E: Which of the following will have the lowest total vapor pressure at 25C? a. pure water (vapor... Problem 62E Problem 63E: Match the vapor pressure diagrams with the solute-solvent combinations and explain your answers. a.... Problem 64E: The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various... Problem 65E: A solution is prepared by dissolving 27.0 g urea, (NH2)CO, in 150.0 g water. Calculate the boiling... Problem 66E: A 2.00-g sample of a large biomolecule was dissolved in 15.0 g carbon tetrachloride. The boiling... Problem 67E: What mass of glycerin (C3H8O3), a nonelectrolyte, must be dissolved in 200.0 g water to give a... Problem 68E: The freezing point of 1-butanol is 25.50C and Kf is 9.1C kg/mol. Usually t-butanol absorbs water on... Problem 69E Problem 70E: What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 15.0 L water to produce... Problem 71E: Reserpine is a natural product isolated from the roots of the shrub Rauwolfia serpenlina. It was... Problem 72E: A solution contains 3.75 g of a nonvolatile pure hydrocarbon in 95 g acetone. The boiling points of... Problem 73E: a. Calculate the freezing-point depression and osmotic pressure at 25C of an aqueous solution... Problem 74E: Erythrocytes are red blood cells containing hemoglobin. In a saline solution they shrivel when the... Problem 75E Problem 76E Problem 77E Problem 78E Problem 79E: Consider the following solutions: 0.010 m Na3PO4 in water 0.020 m CaBr2 in water 0.020 m KCl in... Problem 80E: From the following: pure water solution of C12H22O11 (m = 0.01) in water solution of NaCl (m = 0.01)... Problem 81E Problem 82E Problem 83E Problem 84E: Consider the following representations of an ionic solute in water. Which flask contains MgSO4, and... Problem 85E Problem 86E Problem 87E: Use the following data for three aqueous solutions of CaCl2 to calculate the apparent value of the... Problem 88E: The freezing-point depression of a 0.091-m solution of CsCl is 0.320C. The freezing-point depression... Problem 89E Problem 90E: A 0.500-g sample of a compound is dissolved in enough water to form 100.0 mL of solution. This... Problem 91AE: 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 92AE Problem 94AE: In Exercise 96 in Chapter 8, the pressure of CO2 in a bottle of sparkling wine was calculated... Problem 95AE: Explain the following on the basis of the behavior of atoms and/or ions. a. Cooking with water is... Problem 96AE: The term proof is defined as twice the percent by volume of pure ethanol in solution. Thus, a... Problem 97AE Problem 98AE Problem 99AE: A solution is made by mixing 50.0 g acetone (CH3COCH3) and 50.0 g methanol (CH3OH). What is the... Problem 100AE Problem 101AE: Thyroxine, an important hormone that controls the rate of metabolism in the body, can be isolated... Problem 102AE Problem 103AE: An unknown compound contains only carbon, hydrogen, and oxygen. Combustion analysis of the compound... Problem 104AE Problem 105AE Problem 106AE Problem 107AE Problem 108AE Problem 109AE: Patients undergoing an upper gastrointestinal tract laboratory test are typically given an X-ray... Problem 110CWP Problem 111CWP: The lattice energy of NaCl is 786 kJ/mol, and the enthalpy of hydration of 1 mole of gaseous Na+ and... Problem 112CWP: For each of the following pairs, predict which substance is more soluble in water. a. CH3NH2 or NH3... Problem 113CWP: The normal boiling point of methanol is 64.7C. A solution containing a nonvolatile solute dissolved... Problem 114CWP: A solution is prepared by mixing 1.000 mole of methanol (CH3OH) and 3.18 moles of propanol... Problem 115CWP Problem 116CWP: A 4.7 102 mg sample of a protein is dissolved in water to make 0.25 mL of solution. The osmotic... Problem 117CWP: 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 118CP: The vapor pressure of pure benzene is 750.0 torr and the vapor pressure of toluene is 300.0 torr at... Problem 119CP Problem 120CP: Plants that thrive in salt water must have internal solutions (inside the plant cells) that are... Problem 121CP: You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The... Problem 122CP Problem 123CP: The vapor in equilibrium with a pentane-hexane solution at 25C has a mole fraction of pentane equal... Problem 124CP: A forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar... Problem 125CP: A 1.60-g sample of a mixture of naphthalene (C10H8) and anthracene (C14H10) is dissolved in 20.0 g... Problem 126CP Problem 127CP Problem 128CP: You have a solution of two volatile liquids, A and B (assume ideal behavior). Pure liquid A has a... Problem 129CP: In some regions of the southwest United States, the water is very hard. For example, in Las Cruces,... Problem 130IP: Creatinine, C4H7N3O, is a by-product of muscle metabolism, and creatinine levels in the body are... Problem 131IP: An aqueous solution containing 0.250 mole of Q, a strong electrolyte, in 5.00 102 g water freezes... Problem 132IP: Anthraquinone contains only carbon, hydrogen, and oxygen. When 4.80 mg anthraquinone is burned, 14.2... Problem 108AE
Related questions
Calculate the new initial concentrations of KI, Na2S2O3, HCl and KBrO3 after being diluted in the overall reaction mixture.
B.) For each experiment, determine the rate of reaction with respect to I- (rateI-). Remember that the time you measured was the time for all of the S2O32- to react
Transcribed Image Text: Data:
Exp. 1 - Trial 1
Exp. 1-Trial 2
Exp. 2 - Trial 1
Exp. 2- Trial 2
Exp. 3 - Trial 1
Exp. 3- Trial 2
Exp. 4 - Trial 1
Exp. 4 - Trial 2
Time
9.46
9.31
7.28
9.35
5.23
7.37
4.05
4.24
Unit
S
S
S
S
S
S
S
S
Transcribed Image Text: Exp. Solution 1:
0.010 M KI
1
2
3
4
2.00mL
4.00 mL
2.00 mL
2.00 mL
First Graduated cylinder
Solution 2:
0.001 M Na₂S₂O,
5.00 mL
5.00 mL
5.00 mL
5.00 mL
Water
3.00 mL
1.00 mL
3.00 mL
3.00 mL
Solution 4:
2% Starch
3-4 drops
3-4 drops
3-4 drops
3-4 drops
Second graduated cylinder
Solution 5:
0.10 M HCI
3.00 mL
3.00 mL
3.00 mL
6.00 mL
Solution 6:
0.040 M KBRO,
3.00 mL
3.00 mL
6.00 mL
3.00 mL
Water
4.00 mL
4.00 mL
1.00 mL
1.00 mL
Do the following for each exp.
1. In a 10 mL graduated cylinder measure out solutions 1-4 (one on top of the other)
2. Pour the contents of the graduated cylinder into a small beaker
3. In a separate 10 mL graduated cylinder that will be dedicated for the potassium bromate, measure out solutions 5,
6, and water.
4. The instant this mixture is added to the beaker, you will need to start timing the time it takes until the solution
turns blue.
[(()))
5. Add solution 6 to the beaker, start timing and stir.
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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