Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
Chapter 11, Problem 28Q
Interpretation Introduction
Interpretation: The given statement is true or not has to be explained.
Concept Introduction:
Colligative properties of a substance include the depression in the freezing point, elevation of boiling-point and osmotic pressure. These are dependant only on the number present and not based on the solute particles present in an ideal solution. These properties have a direct relationship to the solute particles, and therefore the colligative properties are useful for identifying the nature of solute particles and also calculating the molar masses of substances.
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Chapter 11 Solutions
Chemistry
Ch. 11 - Prob. 1RQCh. 11 - Using KF as an example, write equations that refer...Ch. 11 - Prob. 3RQCh. 11 - Prob. 4RQCh. 11 - Define the terms in Raoults law. Figure 10-9...Ch. 11 - In terms of Raoults law, distinguish between an...Ch. 11 - Vapor-pressure lowering is a colligative property,...Ch. 11 - What is osmotic pressure? How is osmotic pressure...Ch. 11 - Distinguish between a strong electrolyte, a weak...Ch. 11 - Prob. 10RQ
Ch. 11 - Prob. 1ALQCh. 11 - Once again, consider Fig. 10-9. Suppose instead of...Ch. 11 - Prob. 3ALQCh. 11 - Prob. 4ALQCh. 11 - You have read that adding a solute to a solvent...Ch. 11 - You drop an ice cube (made from pure water) into a...Ch. 11 - Using the phase diagram for water and Raoults law,...Ch. 11 - You and your friend are each drinking cola from...Ch. 11 - Prob. 9ALQCh. 11 - Prob. 10ALQCh. 11 - If a solution shows positive deviations from...Ch. 11 - Prob. 12ALQCh. 11 - Rubbing alcohol contains 585 g isopropanol...Ch. 11 - Prob. 14SRCh. 11 - Prob. 15SRCh. 11 - Prob. 16SRCh. 11 - Calculate the sodium ion concentration when 70.0...Ch. 11 - Write equations showing the ions present after the...Ch. 11 - Rationalize the temperature dependence of the...Ch. 11 - The weak electrolyte NH3(g) does not obey Henrys...Ch. 11 - The two beakers in the sealed container...Ch. 11 - The following plot shows the vapor pressure of...Ch. 11 - When pure methanol is mixed with water, the...Ch. 11 - Prob. 24QCh. 11 - For an acid or a base, when is the normality of a...Ch. 11 - Prob. 26QCh. 11 - Prob. 27QCh. 11 - Prob. 28QCh. 11 - Prob. 29QCh. 11 - Table sugar (C12H22O11) or urea [(NH2)2CO] can be...Ch. 11 - If two different aqueous solutions of proteins...Ch. 11 - An extremely important application of dialysis is...Ch. 11 - Explain the terms isotonic solution, crenation,...Ch. 11 - Prob. 34QCh. 11 - Prob. 35ECh. 11 - A typical IV used in hospitals is dextrose 5% in...Ch. 11 - Prob. 37ECh. 11 - Prob. 38ECh. 11 - Common commercial acids and bases are aqueous...Ch. 11 - In lab you need to prepare at least 100 mL of each...Ch. 11 - Prob. 41ECh. 11 - Prob. 42ECh. 11 - Prob. 43ECh. 11 - Calculate the molarity and mole fraction of...Ch. 11 - Prob. 45ECh. 11 - Prob. 46ECh. 11 - Prob. 47ECh. 11 - a. Use the following data to calculate the...Ch. 11 - Although Al(OH)3 is insoluble in water, NaOH is...Ch. 11 - Prob. 50ECh. 11 - Prob. 51ECh. 11 - Prob. 52ECh. 11 - For each of the following pairs, predict which...Ch. 11 - Which ion in each of the following pairs would you...Ch. 11 - Rationalize the trend in water solubility for the...Ch. 11 - In flushing and cleaning columns used in liquid...Ch. 11 - The solubility of nitrogen in water is 8.21 104...Ch. 11 - Calculate the solubility of O2 in water at a...Ch. 11 - The vapor pressure of a solution containing 53.6 g...Ch. 11 - An aqueous solution containing glucose has a vapor...Ch. 11 - The normal boiling point of diethyl ether is...Ch. 11 - At a certain temperature, the vapor pressure of...Ch. 11 - Prob. 63ECh. 11 - A solution is prepared by mixing 0.0300 mole of...Ch. 11 - What is the composition of a methanol...Ch. 11 - Benzene and toluene form an ideal solution....Ch. 11 - Which of the following will have the lowest total...Ch. 11 - Prob. 68ECh. 11 - Match the vapor pressure diagrams with the...Ch. 11 - The vapor pressures of several solutions of...Ch. 11 - A solution is prepared by dissolving 27.0 g urea,...Ch. 11 - A 2.00-g sample of a large biomolecule was...Ch. 11 - What mass of glycerin (C3H8O3), a nonelectrolyte,...Ch. 11 - The freezing point of 1-butanol is 25.50C and Kf...Ch. 11 - Prob. 75ECh. 11 - What volume of ethylene glycol (C2H6O2), a...Ch. 11 - Reserpine is a natural product isolated from the...Ch. 11 - A solution contains 3.75 g of a nonvolatile pure...Ch. 11 - a. Calculate the freezing-point depression and...Ch. 11 - Erythrocytes are red blood cells containing...Ch. 11 - Prob. 81ECh. 11 - Prob. 82ECh. 11 - Prob. 83ECh. 11 - Prob. 84ECh. 11 - Consider the following solutions: 0.010 m Na3PO4...Ch. 11 - From the following: pure water solution of...Ch. 11 - Prob. 87ECh. 11 - Prob. 88ECh. 11 - Prob. 89ECh. 11 - Consider the following representations of an ionic...Ch. 11 - Prob. 91ECh. 11 - Prob. 92ECh. 11 - Use the following data for three aqueous solutions...Ch. 11 - The freezing-point depression of a 0.091-m...Ch. 11 - Prob. 95ECh. 11 - A 0.500-g sample of a compound is dissolved in...Ch. 11 - The solubility of benzoic acid (HC7H5O2), is 0.34...Ch. 11 - Prob. 99AECh. 11 - Prob. 100AECh. 11 - Prob. 101AECh. 11 - In Exercise 96 in Chapter 8, the pressure of CO2...Ch. 11 - Explain the following on the basis of the behavior...Ch. 11 - The term proof is defined as twice the percent by...Ch. 11 - Prob. 105AECh. 11 - Prob. 106AECh. 11 - A solution is made by mixing 50.0 g acetone...Ch. 11 - Prob. 108AECh. 11 - Thyroxine, an important hormone that controls the...Ch. 11 - Prob. 110AECh. 11 - An unknown compound contains only carbon,...Ch. 11 - Prob. 112AECh. 11 - Prob. 113AECh. 11 - Prob. 115AECh. 11 - Patients undergoing an upper gastrointestinal...Ch. 11 - Prob. 118CWPCh. 11 - The lattice energy of NaCl is 786 kJ/mol, and the...Ch. 11 - For each of the following pairs, predict which...Ch. 11 - The normal boiling point of methanol is 64.7C. A...Ch. 11 - A solution is prepared by mixing 1.000 mole of...Ch. 11 - Prob. 123CWPCh. 11 - A 4.7 102 mg sample of a protein is dissolved in...Ch. 11 - A solid consists of a mixture of NaNO3 and...Ch. 11 - The vapor pressure of pure benzene is 750.0 torr...Ch. 11 - Prob. 127CPCh. 11 - Plants that thrive in salt water must have...Ch. 11 - You make 20.0 g of a sucrose (C12H22O11) and NaCl...Ch. 11 - Prob. 130CPCh. 11 - The vapor in equilibrium with a pentane-hexane...Ch. 11 - A forensic chemist is given a white solid that is...Ch. 11 - A 1.60-g sample of a mixture of naphthalene...Ch. 11 - Prob. 134CPCh. 11 - Prob. 135CPCh. 11 - You have a solution of two volatile liquids, A and...Ch. 11 - In some regions of the southwest United States,...Ch. 11 - Specifications for lactated Ringers solution,...Ch. 11 - Creatinine, C4H7N3O, is a by-product of muscle...Ch. 11 - An aqueous solution containing 0.250 mole of Q, a...Ch. 11 - Anthraquinone contains only carbon, hydrogen, and...
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Similar questions
- A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentratedarrow_forwardCreate a flow diagram, similar to those used in the example problems of this chapter, that outlines the determination of the molar mass of a compound from freezing-point depression measurements. Clearly indicate the data needed for this determination.arrow_forwardDistinguish between a strong electrolyte, a weak electrolyte, and a nonelectrolyte. How can colligative properties be used to distinguish between them? What is the vant Hoff factor? Why is the observed freezing-point depression for electrolyte solutions sometimes less than the calculated value? Is the discrepancy greater for concentrated or dilute solutions?arrow_forward
- You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The freezing point of this solution is found to be 0.426C. Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.arrow_forwardOnce again, consider Fig. 10-9. Suppose instead of having a nonvolatile solute in the solvent in one beaker, the two beakers contain different volatile liquids. That is, suppose one beaker contains liquid A (Pvap = 50 torr) and the other beaker contains liquid B (Pvap = 100 torr). Explain what happens as time passes. How is this similar to the first case (shown in the figure)? How is it different?arrow_forward
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