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Chemistry: Atoms First
18th Edition
ISBN: 9781938168154
Author: Richard Langley, Klaus Theopold, Paul Flowers
Publisher: OpenStax College
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Textbook Question
Chapter 11, Problem 2E
Which of the principal characteristics of solutions are evident in the solutions of
Figure 11.2 When potassium dichromate
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Chapter 11 Solutions
Chemistry: Atoms First
Ch. 11 - How do solutions differ from compounds? From other...Ch. 11 - Which of the principal characteristics of...Ch. 11 - When KNO3 is dissolved in water, the resulting...Ch. 11 - Give an example of each of the following types of...Ch. 11 - Indicate the most important types of...Ch. 11 - Predict whether each of the following substances...Ch. 11 - Heat is released when some solutions form; heat is...Ch. 11 - Solutions of hydrogen in palladium may be formed...Ch. 11 - Explain why the ions Na+ and CI- are strongly...Ch. 11 - Explain why solutions of HBr in benzene (a...
Ch. 11 - Consider the solutions presented: (a) Which of the...Ch. 11 - Compare the processes that occur when methanol...Ch. 11 - What is the expected electrical conductivity of...Ch. 11 - Why are most solid ionic compounds electrically...Ch. 11 - Indicate the most important type of intermolecular...Ch. 11 - Suppose you are presented with a clear solution of...Ch. 11 - Supersaturated solutions of most solids in water...Ch. 11 - Suggest an explanation for the observations that...Ch. 11 - Calculate the percent by mass of KBr in a...Ch. 11 - Which of the following gases is expected to be...Ch. 11 - At 0 C and 1.00 atm, as much as 0.70 g of O2 can...Ch. 11 - Refer to Figure 11.10. (a) How did the...Ch. 11 - The Henrys law constant for CO2 is 3.4102 M/atm at...Ch. 11 - The Henrys law constant for O2 is 1.3103 M/ atm at...Ch. 11 - Assuming ideal solution behavior, how many liters...Ch. 11 - Which is are part of the macroscopic domain of...Ch. 11 - What is the microscopic explanation for the...Ch. 11 - Sketch a qualitative graph of the pressure versus...Ch. 11 - A solution of potassium nitrate, an electrolyte,...Ch. 11 - What are the mole fractions of H3PO4 and water in...Ch. 11 - What are the mole fractions of HNO3 and water in a...Ch. 11 - Calculate the mole fraction of each solute and...Ch. 11 - Calculate the mole fraction of each solute and...Ch. 11 - Calculate the mole fractions of methanol, CH3OH;...Ch. 11 - What is the difference between a 1 M solution and...Ch. 11 - What is the molality of phosphoric acid, H3PO4, in...Ch. 11 - What is the molality of nitric acid in a...Ch. 11 - Calculate the molality of each of the following...Ch. 11 - Calculate the molality of each of the following...Ch. 11 - The concentration of glucose, C6H12O6, in normal...Ch. 11 - A 13.0% solution of K2CO3 by mass has a density of...Ch. 11 - Why does 1 mol of sodium chloride depress the...Ch. 11 - Assuming ideal solution behavior what is the...Ch. 11 - Assuming ideal solution behavior, what is the...Ch. 11 - Assuming ideal solution behavior, what is the...Ch. 11 - Assuming ideal solution behavior, what is the...Ch. 11 - Assuming ideal solution behavior, what is the...Ch. 11 - Assuming ideal solution behavior, what is osmotic...Ch. 11 - Assuming ideal solution behavior, what is the...Ch. 11 - A sample of an organic compound (a nonelectrolyte)...Ch. 11 - A 1.0 m solution of HCI in benzene has a freezing...Ch. 11 - A solution contains 5.00 g of urea, CO(NH2)2 , a...Ch. 11 - A 12.O-g sample of a nonelectrolyte is dissolved...Ch. 11 - Arrange the following solutions in order by their...Ch. 11 - Calculate the boiling point elevation of 0.100 kg...Ch. 11 - How could you prepare a 3.08m aqueous solution of...Ch. 11 - A sample of sulfur weighing 0.210 g was dissolved...Ch. 11 - In a significant experiment performed many years...Ch. 11 - Lysozyme is an enzyme that cleaves cell walls. A...Ch. 11 - The osmotic pressure of a solution containing 7.0...Ch. 11 - The osmotic pressure of human blood is 7.6 atm at...Ch. 11 - Assuming ideal solution behavior, what is the...Ch. 11 - Assuming ideal solution behavior, what is the...Ch. 11 - The sugar fructose contains 40.0% C, 6.7% H, and...Ch. 11 - The vapor pressure of methanol, CH3OH, is 94 torr...Ch. 11 - The triple point of air-free water is defined as...Ch. 11 - Meat can be classified as fresh (not frozen) even...Ch. 11 - An organic compound has a composition of 93.46% C...Ch. 11 - A sample of HgCI2 weighing 9.41 g is dissolved in...Ch. 11 - A salt is known to be an alkali metal fluoride. A...Ch. 11 - Identify the dispersed phase and the dispersion...Ch. 11 - Distinguish between dispersion methods and...Ch. 11 - How do colloids differ from solutions with regard...Ch. 11 - Explain the cleansing action of soap.Ch. 11 - How can it be demonstrated that colloidal...
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- In a mountainous location, the boiling point of pure water is found to be 95C. How many grams of sodium chloride must be added to 1 kg of water to bring the boiling point back to 100C? Assume that i = 2.arrow_forwardConsider two hypothetical pure substances, AB(s) and XY(s). When equal molar amounts of these substances are placed in separate 500-mL samples of water, they undergo the following reactions: AB(s)A+(aq)+B(aq)XY(s)XY(aq) a Which solution would you expect to have the lower boiling point? Why? b Would you expect the vapor pressures of the two solutions to be equal? If not, which one would you expect to have the higher vapor pressure? c Describe a procedure that would make the two solutions have the same boiling point. d If you took 250 mL of the AB(aq) solution prepared above, would it have the same boiling point as the original solution? Be sure to explain your answer. e The container of XY(aq) is left out on the bench top for several days, which allows some of the water to evaporate from the solution. How would the melting point of this solution compare to the melting point of the original solution?arrow_forwardSodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)arrow_forward
- Which of the following salts, Li2SO4 or Cs2SO4, is expected to have the more exothermic enthalpy of hydration?arrow_forwardArrange the following alkaline-earth-metal iodates in order of increasing solubility in water and explain your reasoning: Ba(IO3)2, Ca(IO3)2, Sr(IO3)2, Mg(IO3)2. Note that IO3 is a large anion.arrow_forwardSamples of each of the substances listed below are dissolved in 125 g of water. Which of the solutions has the highest boiling point? (a) 3.0 g sucrose, C12H22O11 (b) 1.0 g glycerol, C3H3(OH)3 (c) 1.0 g propylene glycol, C3H6(OH)2 (d) 2.0 g glucose, C6H12(OH)2arrow_forward
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY