Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 10, Problem 49QAP
Caffeine is made up of 49.5% C, 5.2% H, 16.5% O, and 28.9% N. A solution made up of 8.25 g of caffeine and 100.0 mL of benzene
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Chapter 10 Solutions
Chemistry: Principles and Reactions
Ch. 10 - A solution is prepared by dissolving 12.15 g of...Ch. 10 - Prob. 2QAPCh. 10 - Prob. 3QAPCh. 10 - Solutions Introduced directly into the bloodstream...Ch. 10 - Silver ions can be found in some of the city water...Ch. 10 - Prob. 6QAPCh. 10 - Complete the following table for aqueous solutions...Ch. 10 - Complete the following table for aqueous solutions...Ch. 10 - Complete the following table for aqueous solutions...Ch. 10 - Complete the following table for aqueous solutions...
Ch. 10 - Prob. 11QAPCh. 10 - Prob. 12QAPCh. 10 - Prob. 13QAPCh. 10 - A solution is prepared by diluting 0.7850 L of...Ch. 10 - A bottle of phosphoric acid is labeled 85.0% H3PO4...Ch. 10 - Prob. 16QAPCh. 10 - Complete the following table for aqueous solutions...Ch. 10 - Complete the following table for aqueous solutions...Ch. 10 - Assume that 30 L of maple sap yields one kilogram...Ch. 10 - Juice (d=1.0g/mL) from freshly harvested grapes...Ch. 10 - Prob. 21QAPCh. 10 - Which of the following is more likely to be...Ch. 10 - Prob. 23QAPCh. 10 - Prob. 24QAPCh. 10 - Consider the process by which lead chloride...Ch. 10 - Prob. 26QAPCh. 10 - The Henry's law constant for the solubility of...Ch. 10 - The Henry's law constant for the solubility of...Ch. 10 - A carbonated beverage is made by saturating water...Ch. 10 - Air contains 78% nitrogen. At 25C, Henry's law...Ch. 10 - Vodka is advertised to be 80 proof. That means...Ch. 10 - What is the freezing point of maple syrup (66%...Ch. 10 - Calculate the vapor pressure of water over each of...Ch. 10 - Calculate the vapor pressure of water over each of...Ch. 10 - Prob. 35QAPCh. 10 - Consider an aqueous solution of urea, (CO(NH2)2)...Ch. 10 - Prob. 37QAPCh. 10 - Prob. 38QAPCh. 10 - Calculate the freezing point and normal boiling...Ch. 10 - How many grams of the following nonelectrolytes...Ch. 10 - What is the freezing point and normal boiling...Ch. 10 - Antifreeze solutions are aqueous solutions of...Ch. 10 - When 13.66 g of lactic acid, C3H6O3, are mixed...Ch. 10 - A solution consisting of 4.50 g of propylene...Ch. 10 - Insulin is a hormone responsible for the...Ch. 10 - Epinephrine (or adrenaline) is a hormone and...Ch. 10 - Lauryl alcohol is obtained from the coconut and is...Ch. 10 - The Rast method uses camphor (C10H16O) as a...Ch. 10 - Caffeine is made up of 49.5% C, 5.2% H, 16.5% O,...Ch. 10 - A compound contains 42.9% C, 2.4% H, 16.6% N, and...Ch. 10 - A biochemist isolates a new protein and determines...Ch. 10 - Prob. 52QAPCh. 10 - Estimate the freezing and boiling points of normal...Ch. 10 - Arrange 0.10 m aqueous solutions of the following...Ch. 10 - Aqueous solutions introduced into the stream y...Ch. 10 - What is the osmotic pressure of a 0.135 M solution...Ch. 10 - The freezing point of a 0.11 m solution of HNO2 is...Ch. 10 - The freezing point of a 0.21 m aqueous solution of...Ch. 10 - An aqueous solution of LiX is prepared by...Ch. 10 - An aqueous solution of M2O is prepared by...Ch. 10 - A sucrose (C12H22O11) solution that is 45.0%...Ch. 10 - An aqueous solution made up of 32.47 g of...Ch. 10 - How would you prepare 5.00 L of a solution that is...Ch. 10 - Carbon tetrachloride (CCl4) boils at 76.8C and has...Ch. 10 - Twenty-five milliliters of a solution...Ch. 10 - The Henry's law constant for the solubility of...Ch. 10 - Prob. 67QAPCh. 10 - Consider two solutions at a certain temperature....Ch. 10 - A pharmacist prepares an isotonic saline solution...Ch. 10 - One mole of CaCl2 is represented as where...Ch. 10 - One mole of Na2S is represented as where...Ch. 10 - Prob. 72QAPCh. 10 - Consider three test tubes. Tube A has pure water....Ch. 10 - The freezing point of 0.20 m HF is -0.38C. Is HF...Ch. 10 - A certain gaseous solute dissolves in water,...Ch. 10 - The freezing point of 0.10 M KHSO3 is -0.38C....Ch. 10 - Consider 2 vapor pressure curves A and B. They are...Ch. 10 - A gaseous solute dissolves in water. The solution...Ch. 10 - In your own words, explain (a) why seawater has a...Ch. 10 - Prob. 80QAPCh. 10 - Beaker A has 1.00 mol of chloroform, CHCl3, at...Ch. 10 - Prob. 82QAPCh. 10 - Prob. 83QAPCh. 10 - Prob. 84QAPCh. 10 - Prob. 85QAPCh. 10 - A martini, weighing about 5.0 oz (142 g), contains...Ch. 10 - When water is added to a mixture of aluminum metal...Ch. 10 - Prob. 88QAPCh. 10 - Prob. 89QAP
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- Carbon tetrachloride (CCl4) boils at 76.8C and has a density of 1.59 g/mL. (a) A solution prepared by dissolving 0.287 mol of a nonelectrolyte in 255 mL of CCl4 boils at 80.3C. What is the boiling point constant (kb) for CCl4? (b) Another solution is prepared by dissolving 37.1 g of an electrolyte (MM=167g/mol) in 244 mL of CCl4. The resulting solution boils at 85.2C. What is i for the electrolyte?arrow_forwardFor each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Oxygen gas in water with P = 1 atm and T = 10C Oxygen gas in water with P = 1 atm and T = 20C b. Nitrogen gas in water with P = 2 atm and T = 50C Nitrogen gas in water with P = 1 atm and T = 70C c. Table salt in water with P = 1 atm and T = 40C Table salt in water with P = 1 atm and T = 70C d. Table sugar in water with P = 3 atm and T = 30C Table sugar in water with P = 1 atm and T = 80Carrow_forwardA forensic chemist is given a white solid that is suspected of being pure cocaine (C17H21NO4, molar mass = 303.35 g/mol). She dissolves 1.22 0.01 g of the solid in 15.60 0.01 g benzene. The freezing point is lowered by 1.32 0.04C. a. What is the molar mass of the substance? Assuming that the percent uncertainty in the calculated molar mass is the same as the percent uncertainty in the temperature change, calculate the uncertainty in the molar mass. b. Could the chemist unequivocally state that the substance is cocaine? For example, is the uncertainty small enough to distinguish cocaine from codeine (C18H21NO3, molar mass = 299.36 g/mol)? c. Assuming that the absolute uncertainties in the measurements of temperature and mass remain unchanged, how could the chemist improve the precision of her results?arrow_forward
- 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_forwardFor each of the following pairs of solutions, select the solution for which solute solubility is greatest. a. Ammonia gas in water with P = 1 atm and T = 50C Ammonia gas in water with P = 1 atm and T = 90C b. Carbon dioxide gas in water with P = 2 atm and T = 50C Carbon dioxide gas in water with P = 1 atm and T = 50C c. Table salt in water with P = 1 atm and T = 60C Table salt in water with P = 1 atm and T = 50C d. Table sugar in water with P = 2 atm and T = 40C Table sugar in water with P = 1 atm and T = 70Carrow_forwardCalculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.arrow_forward
- The freezing point of a 0.21 m aqueous solution of H2SO4 is -0.796C. (a) What is i? (b) Is the solution made up primarily of (i) H2SO4 molecules only? (ii) H+ and HSO4- ions? (iii) 2H+ and 1SO42- ions?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_forwardRefer to Figure 13.10 ( Sec. 13-4b) to answer these questions. (a) Does a saturated solution occur when 65.0 g LiCl is present in 100 g H2O at 40 C? Explain your answer. (b) Consider a solution that contains 95.0 g LiCl in 100 g H2O at 40 C. Is the solution unsaturated, saturated, or supersaturated? Explain your answer. (c) Consider a solution that contains 50. g Li2SO4 in 200. g H2O at 50 C. Is this solution unsaturated, saturated, or supersaturated? Explain your answer. Figure 13.10 Solubility of ionic compounds versus temperature.arrow_forward
- The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?arrow_forwardWhat is the freezing point and normal boiling point of a solution made by adding 39 mL of acetone, C3H6O, to 225 mL of water? The densities of acetone and water are 0.790 g/cm3 and 1.00 g/cm3, respectively.arrow_forwardA sample of aluminum sulfate 18-hydrate, Al2(SO4)3. 18H2O, containing 125.0 mg is dissolved in 1.000 L of solution. Calculate the following for the solution: a The molarity of Al2(SO4)3. b The molarity of SO42. c The molality of Al2(SO4)3, assuming that the density of the solution is 1.00 g/mL.arrow_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