Chemistry (OER)
19th Edition
ISBN: 9781947172623
Author: OpenStax
Publisher: OpenStax College
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Textbook Question
Chapter 11, Problem 32E
Calculate the mole fraction of each solute and solvent:
(a) 583 g of H2SO4 in 1.50 kg of water—the acid solution used in an automobile battery
(b) 0.86 g of NaCl in
(c) 46.85 g of codeine, C18H21NO3, in 125.5 g of ethanol, C2H5OH
(d) 25 g of I2 in 125 g of ethanol, C2H5OH
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Calculate the mole fraction of each solute and solvent:(a) 583 g of H2SO4 in 1.50 kg of water—the acid solution used in an automobile battery(b) 0.86 g of NaCl in 1.00 × 102 g of water—a solution of sodium chloride for intravenous injection(c) 46.85 g of codeine, C18H21NO3, in 125.5 g of ethanol, C2H5OH(d) 25 g of I2 in 125 g of ethanol, C2H5OH
Calculate the molality of each of the following solutions:(a) 583 g of H2SO4 in 1.50 kg of water—the acid solution used in an automobile battery(b) 0.86 g of NaCl in 1.00 × 102 g of water—a solution of sodium chloride for intravenous injection(c) 46.85 g of codeine, C18H21NO3, in 125.5 g of ethanol, C2H5OH(d) 25 g of I2 in 125 g of ethanol, C2H5OH
(a) What is the molarity of a solution made by dissolving 10 moles of sucrose, C12H22O11, in 10L of water?
(b) How much boric acid (H3BO3), in grams, is needed to be dissolves in 300.g of water to make a 1.50m aqueous H3BO3 solution? The molar mass of H3BO3 is 61.83g/mol.
(c) How much aluminum sulfate (Al2(SO4)3) in moles, is needed to be dissolved in 500g of water to make a 1.0m aqueous Al2(SO4)3 solution?
Chapter 11 Solutions
Chemistry (OER)
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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