Explanation We need to convert the amount/volume of solute and solvent that present into moles that is necessary for the equations below. Given: Densities of methanol is 0.782 g/mL Densities of water is 1.00 g/mL Formula used: a. molarity = moles solute / litres of total solution b. molarity = moles solute / kg of solvent c. percent by mass = grams solute / total g solution×100/1 d. mole fraction = moles solute / total moles in solution e. mole percent = moles solute / total moles in solution × 100/1 moles = mass / molar mass density = mass / volume Calculation: Volume of methanol = 20.2 ml = 0.0202 L So, Mass of methanol = density x volume = 0.782 g/ml × 20.2 ml = 15.8 g Now , moles of methanol = mass / molar mass = 15.8 g / 32.042 g/mol = 0.493 moles Volume of water= 100.0 ml = 0.1000 L Mass of water = density x volume = 1.00 g/ml × 100.0 ml = 100.0 g Molesof water= mass / molar mass = 100.0 g / 18.016 g/mol = 5.55 moles Total solution volume = 118 ml = 0.118 L Total Mass = Mass of methanol + mass of water = 15...

Chemistry: Structure and Properties, Books a la Carte PACKAGE W/MasteringChemistry, 2nd Edition

2nd Edition

ISBN: 9780134777559

Author: Tro, Nivaldo J.

Publisher: PEARSON

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Question

Chapter 13, Problem 60E

Interpretation Introduction

To determine:

Calculate the concentration of the above mentioned solution in each unit.

a. molarity

b. molarity

c. percent by mass

d. mole fraction

e. mole percent

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Chapter 13, Problem 59E

Chapter 13, Problem 61E

Chapter 13 Solutions

Chemistry: Structure and Properties, Books a la Carte PACKAGE W/MasteringChemistry, 2nd Edition

Ch. 13 - What is a solution? What are the solute and...Ch. 13 - What does it mean when we say that a substance is...Ch. 13 - Why do two ideal gases thoroughly mix when...Ch. 13 - Prob. 4E Ch. 13 - Prob. 5E Ch. 13 - Explain how the relative strengths of...Ch. 13 - What does the statement like dissolves like mean...Ch. 13 - Prob. 8E Ch. 13 - What is the heat of hydration(Hhydration)? How...Ch. 13 - Prob. 10E

Ch. 13 - How does temperature affect the solubility of a...Ch. 13 - Prob. 12E Ch. 13 - How does pressure affect the solubility of a gas...Ch. 13 - What is Henry’s law? For what kinds of...Ch. 13 - Prob. 15E Ch. 13 - How are parts by mass and parts by volume used in...Ch. 13 - Prob. 17E Ch. 13 - What is Raoult’s law? For what kind of...Ch. 13 - Explain the difference between an ideal and a...Ch. 13 - Prob. 20E Ch. 13 - Prob. 21E Ch. 13 - What are colligative properties?Ch. 13 - Prob. 23E Ch. 13 - Explain the significance of the van’t Hoff factor...Ch. 13 - Prob. 25E Ch. 13 - Pick an appropriate solvent from Table 13.3 to...Ch. 13 - Which molecule would you expect to be more soluble...Ch. 13 - Prob. 28E Ch. 13 - Prob. 29E Ch. 13 - Prob. 30E Ch. 13 - When ammonium chloride (NH4Cl) is dissolved in...Ch. 13 - Prob. 32E Ch. 13 - Prob. 33E Ch. 13 - Use the given data to calculate the heats of...Ch. 13 - Lithium iodide has a lattice energy of...Ch. 13 - Prob. 36E Ch. 13 - A solution contains 25 g of NaCl per 100.0 g of...Ch. 13 - A solution contains 32 g of KNO3 per 100.0 g of...Ch. 13 - Prob. 39E Ch. 13 - A KCI solution containing 42 g of KCI per 100.0 g...Ch. 13 - Some laboratory procedures involving...Ch. 13 - A person preparing a fish tank fills the tank with...Ch. 13 - Prob. 43E Ch. 13 - Scuba divers breathing air at increased pressure...Ch. 13 - Calculate the mass of nitrogen dissolved at room...Ch. 13 - Use Henry’s law to determine the molar solubility...Ch. 13 - An aqueous NaCl solution is made using 112 g of...Ch. 13 - Prob. 48E Ch. 13 - To what volume should you dilute 50.0 mL of a...Ch. 13 - Prob. 50E Ch. 13 - Silver nitrate solutions are used to plate silver...Ch. 13 - Prob. 52E Ch. 13 - Prob. 53E Ch. 13 - Prob. 54E Ch. 13 - You can purchase nitric acid in a concentrated...Ch. 13 - You can purchase hydrochloric acid in a...Ch. 13 - Prob. 57E Ch. 13 - Prob. 58E Ch. 13 - Prob. 59E Ch. 13 - Prob. 60E Ch. 13 - Prob. 61E Ch. 13 - Prob. 62E Ch. 13 - Prob. 63E Ch. 13 - Prob. 64E Ch. 13 - A beaker contains 100.0 mL of pure water. A second...Ch. 13 - Which solution has the highest vapor pressure? a....Ch. 13 - Calculate the vapor pressure of a solution...Ch. 13 - A solution contains naphthalene (C10H8) dissolved...Ch. 13 - A solution contains 50.0 g of heptane (C7H16) and...Ch. 13 - A solution contains a mixture of pentane and...Ch. 13 - A solution contains 4.08 g of chloroform (C3H8O3)...Ch. 13 - A solution of methanol and water has a mole...Ch. 13 - Prob. 73E Ch. 13 - An ethylene glycol solution contains 21.2 g of...Ch. 13 - Calculate the freezing point and melting point of...Ch. 13 - Calculate the freezing point and melting point of...Ch. 13 - An aqueous solution containing 17.5 g of an...Ch. 13 - An aqueous solution containing 35.9 g of an...Ch. 13 - Calculate the osmotic pressure of a solution...Ch. 13 - Prob. 80E Ch. 13 - A solution containing 27.55 mg of an unknown...Ch. 13 - Prob. 82E Ch. 13 - Calculate the freezing point and boiling point...Ch. 13 - Calculate the freezing point and boiling point in...Ch. 13 - What mass of salt (NaCl) should you add to 1.00 L...Ch. 13 - Prob. 86E Ch. 13 - Use the van’t Hoff factors in Table 13.7 to...Ch. 13 - Prob. 88E Ch. 13 - A 1.2-m aqueous solution of an ionic compound with...Ch. 13 - A 0.95-m aqueous solution of an ionic compound...Ch. 13 - Prob. 91E Ch. 13 - Prob. 92E Ch. 13 - Prob. 93E Ch. 13 - An aqueous CaCl2 solution has a vapor pressure of...Ch. 13 - Prob. 95E Ch. 13 - Prob. 96E Ch. 13 - Potassium perchlorate (KClO4) has a lattice energy...Ch. 13 - Sodium hydroxide (NaOH) has a lattice energy of...Ch. 13 - Prob. 99E Ch. 13 - Prob. 100E Ch. 13 - Prob. 101E Ch. 13 - Water softeners often replace calcium ions in hard...Ch. 13 - Prob. 103E Ch. 13 - Prob. 104E Ch. 13 - Prob. 105E Ch. 13 - Prob. 106E Ch. 13 - An isotonic solution contains 0.90% NaCl mass to...Ch. 13 - Prob. 108E Ch. 13 - Prob. 109E Ch. 13 - When HNO2 dissolves in water, it partially...Ch. 13 - Prob. 111E Ch. 13 - Prob. 112E Ch. 13 - Prob. 113E Ch. 13 - Distillation is a method of purification based on...Ch. 13 - Prob. 115E Ch. 13 - Find the mass of urea (CH4N2O) needed to prepare...Ch. 13 - A solution contains 10.05 g of unknown compound...Ch. 13 - Prob. 118E Ch. 13 - Prob. 119E Ch. 13 - Prob. 120E Ch. 13 - The small bubbles that form on the bottom of a...Ch. 13 - The vapor above a mixture of pentane and hexane at...Ch. 13 - A 1.10-g sample contains only glucose (C6H12O6)...Ch. 13 - Prob. 124E Ch. 13 - Two alcohols, isopropyl alcohol and propyl...Ch. 13 - A metal, M, of atomic mass 96 amu reacts with...Ch. 13 - Prob. 127E Ch. 13 - Prob. 128E Ch. 13 - A solution is prepared by dissolving 11.60 g of a...Ch. 13 - Substance A is a nonpolar liquid and has only...Ch. 13 - Prob. 131E Ch. 13 - Prob. 132E Ch. 13 - Prob. 133E Ch. 13 - Prob. 134E Ch. 13 - Prob. 135E Ch. 13 - Have each group member make a flashcard with one...Ch. 13 - Prob. 137E Ch. 13 - Prob. 138E Ch. 13 - Prob. 139E Ch. 13 - Prob. 140E Ch. 13 - Which compound is most soluble in octane (C8H18)?...Ch. 13 - Prob. 2SAQ Ch. 13 - A 500.0-mL sample of pure water is allowed to come...Ch. 13 - Prob. 4SAQ Ch. 13 - Prob. 5SAQ Ch. 13 - Prob. 6SAQ Ch. 13 - What is the vapor pressure of an aqueous ethylene...Ch. 13 - Prob. 8SAQ Ch. 13 - What mass of glucose (C6H12O6) should you dissolve...Ch. 13 - Which aqueous solution has the highest boiling...Ch. 13 - The osmotic pressure of a solution containing 22.7...Ch. 13 - The enthalpy of solution for NaOH is -44.6 kJ/mol....Ch. 13 - A 2.4-m aqueous solution of an ionic compound with...Ch. 13 - A solution is an equimolar mixture of two volatile...Ch. 13 - An aqueous solution is in equilibrium with a...

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Water at 25 C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.
Equal numbers of moles of two soluble, substances, substance A and substance B, are placed into separate 1.0-L samples of water. a The water samples are cooled. Sample A freezes at 0.50C, and Sample B freezes at l.00C. Explain how the solutions can have different freezing points. b You pour 500 mL of the solution containing substance B into a different beaker. How would the freezing point of this 500-mL portion of solution B compare to the freezing point of the 1.0-L sample of solution A? c Calculate the molality of the solutions of A and B. Assume that i = 1 for substance A. d If you were to add an additional 1.0 kg of water to solution B, what would be the new freezing point of the solution? Try to write an answer to this question without using a mathematical formula. e What concentration (molality) of substances A and B would result in both solutions having a freezing point of 0.25C? f Compare the boiling points, vapor pressure, and osmotic pressure of the original solutions of A and B. Dont perform the calculations; just state which is the greater in each ease.

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