Explanation Given: Mass of ethylene glycol ( m e ) is 21.2 g . Volume of water ( V ) is 85.4 mL . Density of water ( ρ ) is 1 g / mL . Explanation: Boiling point of water ( T pure ) is 100 ∘ C . Freezing point of water ( T pure ) is 0 ∘ C . Molar mass of ethylene glycol ( MM e ) is 62.068 g / mol . The density of a solution is equal to the ratio of mass and volume of solution. Here, mass of water can be calculated as m w = ρ × V where m w is the mass of water, ρ is the density of water, and V is the volume of water. Substitute 1 g / mL for ρ and 85.4 mL for V : m w = 1 g / mL × 85.4 mL = 85.4 g Mass of water is 85.4 g . One gram is equal to 10 − 3 kilograms. Convert grams to kilograms as follows: 85.4 g = 85.4 g × ( 10 − 3 kg 1 g ) = 0.0854 kg Mass of water in kilograms is 0.0854 kg . Calculate the number of moles of ethylene glycol as follows: n e = m e MM e Here, m e is the given mass of ethylene glycol and MM e is the molar mass of ethylene glycol. Substitute 21.2 g for m e and 62.068 g / mol for MM e : n e = 21.2 g 62.068 g / mol = 0.3416 mol So, the number of moles of ethylene glycol is 0.3416 mol . Molality of a solution ( m ) is equal to ratio of number of moles of solute (ethylene glycol) and mass of solvent (water) in kilograms. m = n e m w Substitute 0.0854 kg for m w and 0.3416 mol for n e : m = 0

Chemistry: A Molecular Approach & Student Solutions Manual for Chemistry: A Molecular Approach, Books a la Carte Edition Package

1st Edition

ISBN: 9780321955517

Author: Nivaldo J. Tro

Publisher: PEARSON

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Chapter 12, Problem 78E

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To determine: The freezing point and the boiling point of the solution.

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Chapter 12, Problem 77E

Chapter 12, Problem 79E

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CHEM2323 Problem 2-26 Tt O PS CH02 Name: Use the curved-arrow formalism to show how the electrons flow in the resonance form on the left to give the one on the right. (Draw all lone pairs first) (a) NH2 NH2 + (b) Problem 2-27 Double bonds can also act like Lewis bases, sharing their electrons with Lewis acids. Use curved arrows to show how each of the following double bonds will react with H-Cl and draw the resulting carbocation. (a) H2C=CH2 (b) (c) Problem 2-28 Identify the most electronegative element in each of the following molecules: (a) CH2FCI F Problem 2-29 (b) FCH2CH2CH2Br (c) HOCH2CH2NH2 (d) CH3OCH2Li F 0 0 Use the electronegativity table in Figure 2.3 to predict which bond in the following pairs is more polar and indicate the direction of bond polarity for each compound. (a) H3C-Cl or Cl-CI (b) H3C-H or H-CI (c) HO-CH3 or (CH3)3Si-CH3 (d) H3C-Li or Li-OH

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Chemistry: A Molecular Approach & Student Solutions Manual for Chemistry: A Molecular Approach, Books a la Carte Edition Package

Ch. 12 - Prob. 1SAQ Ch. 12 - Prob. 2SAQ Ch. 12 - Q3. A 500.0-mL sample of pure water is allowed to...Ch. 12 - Q4. A potassium bromide solution is 7.55 %...Ch. 12 - Prob. 5SAQ Ch. 12 - Prob. 6SAQ Ch. 12 - Prob. 7SAQ Ch. 12 - Prob. 8SAQ Ch. 12 - Prob. 9SAQ Ch. 12 - Prob. 10SAQ

Ch. 12 - Prob. 11SAQ Ch. 12 - Q12. The enthalpy of solution for NaOH is –44.46...Ch. 12 - Q13. A 2.4 m aqueous solution of an ionic compound...Ch. 12 - Q14. A solution is an equimolar mixture of two...Ch. 12 - Prob. 15SAQ Ch. 12 - Prob. 1E Ch. 12 - Prob. 2E Ch. 12 - Prob. 3E Ch. 12 - Prob. 4E Ch. 12 - Prob. 5E Ch. 12 - Prob. 6E Ch. 12 - Prob. 7E Ch. 12 - Prob. 8E Ch. 12 - Prob. 9E Ch. 12 - 10. What is the heat of hydration (ΔHhydration)?...Ch. 12 - Prob. 11E Ch. 12 - Prob. 12E Ch. 12 - Prob. 13E Ch. 12 - Prob. 14E Ch. 12 - Prob. 15E Ch. 12 - Prob. 16E Ch. 12 - Prob. 17E Ch. 12 - Prob. 18E Ch. 12 - Prob. 19E Ch. 12 - Prob. 20E Ch. 12 - Prob. 21E Ch. 12 - 22. Explain why the lower vapor pressure for a...Ch. 12 - Prob. 23E Ch. 12 - Prob. 24E Ch. 12 - Prob. 25E Ch. 12 - Prob. 26E Ch. 12 - Prob. 27E Ch. 12 - Prob. 28E Ch. 12 - Prob. 29E Ch. 12 - 30. Pick an appropriate solvent from Table 13.3 to...Ch. 12 - 31. Which molecule would you expect to be more...Ch. 12 - 32. Which molecule would you expect to be more...Ch. 12 - Prob. 33E Ch. 12 - Prob. 34E Ch. 12 - 35. When ammonium chloride (NH4Cl) is dissolved in...Ch. 12 - 36. When lithium iodide (LiI) is dissolved in...Ch. 12 - Silver nitrate has a lattice energy of 820 kJ/mol...Ch. 12 - Prob. 38E Ch. 12 - Prob. 39E Ch. 12 - Prob. 40E Ch. 12 - Prob. 41E Ch. 12 - 42. A solution contains 32 g of KNO3 per 100.0 g...Ch. 12 - Prob. 43E Ch. 12 - Prob. 44E Ch. 12 - Prob. 45E Ch. 12 - Prob. 46E Ch. 12 - Prob. 47E Ch. 12 - Prob. 48E Ch. 12 - Prob. 49E Ch. 12 - Prob. 50E Ch. 12 - Prob. 51E Ch. 12 - Prob. 52E Ch. 12 - Prob. 53E Ch. 12 - Prob. 54E Ch. 12 - 55. Silver nitrate solutions are often used to...Ch. 12 - Prob. 56E Ch. 12 - Prob. 57E Ch. 12 - Prob. 58E Ch. 12 - Prob. 59E Ch. 12 - Prob. 60E Ch. 12 - Prob. 61E Ch. 12 - Prob. 62E Ch. 12 - Prob. 63E Ch. 12 - Prob. 64E Ch. 12 - Prob. 65E Ch. 12 - Prob. 66E Ch. 12 - Prob. 67E Ch. 12 - Prob. 68E Ch. 12 - Prob. 69E Ch. 12 - Prob. 70E Ch. 12 - 71. Calculate the vapor pressure of a solution...Ch. 12 - Prob. 72E Ch. 12 - 73. A solution contains 50.0 g of heptane (C7H16)...Ch. 12 - Prob. 74E Ch. 12 - 75. A solution contains 4.08 g of chloroform...Ch. 12 - Prob. 76E Ch. 12 - Prob. 77E Ch. 12 - Prob. 78E Ch. 12 - 79. Calculate the freezing point and boiling point...Ch. 12 - 80. Calculate the freezing point and boiling...Ch. 12 - 81. An aqueous solution containing 17.5 g of an...Ch. 12 - Prob. 82E Ch. 12 - 83. Calculate the osmotic pressure of a solution...Ch. 12 - Prob. 84E Ch. 12 - 85. A solution containing 27.55 mg of an unknown...Ch. 12 - Prob. 86E Ch. 12 - 87. Calculate the freezing point and boiling point...Ch. 12 - Prob. 88E Ch. 12 - Prob. 89E Ch. 12 - Prob. 90E Ch. 12 - Prob. 91E Ch. 12 - Prob. 92E Ch. 12 - Prob. 93E Ch. 12 - Prob. 94E Ch. 12 - 95. A 0.100 M ionic solution has an osmotic...Ch. 12 - Prob. 96E Ch. 12 - 97. Calculate the vapor pressure at 25 °C of an...Ch. 12 - Prob. 98E Ch. 12 - Prob. 99E Ch. 12 - 100. The solubility of phenol in water at 25 °C is...Ch. 12 - Prob. 101E Ch. 12 - Prob. 102E Ch. 12 - Prob. 103E Ch. 12 - Prob. 104E Ch. 12 - Prob. 105E Ch. 12 - Prob. 106E Ch. 12 - Prob. 107E Ch. 12 - 108. The vapor above an aqueous solution contains...Ch. 12 - Prob. 109E Ch. 12 - Prob. 110E Ch. 12 - Prob. 111E Ch. 12 - Prob. 112E Ch. 12 - Prob. 113E Ch. 12 - Prob. 114E Ch. 12 - Prob. 115E Ch. 12 - Prob. 116E Ch. 12 - Prob. 117E Ch. 12 - Prob. 118E Ch. 12 - Prob. 119E Ch. 12 - Prob. 120E Ch. 12 - Prob. 121E Ch. 12 - Prob. 122E Ch. 12 - 123. A 100.0-mL aqueous sodium chloride solution...Ch. 12 - Prob. 124E Ch. 12 - Prob. 125E Ch. 12 - Prob. 126E Ch. 12 - 127. A 1.10-g sample contains only glucose...Ch. 12 - 128. A solution is prepared by mixing 631 mL of...Ch. 12 - 129. Two alcohols, isopropyl alcohol and propyl...Ch. 12 - Prob. 130E Ch. 12 - Prob. 131E Ch. 12 - 132. A solution of 75.0 g of benzene (C6H6) and...Ch. 12 - Prob. 133E Ch. 12 - Prob. 134E Ch. 12 - Prob. 135E Ch. 12 - Prob. 136E Ch. 12 - 137. If each substance listed here costs the same...Ch. 12 - Prob. 138E

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