Explanation Given: Mass of nonelectrolyte ( m n ) is 35.9 g . Mass of water ( m w ) is 150 g . Freezing point of solution ( T solution ) is − 1.3 ∘ C . Explanation: Freezing point of water ( T pure ) is 0 ∘ C . One gram is equal to 10 − 3 kilograms. Convert grams to kilograms as follows: 150 g = 150 g × ( 10 − 3 kg 1 g ) = 0.15 kg Mass of water in kilograms ( m w ) is 0.15 kg . Calculate the molality of the solution as follows. Use the formula for depression in freezing point: Δ T f = K f × m Δ T f is the change in the temperature of freezing point, K f is the freezing point depression constant, and m is the molality. For water, K f = 1.86 ∘ C / m . Δ T f = T pure − T solution Substitute 0 ∘ C for T pure and − 1.3 ∘ C for T solution : Δ T f = 0 ∘ C − ( − 1.3 ∘ C ) = 1.3 ∘ C Substitute 1.86 ∘ C / m for K f and 1

Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Principles Of Chemistry: A Molecular Approach

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ISBN: 9780133890686

Author: Tro

Publisher: PEARSON

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Chapter 12, Problem 82E

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To determine: The molar mass of the nonelectrolyte.

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Chapter 12, Problem 81E

Chapter 12, Problem 83E

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Chapter 12 Solutions

Masteringchemistry With Pearson Etext -- Valuepack Access Card -- For Principles Of Chemistry: A Molecular Approach

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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