Explanation Given: Mass ( HNO 2 ) = 7 .050 g Mass ( H 2 O ) = 1 .000 kg Freezing point, T f ( solution ) = − 0 .2929 ° C Molal freezing point depression constant, K f ( water ) = 1 .86 ° C/m Freezing point, T f ( water ) = 0 ° C Explanation: (1) Calculate the number of moles of HNO 2 dissolved in the solution as follows: n HNO 2 ( dissolved ) = m HNO 2 Molar mass (HNO 2 ) = 7 .050 g 47 .013 g/mol =0 .14996 mol (2) Molality of a solution is the number of moles of solute per kilogram of the solvent. Therefore, the molality of this solution is the number of moles of HNO 2 in the solution containing 1.000 kg water, which is 0 .14996 m . (3) Calculate the depression in freezing point ( Δ T f ) as follows: Δ T f = T f ( water ) − T f ( solution ) = 0 ° C − ( − 0 .2929 ° C ) = 0 .2929 ° C (4) The depression in freezing point for an ionic solution is given as follows: Δ T f = i × K f × m Here, Δ T f is the depression in freezing point, i is the van’t Hoff factor, K f is the molal freezing point depression constant, and m is the molality of the solution. Calculate the van’t Hoff factor ( i ) for HNO 2 in the solution as follows: i = Δ T f K f × m = 0

3rd Edition

ISBN: 9780321809247

Author: Nivaldo J. Tro

Publisher: Prentice Hall

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Chapter 12, Problem 114E

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To determine: Dissociated fraction of nitrous acid.

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Chapter 12, Problem 113E

Chapter 12, Problem 115E

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Chapter 12 Solutions

Chemistry: A Molecular Approach

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