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50.0 mL of 1.45 mol/L NaOH and 50.0 mL of 1.45 mol/L HA are added to a coffee cup calorimeter, and the mixture was allowed to reach thermal equilibrium. Determine ΔrH°, in units of kJ mol–1, using the following data collected and assumptions made: The initial temperatures of both solutions were 24.00°C The final temperature of the mixture was 27.82°C Assume that the density and specific heat of the mixture is the same as that of water

50.0 mL of 1.45 mol/L NaOH and 50.0 mL of 1.45 mol/L HA are added to a coffee cup calorimeter, and the mixture was allowed to reach thermal equilibrium. Determine ΔrH°, in units of kJ mol–1, using the following data collected and assumptions made: The initial temperatures of both solutions were 24.00°C The final temperature of the mixture was 27.82°C Assume that the density and specific heat of the mixture is the same as that of water

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section4.8: Measuring Reaction Enthalpies: Calorimetry
Problem 4.17E
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Sodium hydroxide reacts with a monoprotic weak acid HA according to the following balanced chemical reaction:

            NaOH(aq)  +  HA(aq)  →   NaA(aq)  +  H2O(l)        ΔrH° = ?

 

50.0 mL of 1.45 mol/L NaOH and 50.0 mL of 1.45 mol/L HA are added to a coffee cup calorimeter, and the mixture was allowed to reach thermal equilibrium. Determine ΔrH°, in units of kJ mol–1, using the following data collected and assumptions made:

  • The initial temperatures of both solutions were 24.00°C
  • The final temperature of the mixture was 27.82°C
  • Assume that the density and specific heat of the mixture is the same as that of water (0.9970 g/mL, 4.184 J g–1 °C–1) 
  • Assume that no heat is lost to the surroundings.
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