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Citric acid, represented by H3Cit, is a triprotic acid. A student mixes together the following solutions in a styrofoam coffee cup: • 5.00 mL of 0.64 M citric acid

• 45.00 mL of 0.77 M NaOH

The two solutions start at a temperature of 25.5°C, and reach a final temperature of 27.8°C. The final, combined mixture has a mass of 51.6 grams and a specific heat of 4.0 J/g°C. Assume that no heat is transferred to the cup or surroundings.

a) Write a complete, balanced equation for the neutralization of citric acid (H3Cit) and NaOH.

b) Determine the total heat absorbed by the solution during this reaction.

c) Calculate the number of moles of citric acid that reacted.

d) Calculate the enthalpy of reaction, ?H, for this reaction in kJ/mol. Is the reaction exothermic or endothermic?

Chemistry, Academics

  • Category:- Chemistry
  • Reference No.:- M91101857

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