I\'ll be doing a coffee cup calorimeter experiment tomorrowwith citric acid and

Question

I'll be doing a coffee cup calorimeter experiment tomorrowwith citric acid and NaOH to find the enthalpy of reaction(Hrxn) The balanced equation for this reaction is given asfollows: My job for prelab is to calculate what volume of each 0.5 Msolution of H3Cit and NaOH should be mixed to give atotal volume of 50.0mL and the reactants in the correctstoichiometry. I'm honestly stuck on this part. I don't know how to calculatethe volume for each reactant in the correct stoichiometry. Cansomebody help me? And also, when do I need to measure the initialtemperature for the solution? Is it just the roomtemperature? Thank you very much!

Explanation / Answer

Well you need 1 mole of H3Cit for every 3 moles ofNaOH. If each of the solutions is .5 M, then the volume of NaOH will alsobe 3 times the volume of the H3Cit. So if the volume of the H3Cit is x and the volume of theNaOH is 3x, then the total volume is 4x. If you need a total volume of 50.0 mL, then 50.0=4x x=12.5 So the volume of H3Cit that you need is 12.5 mL, and thevolume of NaOH that you need is 37.5 mL. The initial temperature of the solution is its temperature beforethe reaction occurs. It's probably somewhere around roomtemperature.

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