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Determination of enthalpy change of neutralization

Determination of enthalpy change of neutralization. vs. HCI(aq). NH. (aq). 3. Dilution of HCl(aq). 50.00 cm 3 of HCl(aq) was diluted to 250.0 cm 3 Pipette and pipette filler Volumetric flask. Standardization of HCl(aq). Burette End point of indicator Burette reading.

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Determination of enthalpy change of neutralization

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  1. Determination of enthalpy change of neutralization vs HCI(aq) NH (aq) 3

  2. Dilution of HCl(aq) • 50.00 cm3 of HCl(aq) was diluted to 250.0 cm3 • Pipette and pipette filler • Volumetric flask

  3. Standardization of HCl(aq) • Burette • End point of indicator • Burette reading

  4. CO32–(aq) + 2H+(aq) → CO2(g) + H2O(l) Mole ratio of CO32–(aq) to H+(aq) is 1 : 2

  5. Mixing different volumes of HCl(aq) and NH3(aq) • Measuring cylinder and dropper • Swirling the mixture • Taking thermometer readings

  6. Initial temperature should be taken • Recording the highest temperature

  7. Volume of ‘A’ used    / cm3 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 45.0 Volume of ‘B’ used / cm3 45.0 40.0 35.0 30.0 25.0 20.0 15.0 10.0 5.0  Maximum rise in temperature of the mixture / oC 1.3 2.5 3.9 5.4 6.3 5.1 3.5 2.3 1.2

  8. Graph • Maximum rise in temperature • Two straight lines are drawn • The lines pass through (0,0) and (50,0) • Intersection of the lines is the end point

  9. Calculation Enthalpy change of neutralization Negative sign kJ mol-1

  10. Another result The molarity of NH3(aq) can be calculated

  11. Other combinations • Using standard Na2CO3(aq) • HCl(aq) vs NH3(aq) • HCl(aq) vs NaOH(aq) • Using standard NaOH(aq) • CH3CO2H(aq) vs NH3(aq)

  12. Assessment • Completed within 90 minutes • Area A and area B both • Candidates’ performance • Standardization of HCl(aq) : fair • Enthalpy change : satisfactory • Graph and result : poor

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