Determination of Heat of Neutralization
PRACTICAL 15: DETERMINATION OF HEAT OF NEUTRALIZATION
Data collection:
|Reaction |Initial Temperature/°C (±0.25) |Final Temperature of Mixture/°C (±0.25) |
| |Acid |Base | |
|HNO3 + NaOH |28.00 |28.25 |34.50 |
|HNO3 + KOH |28.25 |28.25 |34.00 |
|HCl + NaOH |28.25 |28.00 |34.75 |
|HCl + KOH |28.25 |28.25 |34.00 |
|H2SO4 + NaOH |28.00 |28.50 |36.50 |
|H2SO4 + KOH |28.50 |28.00 |34.00 |
Volume of acid = 50 cm3 ± 0.25
Acid concentration = 1.0 M
Volume of base = 50cm3 ± 0.25
Base concentration = 1.0 M
Number of mole of solution used = [pic] = [pic] = 0.05 mole ± 0.5 %
Data Processing:
Calculation:
Temperature Change, [pic] = Final temperature – Average temperature of Acid and Base
|Reaction |Average Temperature of Acid and Base, °C|Final Temperature, °C |Change of Temperature, °C |
| |(±0.5) |(±0.25) |(±0.75) |
|HNO3 + NaOH |28.13 |34.50 |6.38 |
|HNO3 + KOH |28.25 |34.00 |5.75 |
|HCl + NaOH |28.13 |34.75 |6.63 |
|HCl + KOH
Data collection:
|Reaction |Initial Temperature/°C (±0.25) |Final Temperature of Mixture/°C (±0.25) |
| |Acid |Base | |
|HNO3 + NaOH |28.00 |28.25 |34.50 |
|HNO3 + KOH |28.25 |28.25 |34.00 |
|HCl + NaOH |28.25 |28.00 |34.75 |
|HCl + KOH |28.25 |28.25 |34.00 |
|H2SO4 + NaOH |28.00 |28.50 |36.50 |
|H2SO4 + KOH |28.50 |28.00 |34.00 |
Volume of acid = 50 cm3 ± 0.25
Acid concentration = 1.0 M
Volume of base = 50cm3 ± 0.25
Base concentration = 1.0 M
Number of mole of solution used = [pic] = [pic] = 0.05 mole ± 0.5 %
Data Processing:
Calculation:
Temperature Change, [pic] = Final temperature – Average temperature of Acid and Base
|Reaction |Average Temperature of Acid and Base, °C|Final Temperature, °C |Change of Temperature, °C |
| |(±0.5) |(±0.25) |(±0.75) |
|HNO3 + NaOH |28.13 |34.50 |6.38 |
|HNO3 + KOH |28.25 |34.00 |5.75 |
|HCl + NaOH |28.13 |34.75 |6.63 |
|HCl + KOH