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Enthalpy of Neutralization of Strong Base and Acid

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Introduction

Experiment 1: Enthalpy of Neutralization of Strong Acid with Strong Base ________________ Strong Base: Sodium Hydroxide (NaOH) Strong Acid: Hydrochloric Acid (HCl) Reaction: HCl (aq) + NaOH (aq) --> NaCl (aq) + H2O (l) Time (sec) Temperature (°C) Trial 1 Trial 2 Trial 3 Average Before adding base Initial Temperature 26 27 28 27 60 26 27 28 27 120 26 27 28 27 180 26 26.5 27.5 26.7 240 25.5 26.5 27.5 26.5 300 25.5 26.5 27.5 26.5 After adding base Peak Temperature 29.5 30 31 30.2 ...read more.

Middle

count in Measuring cylinder = 1ml Uncertainty in measuring cylinder = ± 0.5ml Molarity of Acid = 1M Molarity of Base = 1M Processed Data To find enthalpy we can use this equation: Where E = Energy transfer between system and surroundings m = Mass of Substance c = Specific Heat capacity of substance âT = Change in Temperature Volume of solutions cup (Salt + Water) after reaction = 5ml (± 0.5ml) ...read more.

Conclusion

OR 3.7K (± 1K) Percentage error in mass of water: Percentage error in temperature: Percentage error in number of moles = Energy released in reaction: Moles of Hydrogen ions neutralized by Hydroxide ions = = = 0.005 moles (±0.0005 moles) Energy released per mole of hydrogen ions neutralized = = = 30940 J mol-1 or 30.94 kJ mol-1 ï30.9 kJ mol-1 Total uncertainty for enthalpy value = 27% + 10% + 10% = 47% Absolute uncertainty= ï The standard enthalpy change of neutralization of a strong acid (HCl) by a strong base (NaOH) = -30.9 kJ mol-1 ± 14.5 kJ/mol-1 The percentage error compared to literature value: ...read more.

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