• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Enthalpy of Neutralization of Strong Base and Acid

Extracts from this document...


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.


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.


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.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. IB IA: Determination of Heat of Neutralization

    57 HNO3(aq) + 1/2 Ba(OH)2(aq) � 1/2 Ba(NO3)2(aq) + H2O(l) 57 3. From the above table, we can conclude that standard enthalpy change of neutralization for reactions between strong acids and strong bases is theoretically 57kJmol-1. 4. However, all the 5 experiments have shown a significant deviation in terms of the value for the standard enthalpy change for neutralization.

  2. Thermodynamics: Enthalpy of Neutralization and Calorimetry

    Another 50 mL of water is placed on a heating plate until it reaches 65 C�, taken off, then its temperature is taken and allowed to rest until the temperature stops increasing (this temperature is recorded), and added into the calorimeter along with the cooler water.

  1. A Comparison of Strong and Weak Acids and Bases

    0.10 37701 H2O(l) - 48 NaOH(aq) 0.01 2969 NaOH(aq) 0.10 26531 Table 2.3: The conductivity of NH3(aq). Solution Concentration of solution / mol dm-3 Conductivity of solution / �s (� 20 �s ) NH3 (aq) 1.00 1138 Graph 2.3: A comparison of the conductivity of the CH3COOH(aq), HCl(aq) NH3(aq)

  2. Experimental Molar Enthalpy of Neutralization for Sodium Hydroxide Solution

    As mentioned earlier, the result in this lab is very rare. This is mainly due to the fact that the Styrofoam calorimeter used to conduct the calorimetric experiment most likely does not provide a perfectly sealed environment.

  1. Analysis of the Standard Enthalpy of Combustion for Alcohols

    17.1 34.7 23.4 21.0 31.6 Trial 3 initial 18.3 17.1 18.4 17.9 19.7 final 35.7 52.6 42.5 42.2 53.0 change (°C ± 0.2 °C) 17.4 35.5 24.1 24.3 33.3 *The value of initial temperature to 1 decimal place has been subtracted from the value to 1 decimal place of the

  2. Measuring the fatty acid percentage of the reused sunflower oil after numerous times of ...

    Hence the second part of the hypothesis tries to prove the harmfulness; this claim should has another assessment after the new part. As the human mechanism needs free fatty acids as an important source of ATP and the heart and skeletal muscle prefer them as an energy source, a decrease

  1. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

    The value for ΔHMgO was determined to be -432.2±72.3kJ.mol-1. This means that according to this experiment, the value of ΔHMgO lies anywhere from -359.9 kJ.mol-1 to -504.5kJ.mol-1. The literature value for ΔHMgO was given to be -601.2kJ.mol-1 therefore the value in the range closest to the literature value (-504.5kJ.mol-1)

  2. Chemistry Titration Acid Base Lab

    beaker during this process is accounted for by slowing pouring in the amount necessary in the burette for the trial to begin. One experimental error that was unavoidable was the cleaning of the burette before using it. It was necessary to clean the burette using water, as it may have had some residue or contamination from a previous experiment.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work