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

Enthalpy of Weak Base and Acid

Extracts from this document...

Introduction

Experiment 2: Enthalpy of Neutralization of Weak Acid with Weak Base ________________ Weak Base: Ammonium Hydroxide (NH4OH) Weak Acid: Acetic Acid (CH3CO2H) Reaction: NH4OH (aq) + CH3CO2H (aq) --> CH3COONH4 (aq) + H2O (l) Time (s) (±0.05s) Temperature (°C) (±0.05°C) Trial 1 Trial 2 Trial 3 Average Before adding base Initial Temperature 23 23 23 23 60 23 23 23 23 120 23 23 22.5 22.8 180 23 22.5 22.5 22.7 240 22.5 22.5 22.5 22.5 300 22.5 22.5 22 22.3 After adding base Peak Temperature 26.5 27.5 ...read more.

Middle

Least 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 = 10ml (± 0.5ml) ...read more.

Conclusion

OR 4.9K (± 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 = = = 0.01 moles (±0.0005 moles) Energy released per mole of hydrogen ions neutralized = = = 40960 J mol-1 or 40.96 kJ mol-1 ï41.0 kJ mol-1 Total uncertainty for enthalpy value = 20.4% + 5% + 5% = 30.4% Absolute uncertainty= ï The standard enthalpy change of neutralization of a weak acid (CH3CO2H) by a weak base (NH4OH) = -41.0 kJ mol-1 ± 12.5 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. The Enthalpy of Neutralization

    + HCl(aq)-->KCl(aq) + H2O(l) Finding the Moles of Water Moles of hydrochloric acid: [Volume x Concentration] 0.025dm3 x 2.00mol�dm-3 = 0.050mol HCl Moles of potassium hydroxide: [Volume x Concentration] 0.025dm3 x 2.00mol�dm-3 = 0.050mol KOH Moles of water: [Equal to moles of limiting reagent] 0.050mol H2O Calculating Enthalpy of Neutralization

  2. Thermodynamics: Enthalpy of Neutralization and Calorimetry

    At the end of the minutes the temperature of the solution is taken again. Measure the weight of calorimeter and of the NaCl. In order to find the heat of neutralization of the reaction though, we first need the specific heat of NaCl which is the next part of the experiment.

  1. Free essay

    Titration of a weak acid with a strong base

    Volume of weak acid: 25 ml Number of moles: 0.00366 mol Concentration =? c = n/v c = 0.00366/0.025 c = 0.146 moldm-3 (concentration of weak acid) In order to find out the weak acid, its pKa value should be determined.

  2. Analysis of the Standard Enthalpy of Combustion for Alcohols

    Calculating the temperature change for each trial of each alcohol Initial and final temperature of 100 cm3 ± 0.08 cm3 distilled water which had been heated for 180 seconds. methanol ethanol propan-1-ol butan-1-ol pentan-1-ol Temperature (°C ± 0.1 °C)

  1. The aim of this experiment is to examine the enthalpy of combustion of the ...

    Bond breaking is endothermic which means energy is given out to the surroundings. The more carbon atoms there are in a chain the more energy there will be given out to the surroundings through the breaking of bonds, therefore the greater the enthalpy change of combustion.

  2. Chemistry Titration Acid Base Lab

    + Na+(aq) + Cl-(aq) H+(aq) + OH-(aq) --> H2O(l) The first equation displays the reaction between the strong acid and strong base. The second reaction displays the HCl and NaOH dissociated in their respective ions. The last equation is known as the net ionic equation which eliminates the spectator ions from the previous equation.

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

    Then the rest of the hypothesis became wrong. Hence the second part of the hypothesis which claims that an increase in the fatty acid percentage will be harmful should be changed because of the new result. And the reason for that is the well-known harmful effect of repeatedly used vegetable oil.

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

    In fact, only water and no gas was produced. As time went by, the solution was turning milky white. This was due to the production of MgO which is white in color and since it is insoluble in water, it turns water milky.

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