6.03 Calorimtery Honors Essay - 897 Words

The Dissolving of Solid Sodium Hydroxide in Water Procedure: 1. Measure out approximately 200 mL of distilled water and pour it into the calorimeter. Stir carefully with a thermometer until a constant temperature is reached. Record the volume of water and the constant initial temperature of the water on your data table. 2. Place a plastic measuring trough on top of the digital balance, and then zero the balance (press the tare button) so that the mass of the trough will be ignored and will not be added to the total mass measured by the balance. 3. Measure out approximately three to five scoops of solid sodium hydroxide and record the mass to your data table. 4. Place the solid sodium hydroxide into the water in the†¦show more content†¦The value determined in question 4 is the enthalpy change value you will need for Conclusion question 1 below. Part II The Reaction of Sodium Hydroxide Solution with Hydrochloric Acid Procedure: 1. Measure out approximately 100 mL of 0.50 M hydrochloric acid solution and 100 mL of 0.50 M sodium hydroxide solution. Record both volumes on your data table. 2. Pour the hydrochloric acid solution into the calorimeter. Measure and record the initial temperature of each solution and record on your data table. 3. Add the sodium hydroxide solution to the acid solution in the calorimeter and immediately replace the lid of the calorimeter. Stir the mixture and record the highest temperature reached. Data and Observations: Insert a complete data table, including appropriate significant figures and units, in the space below. Also include any observations that you made over the course of Part II. Calculations: 1. Write out a balanced equation for the reaction you investigated in Part II, including phase symbols. 2. Determine the enthalpy change of this reaction. The mass of the sodium hydroxide and the mass of the hydrochloric acid should be added together. 3. Determine the number of moles of NaOH. 4. Determine enthalpy per mole of NaOH. Show all of your work. 5. The value determined in question 4 is the enthalpy change value you will need for Conclusion question 1