Part A - AHfor Hydrochloric Acid reacting with Aqueous Sodium Hydroxide.PART A - AHfor Hydrochloric Acid reacting with aqueous Sodium Hydroxide.For students with student numbers ending in 1, 2, 4, 5, 7, 8, or 0.Type of calorimeter used: M whiteO transparentO blue(see page 96)NaOH(aq) + HСКаq) — NaCЦаq) + Hz0()Concentration of HCl(aq):1.00 mol/LConcentration of NaOH(aq): 1.00 mol/Lorон (аq) + H'(aq) Н200)Elapsed time / min0.51.01.52.02.51.Clean and dry the calorimeter.Temperature of aqueous NaOH / °C23.623.623.723.723.723.72.Dispense 60 mL of the standardised sodium hydroxide solution directly into the dry, clean calorimeter.3.Dispense 50 mL of the standardised hydrochloric acid directly into a clean, dry beaker. Record in pen the exactconcentration of the acid used onto your results page.Elapsed time / min3.03.54.04.55.05.54.Temperature of HCI / °C23.823.823.823.823.723.7Starting timing (preferably using a stopwatch on a phone or tablet, or a real watch) and measure and record to 0.1 °Cthe temperature of the sodium hydroxide solution at 0.5 minute intervals for a total of 6 measurements. Wash and dryElapsed time at mixing = 6.0 min (it is important to mix the solutions al exactly 6.0 minules and then stir thoroughly.)the thermometer. Next, measure and record the temperature of the hydrochloric acid solution at 0.5 minute intervals fora total of 6 measurements.Elapsed time / min6.57.07.58.08.59.09.510.010.511.0At time = 6.0 minutes (exactly, not earlier, not later), add the hydrochloric acid solution to the sodium hydroxide solutionin the calorimeter. Mix well using a stirring rod or spatula and stir the solution for 15 seconds.5.Temp. of mixture / °C28.629.529.429.329.229.129.029.028.928.8Caution: Do not use the thermometer to stir the solution.Calculation of Enthalpy of Neutralisation6.At time = 6.5 minutes, (and at further 0.5 minute intervals), measure the temperature of the solution. Stir the solutionInclude units for all quantities you calculate. Keep intermediate results in your calculator to avoid round-off error and reporttheir values with 2 or 3 extra non-significant digits. Report the final molar enthalpy change with an appropriate number ofsignificant digits.between the temperature measurements. Continue to measure the temperature until a steady decrease in temperature isnoted or until time = 11.0 minutes.Note: In order to obtain a smooth temperature curve you must stir the solution continuously between temperaturemeasurements and keep the thermometer in the solution the whole time.1.Use the total volume of solution and its density to calculate the mass of the final solution:Rinse (under the tap) the temperature probe on the thermometer and dry it.Volume of final solution/mL =Density = 1.02 g mL at 20 °C7.8.Obtain a piece of blue litmus paper and a piece of red litmus paper. Transfer a drop of the final solution onto both piecesMass of final solution =of litmus paper. Use the colours to determine whether the resultant solution is acidic or basic and record this in your2.Use the mass of the final solution, AT, and the specific heat capacity of the solution to calculate the heat absorbed by thereport.solution.9. Graph the results on the results page. Be sure to allow sufficient range on the temperature axis so that the temperatureat the time of mixing fits on the graph.- 4.04 J g KMass of final solution /g =10. Extrapolate your lines to the time of mixing (time = 6.0 minutes) and determine the change in temperature as shown onthe graph in the introduction.Heat absorbed by solution =11. Calculate the enthalpy change for the reaction by completing the calculations in the results pages.

Question

Part A - AHfor Hydrochloric Acid reacting with Aqueous Sodium Hydroxide.PART A - AHfor Hydrochloric Acid reacting with aqueous Sodium Hydroxide.For students with student numbers ending in 1, 2, 4, 5, 7, 8, or 0.Type of calorimeter used: M whiteO transparentO blue(see page 96)NaOH(aq) + HСКаq) —> NaCЦаq) + Hz0()Concentration of HCl(aq):1.00 mol/LConcentration of NaOH(aq): 1.00 mol/Lorон (аq) + H'(aq) > Н200)Elapsed time / min0.51.01.52.02.51.Clean and dry the calorimeter.Temperature of aqueous NaOH / °C23.623.623.723.723.723.72.Dispense 60 mL of the standardised sodium hydroxide solution directly into the dry, clean calorimeter.3.Dispense 50 mL of the standardised hydrochloric acid directly into a clean, dry beaker. Record in pen the exactconcentration of the acid used onto your results page.Elapsed time / min3.03.54.04.55.05.54.Temperature of HCI / °C23.823.823.823.823.723.7Starting timing (preferably using a stopwatch on a phone or tablet, or a real watch) and measure and record to 0.1 °Cthe temperature of the sodium hydroxide solution at 0.5 minute intervals for a total of 6 measurements. Wash and dryElapsed time at mixing = 6.0 min (it is important to mix the solutions al exactly 6.0 minules and then stir thoroughly.)the thermometer. Next, measure and record the temperature of the hydrochloric acid solution at 0.5 minute intervals fora total of 6 measurements.Elapsed time / min6.57.07.58.08.59.09.510.010.511.0At time = 6.0 minutes (exactly, not earlier, not later), add the hydrochloric acid solution to the sodium hydroxide solutionin the calorimeter. Mix well using a stirring rod or spatula and stir the solution for 15 seconds.5.Temp. of mixture / °C28.629.529.429.329.229.129.029.028.928.8Caution: Do not use the thermometer to stir the solution.Calculation of Enthalpy of Neutralisation6.At time = 6.5 minutes, (and at further 0.5 minute intervals), measure the temperature of the solution. Stir the solutionInclude units for all quantities you calculate. Keep intermediate results in your calculator to avoid round-off error and reporttheir values with 2 or 3 extra non-significant digits. Report the final molar enthalpy change with an appropriate number ofsignificant digits.between the temperature measurements. Continue to measure the temperature until a steady decrease in temperature isnoted or until time = 11.0 minutes.Note: In order to obtain a smooth temperature curve you must stir the solution continuously between temperaturemeasurements and keep the thermometer in the solution the whole time.1.Use the total volume of solution and its density to calculate the mass of the final solution:Rinse (under the tap) the temperature probe on the thermometer and dry it.Volume of final solution/mL =Density = 1.02 g mL at 20 °C7.8.Obtain a piece of blue litmus paper and a piece of red litmus paper. Transfer a drop of the final solution onto both piecesMass of final solution =of litmus paper. Use the colours to determine whether the resultant solution is acidic or basic and record this in your2.Use the mass of the final solution, AT, and the specific heat capacity of the solution to calculate the heat absorbed by thereport.solution.9. Graph the results on the results page. Be sure to allow sufficient range on the temperature axis so that the temperatureat the time of mixing fits on the graph.- 4.04 J g KMass of final solution /g =10. Extrapolate your lines to the time of mixing (time = 6.0 minutes) and determine the change in temperature as shown onthe graph in the introduction.Heat absorbed by solution =11. Calculate the enthalpy change for the reaction by completing the calculations in the results pages.

Accepted Answer

We need to determine the heat absorbed by the solution, and molar its enthalpy change.