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) + НCС(аq) NaCl{aq) + H20()Concentration of HC(aq):1.00 mol/LConcentration of NaOH(aq): 1.00 mol/LorОН (аq) + Н (аq) — Н,0(0)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 / min3.03.54.04.55.05.5Temperature 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 drythe thermometer. Next, measure and record the temperature of the hydrochloric acid solution at 0.5 minute intervals for4.Elapsed time al mixing = 6.0 min (it is important to mix the solutions al exactly 6.0 minules and then stir thoroughly.)a 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.Calculate AT from the temperatures extrapolated to the time of mixing:At time = 6.5 minutes, (and at further 0.5 minute intervals), measure the temperature of the solution. Stir the solutionbetween the temperature measurements. Continue to measure the temperature until a steady decrease in temperature is6.AT =temperature of mixture – average of temperatures of NaOH(aq) and HCl(aq) solutionsnoted 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.Calculate the number of moles of H* neutralised:[HCI]/mol L¬!Volume of HCl solution/mL =7.Rinse (under the tap) the temperature probe on the thermometer and dry it."HCI 'mol =8.Obtain a piece of blue litmus paper and a piece of red litmus paper. Transfer a drop of the final solution onto both piecesof litmus paper. Use the colours to determine whether the resultant solution is acidic or basic and record this in your[NAOH]/mol L-Volume of NaOH solution/mL =rерort.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."NaOH /mol =.. Limiting reagent isamount H' reacted/mol =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.Knowing which reagent is in excess, should the final solution be acidic or basic?11. Calculate the enthalpy change for the reaction by completing the calculations in the results pages.Is this consistent with your observations and why?

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) + НCС(аq) > NaCl{aq) + H20()Concentration of HC(aq):1.00 mol/LConcentration of NaOH(aq): 1.00 mol/LorОН (аq) + Н (аq) — Н,0(0)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 / min3.03.54.04.55.05.5Temperature 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 drythe thermometer. Next, measure and record the temperature of the hydrochloric acid solution at 0.5 minute intervals for4.Elapsed time al mixing = 6.0 min (it is important to mix the solutions al exactly 6.0 minules and then stir thoroughly.)a 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.Calculate AT from the temperatures extrapolated to the time of mixing:At time = 6.5 minutes, (and at further 0.5 minute intervals), measure the temperature of the solution. Stir the solutionbetween the temperature measurements. Continue to measure the temperature until a steady decrease in temperature is6.AT =temperature of mixture – average of temperatures of NaOH(aq) and HCl(aq) solutionsnoted 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.Calculate the number of moles of H* neutralised:[HCI]/mol L¬!Volume of HCl solution/mL =7.Rinse (under the tap) the temperature probe on the thermometer and dry it.&#34;HCI 'mol =8.Obtain a piece of blue litmus paper and a piece of red litmus paper. Transfer a drop of the final solution onto both piecesof litmus paper. Use the colours to determine whether the resultant solution is acidic or basic and record this in your[NAOH]/mol L-Volume of NaOH solution/mL =rерort.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.&#34;NaOH /mol =.. Limiting reagent isamount H' reacted/mol =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.Knowing which reagent is in excess, should the final solution be acidic or basic?11. Calculate the enthalpy change for the reaction by completing the calculations in the results pages.Is this consistent with your observations and why?

Accepted Answer

Interpretation:
To fill the details in the table.
Given data:
From the experimental steps, we can…