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Calculate AT from the temperatures extrapolated to the time of mixing: AT = temperature of mixture – average of temperatures of NaOH(aq) and HCl(aq) solutions Calculate the number of moles of H* neutralised: (HCI)/mol L-I Volume of HCl solution/mL = "HCI /mol (NAOHJ/mol L- Volume of NaOH solution/mL = "NAOH /mol = : Limiting reagent is Knowing which reagent is in excess, should the final solution be acidic or basic?. amount H* reacted/mol =

Calculate AT from the temperatures extrapolated to the time of mixing: AT = temperature of mixture – average of temperatures of NaOH(aq) and HCl(aq) solutions Calculate the number of moles of H* neutralised: (HCI)/mol L-I Volume of HCl solution/mL = "HCI /mol (NAOHJ/mol L- Volume of NaOH solution/mL = "NAOH /mol = : Limiting reagent is Knowing which reagent is in excess, should the final solution be acidic or basic?. amount H* reacted/mol =

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 white O transparent O blue (see page 96) NaOH(aq) + НCС(аq) > NaCl{aq) + H20() Concentration of HC(aq): 1.00 mol/L Concentration of NaOH(aq): 1.00 mol/L or ОН (аq) + Н (аq) — Н,0(0) Elapsed time / min 0.5 1.0 1.5 2.0 2,5 1. Clean and dry the calorimeter. Temperature of aqueous NaOH / °C 23.6 23.6 23.7 23.7 23.7 23.7 2. 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 exact concentration of the acid used onto your results page. Elapsed time / min 3.0 3.5 4.0 4.5 5.0 5.5 Temperature of HCI / °C 23.8 23.8 23.8 23.8 23.7 23.7 Starting timing (preferably using a stopwatch on a phone or tablet, or a real watch) and measure and record to 0.1 °C the temperature of the sodium hydroxide solution at 0.5 minute intervals for a total of 6 measurements. Wash and dry the thermometer. Next, measure and record the temperature of the hydrochloric acid solution at 0.5 minute intervals for 4. 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 / min 6.5 7.0 7.5 8.0 8.5 9.0 9.5 10.0 10.5 11.0 At time = 6.0 minutes (exactly, not earlier, not later), add the hydrochloric acid solution to the sodium hydroxide solution in the calorimeter. Mix well using a stirring rod or spatula and stir the solution for 15 seconds. 5. Temp. of mixture / °C 28.6 29.5 29.4 29.3 29.2 29.1 29.0 29.0 28.9 28.8 Caution: 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 solution between the temperature measurements. Continue to measure the temperature until a steady decrease in temperature is 6. AT =temperature of mixture – average of temperatures of NaOH(aq) and HCl(aq) solutions noted or until time = 11.0 minutes. Note: In order to obtain a smooth temperature curve you must stir the solution continuously between temperature measurements 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 pieces of 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 temperature at the time of mixing fits on the graph. "NaOH /mol = .. Limiting reagent is amount H' reacted/mol = 10. Extrapolate your lines to the time of mixing (time = 6.0 minutes) and determine the change in temperature as shown on the 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?
Transcribed Image Text: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 white O transparent O blue (see page 96) NaOH(aq) + НCС(аq) > NaCl{aq) + H20() Concentration of HC(aq): 1.00 mol/L Concentration of NaOH(aq): 1.00 mol/L or ОН (аq) + Н (аq) — Н,0(0) Elapsed time / min 0.5 1.0 1.5 2.0 2,5 1. Clean and dry the calorimeter. Temperature of aqueous NaOH / °C 23.6 23.6 23.7 23.7 23.7 23.7 2. 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 exact concentration of the acid used onto your results page. Elapsed time / min 3.0 3.5 4.0 4.5 5.0 5.5 Temperature of HCI / °C 23.8 23.8 23.8 23.8 23.7 23.7 Starting timing (preferably using a stopwatch on a phone or tablet, or a real watch) and measure and record to 0.1 °C the temperature of the sodium hydroxide solution at 0.5 minute intervals for a total of 6 measurements. Wash and dry the thermometer. Next, measure and record the temperature of the hydrochloric acid solution at 0.5 minute intervals for 4. 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 / min 6.5 7.0 7.5 8.0 8.5 9.0 9.5 10.0 10.5 11.0 At time = 6.0 minutes (exactly, not earlier, not later), add the hydrochloric acid solution to the sodium hydroxide solution in the calorimeter. Mix well using a stirring rod or spatula and stir the solution for 15 seconds. 5. Temp. of mixture / °C 28.6 29.5 29.4 29.3 29.2 29.1 29.0 29.0 28.9 28.8 Caution: 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 solution between the temperature measurements. Continue to measure the temperature until a steady decrease in temperature is 6. AT =temperature of mixture – average of temperatures of NaOH(aq) and HCl(aq) solutions noted or until time = 11.0 minutes. Note: In order to obtain a smooth temperature curve you must stir the solution continuously between temperature measurements 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 pieces of 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 temperature at the time of mixing fits on the graph. "NaOH /mol = .. Limiting reagent is amount H' reacted/mol = 10. Extrapolate your lines to the time of mixing (time = 6.0 minutes) and determine the change in temperature as shown on the 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?
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