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Complete the Table based on the picture (Heat Neutralization between a strong acid and a strong base) In calculating the mass of water in the mixture, assume that the volume of the solution is mainly from water and that the volume of HCl and NaOH are negligible. Also, assume that the density of water is 1 g/mL. Volume of HCl solution = 100 mL Volume of NaOH solution = 100 mL Total Volume of mixture= 200 mL Mass of Water in the mixture=  Initial temperature of Water= 20.0°C Final Temperature of Water = 23.41°C q water = q reaction= Molarity of HCl solution= 0.500 M Molarity of NaOH solution = 0.500M moles of HCl=  moles of NaOH= Limiting Reactant= moles of limiting reactant= ΔH reaction=

Complete the Table based on the picture (Heat Neutralization between a strong acid and a strong base) In calculating the mass of water in the mixture, assume that the volume of the solution is mainly from water and that the volume of HCl and NaOH are negligible. Also, assume that the density of water is 1 g/mL. Volume of HCl solution = 100 mL Volume of NaOH solution = 100 mL Total Volume of mixture= 200 mL Mass of Water in the mixture=  Initial temperature of Water= 20.0°C Final Temperature of Water = 23.41°C q water = q reaction= Molarity of HCl solution= 0.500 M Molarity of NaOH solution = 0.500M moles of HCl=  moles of NaOH= Limiting Reactant= moles of limiting reactant= ΔH reaction=

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Complete the Table based on the picture

(Heat Neutralization between a strong acid and a strong base)

In calculating the mass of water in the mixture, assume that the volume of the solution is mainly from water and that the volume of HCl and NaOH are negligible.

Also, assume that the density of water is 1 g/mL.

Volume of HCl solution = 100 mL

Volume of NaOH solution = 100 mL

Total Volume of mixture= 200 mL

Mass of Water in the mixture= 

Initial temperature of Water= 20.0°C

Final Temperature of Water = 23.41°C

q water =

q reaction=

Molarity of HCl solution= 0.500 M

Molarity of NaOH solution = 0.500M

moles of HCl= 

moles of NaOH=

Limiting Reactant=

moles of limiting reactant=

ΔH reaction=

Chemistry Simulations : Calorimetry Overview Learning Outcomes Experiment Experiment Step 5 Now that the experiment is complete, you can opt to show/hide the graph and/or microscopic views for subsequent runs. 23.4 1°C Click the Replay button to run the experiment again. 300mL I HCI (aq) IN2OH (ag) Click the Reset button to 200mL 600mL 500mL Time start a new experiment. 100ml The specific heat of the solution is assumed to be the 300mL 200ml same as water (4.184 J/g 100mL °C). LIQUIDS SOLIDS SOLUTIONS LIQUIDS SOLIDS SOLUTIONS HgO+ OH- Anion Cation H20 Hydrochloric acid - HCI (aq) Sodium hydroxide - NAOH (aq) RUN EXPERIMENT Vol (ml) X Show graph view 100. Vol (ml) 100. Molarity 0.500 Molarity 0.500 X Show microscopic view X Show specific heat (J/g°C) 4.184 | Show specific heat (J/g°C) 4.184 Replay Reset Temp erature
Transcribed Image Text:Chemistry Simulations : Calorimetry Overview Learning Outcomes Experiment Experiment Step 5 Now that the experiment is complete, you can opt to show/hide the graph and/or microscopic views for subsequent runs. 23.4 1°C Click the Replay button to run the experiment again. 300mL I HCI (aq) IN2OH (ag) Click the Reset button to 200mL 600mL 500mL Time start a new experiment. 100ml The specific heat of the solution is assumed to be the 300mL 200ml same as water (4.184 J/g 100mL °C). LIQUIDS SOLIDS SOLUTIONS LIQUIDS SOLIDS SOLUTIONS HgO+ OH- Anion Cation H20 Hydrochloric acid - HCI (aq) Sodium hydroxide - NAOH (aq) RUN EXPERIMENT Vol (ml) X Show graph view 100. Vol (ml) 100. Molarity 0.500 Molarity 0.500 X Show microscopic view X Show specific heat (J/g°C) 4.184 | Show specific heat (J/g°C) 4.184 Replay Reset Temp erature
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