How can you solve for miles of acid neutralized? And the netball of neautralization perature after mixing mL Heat Released Moles of NaOH (s) dissolved Enthalpy of solution per mole of NaOH (s), AHi 5.00 moles kJ/mole Reaction 2 Mass of NaOH (s) (1XX, XX-last 2 digits of ID#) volume of 1.0 M HCl measured (4X.0, X is the last digit of ID #) Initial temperature of 1.0 M HCI Temperature after mixing Heat Released Moles of NaOH (s) used Moles of HCI used Moles of acid Neutralized Enthalpy of Neutralization, AH2 mL ëë,ISL °c 635moles moles kJ/mole mL mL oC OC eaction3 40.0 olume of 1.0 M HCI measured f 1 0 M NaOH (4X.ON is the last digit of ID#)
How can you solve for miles of acid neutralized? And the netball of neautralization
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Related questions
Part A
The aluminum cup inside your calorimeter weighs 40.95 g. You add 59.21 g of 1.0 M acetic acid solution and 49.03 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 20.0 oC, and the final temperature after addition is 26.8 oC. What is the heat of neutralization for the amounts of reactants used, in units of J?
Assume that:
the calorimeter is completely insulated
the heat capacity of the empty calorimeter is the heat capacity of the aluminum cup.
the density of the two solutions is the same as that of water: 1.00 g/mL.
the heat capacity of the two slutions is the same as that of water: 4.184 J g-1oC-1.
Perform all calculations without rounding, but then provide your answer to the correct number of significant figures.
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Part B
What are the moles of the limiting reagent?
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Part C
What is the molar enthalpy of neutralization determined from the calorimeter experiment, in units of kJ/mol?
Use unrounded values in your calculation, but then provide your answer to the correct number of significant figures.