Molar heat of Neutralization
A student collected the following data while demonstrating the molar heat of neutralization of a monoprotic acid, HA, with NaOH. Calculate the molar heat of neutralization of this acid with NaOH. Assume that the specific heats of the solutions are the same as water
a) Temperature of HA and NaOH before mixing 23.7 degrees celcius
b) Concentration of HA 1.06M
c) Concentration of NaOH 1.12M
d)Volume of HA and NaOH used 50.0mL
e) Temperature after of calorimeter after mixing 29.7 degrees celcius
Calculate the molar heat of neutralization of this acid with NaOH
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1. Construct two plots with the following data a. plot 1: ΔT (oC) (y-axis) vs. moles of HCl (x-ax...
1. Construct two plots with the following data
a. plot 1: ΔT (oC) (y-axis) vs. moles of HCl
(x-axis)
b. plot 2: qrxn (yaxis) vs. moles of HCl (x-axis).
(Use equations 3 and 2 from the lab handout to calculate the y-axis
values and 100.0 g as the mass of the solution.)
2. The complete neutralization of 0.0482 moles of a monoprotic
acid (HA) with excess NaOH evolves 2.58 kJ of heat. What is the
molar heat of neutralization of...
Suppose you perform a calorimeter experiment to determine the molar heat of neutralization of an unknown...
Suppose you perform a calorimeter experiment to determine the molar heat of neutralization of an unknown acid, HA, with sodium hydroxide, NaOH. You mix 35.5 mL of 0.50 M HA with 56.7 mL of 0.75 M NaOH and calculate the heat of reaction as-2.1 kJ. What is the molar heat of neutralization (in kJ/mol) for the unknown acid? Type answer
A a. After having completed your experiment and calculated your Enthalpy of Neutralization, e usu-you are...
A a. After having completed your experiment and calculated your Enthalpy of Neutralization, e usu-you are told concentration of the NaOH solution you used was 5% less than indicated on its label and asked to recalculate your enthalpy of neutralization. Will the recalculated cment value be larger, smaller, or the same as you originally calculated? b. Now consider the HCl you used in your experiment, if the concentration was 5% higher than that stated on its label, what will be...
3) You would like to measure the heat of neutralization of an acid with a base....
3) You would like to measure the heat of neutralization of an acid with a base. You mix 225 mL each of 0.65 M HNO, and 0.65 M LiOH, both at a temperature of 18.1 °C in a calorimeter cup equilibrated to that same temperature. After following the temperature change for 10 min and extrapolating it back to the time of addition, you find that the "final temperature" after mixing was 22.3 °C. Previously, you measured the heat capacity of...
Part IlI Heat of Neutralization of Weak Acid, HC,H,O, and Strong Base, NaOH Balanced reaction: 1)...
Part IlI Heat of Neutralization of Weak Acid, HC,H,O, and Strong Base, NaOH Balanced reaction: 1) Temperature of S0 mL of 2.0 M HCHO, before misxing 2) Temperature of 50 mL of 2.0 M NaOH before mixing 3) Temperature of 100 mL of solution after mixing 4) Assume that the density (1.00 g/ml) and specific heat of the solution (4.184 1-g' C') are the same as pure water. The heat gained by the solution is Calculation Using the heat capacity....
74 EXPERIMENT 6 Introduction to Calorimetry Measurement of Enthalpy of Acid-Base Neutralization T...
74 EXPERIMENT 6 Introduction to Calorimetry Measurement of Enthalpy of Acid-Base Neutralization Trial 1 Trial 2 Initial concentration of acid Initial concentration of base Initial temperature of acid Initial temperature of base Final temperature of mixture Temperature change of calorimeter ΔΤ Specific heat of salt solution (Table 6.2) Moles of water formed Molar enthalpy of neutralization Report Measurement of Specific Heat Copper Unknown Mass of metal sample Initial temperature of calorimeter Temperature of boiling water Maximum temperature of calorimeter Specific...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 22.8*C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.53/°C. Density Aqueous Solution - 1.00 g/mL Specific Heat of water = 4.184J/g•°C a. What is the total amount of heat evolved in this reaction? b. If 148 mmol of the...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 23.9°C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.6J/°C. Density Aqueous Solution = 1.00 g/ml Specific Heat of water = 4.184 J/g °C Hide a. What is the total amount of heat evolved in this reaction? NG 3 b....
Our chemist found a solution of 0.333M H3PO4 (phosphoric acid) and another of 1.05M NaOH (amazing...
Our chemist found a solution of 0.333M H3PO4 (phosphoric acid) and another of 1.05M NaOH (amazing what you can find in the belly of a ship) and so she did an enthalpy of neutralization reaction using 50.0mL of each solution. (Phosphoric acid is a triprotic acid; each mole of acid can yield 3 moles of H+ ions.) Using the CRC Handbook at hand, the density and specific heats of the final solution were found to be 1.11 g/mL and 3.81...
Our chemist found a solution of 0.333M H3PO4 (phosphoric acid) and another of 1.05M NaOH (amazing...
Our chemist found a solution of 0.333M H3PO4 (phosphoric acid) and another of 1.05M NaOH (amazing what you can find in the belly of a ship) and so she did an enthalpy of neutralization reaction using 50.0mL of each solution. (Phosphoric acid is a triprotic acid; each mole of acid can yield 3 moles of H* ions.) Using the CRC Handbook at hand, the density and specific heats of the final solution were found to be 1.11 g/mL and 3.81...
1. Construct two plots with the following data
a. plot 1: ΔT (oC) (y-axis) vs. moles of HCl
(x-axis)
b. plot 2: qrxn (yaxis) vs. moles of HCl (x-axis).
(Use equations 3 and 2 from the lab handout to calculate the y-axis
values and 100.0 g as the mass of the solution.)
2. The complete neutralization of 0.0482 moles of a monoprotic
acid (HA) with excess NaOH evolves 2.58 kJ of heat. What is the
molar heat of neutralization of...
Suppose you perform a calorimeter experiment to determine the molar heat of neutralization of an unknown acid, HA, with sodium hydroxide, NaOH. You mix 35.5 mL of 0.50 M HA with 56.7 mL of 0.75 M NaOH and calculate the heat of reaction as-2.1 kJ. What is the molar heat of neutralization (in kJ/mol) for the unknown acid? Type answer
A a. After having completed your experiment and calculated your Enthalpy of Neutralization, e usu-you are told concentration of the NaOH solution you used was 5% less than indicated on its label and asked to recalculate your enthalpy of neutralization. Will the recalculated cment value be larger, smaller, or the same as you originally calculated? b. Now consider the HCl you used in your experiment, if the concentration was 5% higher than that stated on its label, what will be...
3) You would like to measure the heat of neutralization of an acid with a base. You mix 225 mL each of 0.65 M HNO, and 0.65 M LiOH, both at a temperature of 18.1 °C in a calorimeter cup equilibrated to that same temperature. After following the temperature change for 10 min and extrapolating it back to the time of addition, you find that the "final temperature" after mixing was 22.3 °C. Previously, you measured the heat capacity of...
Part IlI Heat of Neutralization of Weak Acid, HC,H,O, and Strong Base, NaOH Balanced reaction: 1) Temperature of S0 mL of 2.0 M HCHO, before misxing 2) Temperature of 50 mL of 2.0 M NaOH before mixing 3) Temperature of 100 mL of solution after mixing 4) Assume that the density (1.00 g/ml) and specific heat of the solution (4.184 1-g' C') are the same as pure water. The heat gained by the solution is Calculation Using the heat capacity....
74 EXPERIMENT 6 Introduction to Calorimetry Measurement of Enthalpy of Acid-Base Neutralization Trial 1 Trial 2 Initial concentration of acid Initial concentration of base Initial temperature of acid Initial temperature of base Final temperature of mixture Temperature change of calorimeter ΔΤ Specific heat of salt solution (Table 6.2) Moles of water formed Molar enthalpy of neutralization Report Measurement of Specific Heat Copper Unknown Mass of metal sample Initial temperature of calorimeter Temperature of boiling water Maximum temperature of calorimeter Specific...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 22.8*C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.53/°C. Density Aqueous Solution - 1.00 g/mL Specific Heat of water = 4.184J/g•°C a. What is the total amount of heat evolved in this reaction? b. If 148 mmol of the...
4. You mix 50.0 ml. of a weak monoprotic acid with 50.0 mL of NaOH solution in a coffee cup calorimeter. Both solutions and the calorimeter were initially at 23.9°C. The final temperature of the neutralization reaction was determined to be 41.2°C. The calorimeter constant was known to be 110.6J/°C. Density Aqueous Solution = 1.00 g/ml Specific Heat of water = 4.184 J/g °C Hide a. What is the total amount of heat evolved in this reaction? NG 3 b....
Our chemist found a solution of 0.333M H3PO4 (phosphoric acid) and another of 1.05M NaOH (amazing what you can find in the belly of a ship) and so she did an enthalpy of neutralization reaction using 50.0mL of each solution. (Phosphoric acid is a triprotic acid; each mole of acid can yield 3 moles of H* ions.) Using the CRC Handbook at hand, the density and specific heats of the final solution were found to be 1.11 g/mL and 3.81...
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