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When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured.
(Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)
Q.
The pH of the solution after Expt. 2 is
- a)2.8
- b)4.7
- c)5.0
- d)7.0
Correct answer is option 'B'. Can you explain this answer?
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When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an ins...
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When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an ins...
10-5) was mixed with 100 mL of 2.0 M NaOH in the same calorimeter at constant pressure. A temperature increase of 3.2oC was measured. Calculate the calorimeter constant.
First, we need to calculate the amount of heat released in Expt. 1:
moles of HCl = 0.1 L x 1.0 mol/L = 0.1 mol
moles of NaOH = 0.1 L x 1.0 mol/L = 0.1 mol
moles of HCl = moles of NaOH (1:1 stoichiometry)
heat released = -57.0 kJ/mol x 0.1 mol = -5.70 kJ
Next, we can use the heat released in Expt. 1 and the temperature change in Expt. 2 to calculate the calorimeter constant:
moles of acetic acid = 0.1 L x 2.0 mol/L = 0.2 mol
moles of NaOH = 0.1 L x 2.0 mol/L = 0.2 mol
moles of acetic acid = moles of NaOH (1:1 stoichiometry)
heat released = -5.70 kJ (from Expt. 1)
q = mcΔT, where q is heat, m is mass, c is specific heat, and ΔT is temperature change
Assuming the specific heat of the solution is the same as water (4.18 J/g°C):
q = (200 g + 200 g) x 4.18 J/g°C x 3.2°C = 5.34 kJ
Since the calorimeter is insulated and no heat is lost to the surroundings, the heat released in Expt. 1 is equal to the heat absorbed in Expt. 2:
-5.70 kJ = 5.34 kJ + CΔT
C = ( -5.70 kJ - 5.34 kJ ) / (0.0032 K) = 1.11 kJ/K
Therefore, the calorimeter constant is 1.11 kJ/K.
First, we need to calculate the amount of heat released in Expt. 1:
moles of HCl = 0.1 L x 1.0 mol/L = 0.1 mol
moles of NaOH = 0.1 L x 1.0 mol/L = 0.1 mol
moles of HCl = moles of NaOH (1:1 stoichiometry)
heat released = -57.0 kJ/mol x 0.1 mol = -5.70 kJ
Next, we can use the heat released in Expt. 1 and the temperature change in Expt. 2 to calculate the calorimeter constant:
moles of acetic acid = 0.1 L x 2.0 mol/L = 0.2 mol
moles of NaOH = 0.1 L x 2.0 mol/L = 0.2 mol
moles of acetic acid = moles of NaOH (1:1 stoichiometry)
heat released = -5.70 kJ (from Expt. 1)
q = mcΔT, where q is heat, m is mass, c is specific heat, and ΔT is temperature change
Assuming the specific heat of the solution is the same as water (4.18 J/g°C):
q = (200 g + 200 g) x 4.18 J/g°C x 3.2°C = 5.34 kJ
Since the calorimeter is insulated and no heat is lost to the surroundings, the heat released in Expt. 1 is equal to the heat absorbed in Expt. 2:
-5.70 kJ = 5.34 kJ + CΔT
C = ( -5.70 kJ - 5.34 kJ ) / (0.0032 K) = 1.11 kJ/K
Therefore, the calorimeter constant is 1.11 kJ/K.
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When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer?
Question Description
When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer?.
When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer?.
Solutions for When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer?, a detailed solution for When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice When 100 mL of 1.0 M HCl was mixed with 100 mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7oC was measured for the beaker and its contents (Expt. 1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol-1), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10-5) was mixed with 100 mL of 1.0 M NaOH (under identical conditions to Expt. 1) where a temperature rise of 5.6oC as measured. (Consider heat capacity of all solutions as 4.2 J g-1 K-1 and density of all solutions as 1.0 g mL-1)Q.The pH of the solution after Expt. 2 isa)2.8b)4.7c)5.0d)7.0Correct answer is option 'B'. Can you explain this answer? tests, examples and also practice JEE tests.
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