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Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)
- a)200ml
- b)500ml
- c)400ml
- d)300ml
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydr...
N1V1 = N2V2
50 x 01 = 0.1 x Vml
Vm = 500ml
50 x 01 = 0.1 x Vml
Vm = 500ml
Most Upvoted Answer
Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydr...
Given:
Volume of calcium hydroxide solution = 50 mL
Molarity of calcium hydroxide solution = 0.5 M
Molarity of hydrochloric acid = 0.1 N
Calculation:
The balanced chemical equation for the reaction of calcium hydroxide with carbon dioxide is as follows:
Ca(OH)2 + CO2 → CaCO3 + H2O
From the equation, we can see that 1 mole of calcium hydroxide reacts with 1 mole of carbon dioxide to form 1 mole of calcium carbonate.
The number of moles of calcium hydroxide present in 50 mL of 0.5 M calcium hydroxide solution is given by:
n = M × V/1000 = 0.5 × 50/1000 = 0.025 moles
Since 1 mole of calcium hydroxide reacts with 1 mole of carbon dioxide, the number of moles of carbon dioxide required for complete reaction with 0.025 moles of calcium hydroxide is also 0.025 moles.
The volume of carbon dioxide required can be calculated using the ideal gas law as follows:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Assuming that the pressure and temperature are constant, we can write:
V = nRT/P
The volume of carbon dioxide required can be calculated as follows:
V = 0.025 × 0.082 × 298/1 = 0.609 L = 609 mL
Therefore, 609 mL of carbon dioxide is required for complete reaction with 50 mL of 0.5 M calcium hydroxide solution.
The balanced chemical equation for the reaction of calcium carbonate with hydrochloric acid is as follows:
CaCO3 + 2HCl → CaCl2 + H2O + CO2
From the equation, we can see that 1 mole of calcium carbonate reacts with 2 moles of hydrochloric acid to form 1 mole of calcium chloride, 1 mole of water, and 1 mole of carbon dioxide.
The number of moles of calcium carbonate formed from the reaction of 0.025 moles of calcium hydroxide with carbon dioxide is also 0.025 moles.
Therefore, the number of moles of hydrochloric acid required to completely neutralize 0.025 moles of calcium carbonate is given by:
n = 2 × 0.025 = 0.05 moles
The volume of 0.1 N hydrochloric acid required can be calculated as follows:
n = M × V/1000
V = n × 1000/M = 0.05 × 1000/0.1 = 500 mL
Therefore, the volume of 0.1 N hydrochloric acid required to completely neutralize the calcium carbonate formed from the reaction of 50 mL of 0.5 M calcium hydroxide with excess carbon dioxide is 500 mL. Hence, the correct option is (B).
Volume of calcium hydroxide solution = 50 mL
Molarity of calcium hydroxide solution = 0.5 M
Molarity of hydrochloric acid = 0.1 N
Calculation:
The balanced chemical equation for the reaction of calcium hydroxide with carbon dioxide is as follows:
Ca(OH)2 + CO2 → CaCO3 + H2O
From the equation, we can see that 1 mole of calcium hydroxide reacts with 1 mole of carbon dioxide to form 1 mole of calcium carbonate.
The number of moles of calcium hydroxide present in 50 mL of 0.5 M calcium hydroxide solution is given by:
n = M × V/1000 = 0.5 × 50/1000 = 0.025 moles
Since 1 mole of calcium hydroxide reacts with 1 mole of carbon dioxide, the number of moles of carbon dioxide required for complete reaction with 0.025 moles of calcium hydroxide is also 0.025 moles.
The volume of carbon dioxide required can be calculated using the ideal gas law as follows:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature.
Assuming that the pressure and temperature are constant, we can write:
V = nRT/P
The volume of carbon dioxide required can be calculated as follows:
V = 0.025 × 0.082 × 298/1 = 0.609 L = 609 mL
Therefore, 609 mL of carbon dioxide is required for complete reaction with 50 mL of 0.5 M calcium hydroxide solution.
The balanced chemical equation for the reaction of calcium carbonate with hydrochloric acid is as follows:
CaCO3 + 2HCl → CaCl2 + H2O + CO2
From the equation, we can see that 1 mole of calcium carbonate reacts with 2 moles of hydrochloric acid to form 1 mole of calcium chloride, 1 mole of water, and 1 mole of carbon dioxide.
The number of moles of calcium carbonate formed from the reaction of 0.025 moles of calcium hydroxide with carbon dioxide is also 0.025 moles.
Therefore, the number of moles of hydrochloric acid required to completely neutralize 0.025 moles of calcium carbonate is given by:
n = 2 × 0.025 = 0.05 moles
The volume of 0.1 N hydrochloric acid required can be calculated as follows:
n = M × V/1000
V = n × 1000/M = 0.05 × 1000/0.1 = 500 mL
Therefore, the volume of 0.1 N hydrochloric acid required to completely neutralize the calcium carbonate formed from the reaction of 50 mL of 0.5 M calcium hydroxide with excess carbon dioxide is 500 mL. Hence, the correct option is (B).
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Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)a)200mlb)500mlc)400mld)300mlCorrect answer is option 'B'. Can you explain this answer?
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Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)a)200mlb)500mlc)400mld)300mlCorrect answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)a)200mlb)500mlc)400mld)300mlCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)a)200mlb)500mlc)400mld)300mlCorrect answer is option 'B'. Can you explain this answer?.
Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)a)200mlb)500mlc)400mld)300mlCorrect answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)a)200mlb)500mlc)400mld)300mlCorrect answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Excess of carbon dioxide is passed through 50 mL of 0.5 M calcium hydroxide solution.After the composition of the reaction, the solutionwas evaporated to dryness. The solid calcium carbonate was completely neutralized with 0.1 N hydrochloric acid.The volume of the hydrochloric acid required is (At. mass of carbon = 40)a)200mlb)500mlc)400mld)300mlCorrect answer is option 'B'. Can you explain this answer?.
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