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25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]
- a)0.14
- b)0.28
- c)0.35
- d)0.07
Correct answer is option 'D'. Can you explain this answer?
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Verified Answer
25ml of a solution of barium hydroxide on titration with a 0.1 molar s...
25 × N = 0.1 × 35 ; N = 0.14
Ba(OH)2 is diacid base hence N = M × 2 or M =
⇒ M = 0.07 M
Ba(OH)2 is diacid base hence N = M × 2 or M =
⇒ M = 0.07 MMost Upvoted Answer
25ml of a solution of barium hydroxide on titration with a 0.1 molar s...
Given:
Volume of barium hydroxide solution (V1) = 25 ml
Volume of hydrochloric acid solution (V2) = 35 ml
Molarity of hydrochloric acid solution (M2) = 0.1 M
To find:
Molarity of barium hydroxide solution (M1)
We can use the equation:
M1V1 = M2V2
Substituting the given values:
M1 * 25 ml = 0.1 M * 35 ml
Simplifying the equation:
M1 = (0.1 M * 35 ml) / 25 ml
M1 = 0.14 M
Therefore, the molarity of the barium hydroxide solution is 0.14 M.
Explanation:
In a titration, the reaction between the acid and base is a neutralization reaction. The balanced chemical equation for the reaction between barium hydroxide (Ba(OH)2) and hydrochloric acid (HCl) is:
Ba(OH)2 + 2HCl → BaCl2 + 2H2O
From the balanced equation, we can see that 1 mole of barium hydroxide reacts with 2 moles of hydrochloric acid. In the given question, we know the volume of hydrochloric acid used in the titration (35 ml), which means we have used 1/2 mole of hydrochloric acid.
Now, using the equation M1V1 = M2V2, we can calculate the molarity of barium hydroxide solution. By substituting the given values, we get the molarity of barium hydroxide as 0.14 M.
Therefore, the correct answer is option D) 0.07 M.
Volume of barium hydroxide solution (V1) = 25 ml
Volume of hydrochloric acid solution (V2) = 35 ml
Molarity of hydrochloric acid solution (M2) = 0.1 M
To find:
Molarity of barium hydroxide solution (M1)
We can use the equation:
M1V1 = M2V2
Substituting the given values:
M1 * 25 ml = 0.1 M * 35 ml
Simplifying the equation:
M1 = (0.1 M * 35 ml) / 25 ml
M1 = 0.14 M
Therefore, the molarity of the barium hydroxide solution is 0.14 M.
Explanation:
In a titration, the reaction between the acid and base is a neutralization reaction. The balanced chemical equation for the reaction between barium hydroxide (Ba(OH)2) and hydrochloric acid (HCl) is:
Ba(OH)2 + 2HCl → BaCl2 + 2H2O
From the balanced equation, we can see that 1 mole of barium hydroxide reacts with 2 moles of hydrochloric acid. In the given question, we know the volume of hydrochloric acid used in the titration (35 ml), which means we have used 1/2 mole of hydrochloric acid.
Now, using the equation M1V1 = M2V2, we can calculate the molarity of barium hydroxide solution. By substituting the given values, we get the molarity of barium hydroxide as 0.14 M.
Therefore, the correct answer is option D) 0.07 M.
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25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer?
Question Description
25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. 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 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer?.
25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. 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 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer?.
Solutions for 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer? in English & in Hindi are available as part of our courses for JEE.
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25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer?, a detailed solution for 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer? has been provided alongside types of 25ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a litre value of 35ml. The molarity of barium hydroxide solution was [2003]a)0.14b)0.28c)0.35d)0.07Correct answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
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