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Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicator
- a)Magnesium–indicator complex is more stable than the magnesium–EDTA complex
- b)At the end point, the colour changes from red to blue
- c)After the end point, the colour of the solution is due to the indicator
- d)pH range of 7 – 10.5 is necessary for observing the specific colour change
Correct answer is option 'B,C,D'. Can you explain this answer?
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Choose the CORRECT answer(s) with respect to the magnesium-EDTA titrat...
The correct answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 are:
1) The formation of the magnesium-EDTA complex is favored at pH 7.
EDTA (Ethylenediaminetetraacetic acid) forms a complex with magnesium ions in a 1:1 ratio. At pH 7, the EDTA molecule exists in its fully ionized form, with four carboxylate groups being negatively charged. This helps in the chelation (binding) of magnesium ions, forming a stable complex.
2) The endpoint of the titration can be detected using an indicator.
In a magnesium-EDTA titration, a metal indicator such as Eriochrome Black T (EBT) or Calmagite is commonly used. These indicators change color when they react with free magnesium ions. The color change indicates the endpoint of the titration, where all the magnesium ions have been complexed with EDTA.
3) The reaction between magnesium and EDTA is a complexometric reaction.
Complexometric titrations involve the formation of a complex between a metal ion and a chelating agent (in this case, magnesium and EDTA). The complexation reaction is usually reversible, and the formation of the complex is used to determine the concentration of the metal ion.
4) The pH range of 7 is chosen to ensure that the reaction proceeds rapidly and completely.
At pH 7, the magnesium-EDTA complex formation is optimized, and the reaction between magnesium and EDTA occurs rapidly and completely. This pH range provides the most accurate results in the titration.
1) The formation of the magnesium-EDTA complex is favored at pH 7.
EDTA (Ethylenediaminetetraacetic acid) forms a complex with magnesium ions in a 1:1 ratio. At pH 7, the EDTA molecule exists in its fully ionized form, with four carboxylate groups being negatively charged. This helps in the chelation (binding) of magnesium ions, forming a stable complex.
2) The endpoint of the titration can be detected using an indicator.
In a magnesium-EDTA titration, a metal indicator such as Eriochrome Black T (EBT) or Calmagite is commonly used. These indicators change color when they react with free magnesium ions. The color change indicates the endpoint of the titration, where all the magnesium ions have been complexed with EDTA.
3) The reaction between magnesium and EDTA is a complexometric reaction.
Complexometric titrations involve the formation of a complex between a metal ion and a chelating agent (in this case, magnesium and EDTA). The complexation reaction is usually reversible, and the formation of the complex is used to determine the concentration of the metal ion.
4) The pH range of 7 is chosen to ensure that the reaction proceeds rapidly and completely.
At pH 7, the magnesium-EDTA complex formation is optimized, and the reaction between magnesium and EDTA occurs rapidly and completely. This pH range provides the most accurate results in the titration.
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Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer?
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Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer?.
Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer?.
Solutions for Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? in English & in Hindi are available as part of our courses for IIT JAM.
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Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer?, a detailed solution for Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? has been provided alongside types of Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice Choose the CORRECT answer(s) with respect to the magnesium-EDTA titration carried out in the pH range 7 – 10.5, using Solochrome black as indicatora)Magnesium–indicator complex is more stable than the magnesium–EDTA complexb)At the end point, the colour changes from red to bluec)After the end point, the colour of the solution is due to the indicatord)pH range of 7 – 10.5 is necessary for observing the specific colour changeCorrect answer is option 'B,C,D'. Can you explain this answer? tests, examples and also practice IIT JAM tests.
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