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One desires to prepare a positively charged solution of silver iodide. This can be achieved by
- a)Adding a little AgNO3 solution to KI solution in slight excess
- b)Adding a little KI solution to AgNO3 solution in slight excess
- c)Mixing equal volumes of equimolar solutions of AgNO3 and KI
- d)None of these
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
One desires to prepare a positively charged solution of silver iodide....
KI + AgNO3 → AgI + KNO3
AgNO3 → Ag+ + NO3-
AgI(s) + Ag+ → [AgI] + Ag+.
AgNO3 → Ag+ + NO3-
AgI(s) + Ag+ → [AgI] + Ag+.
Most Upvoted Answer
One desires to prepare a positively charged solution of silver iodide....
Answer:
To prepare a positively charged solution of silver iodide, we need to consider the solubility and dissociation of the compounds involved.
Solubility and Dissociation:
- AgNO3 (silver nitrate) is a soluble compound that dissociates into Ag+ and NO3- ions.
- KI (potassium iodide) is also a soluble compound that dissociates into K+ and I- ions.
- AgI (silver iodide) is a sparingly soluble compound that dissociates into Ag+ and I- ions.
Formation of Positively Charged Solution:
In order to prepare a positively charged solution of silver iodide, we need to have an excess of Ag+ ions in the solution. This can be achieved by adding a little KI solution to AgNO3 solution in slight excess.
Explanation of Options:
a) Adding a little AgNO3 solution to KI solution in slight excess:
- This option would result in the formation of AgI, but it would not ensure the presence of excess Ag+ ions. Therefore, it does not fulfill the requirement of preparing a positively charged solution of silver iodide.
b) Adding a little KI solution to AgNO3 solution in slight excess:
- This option is correct because the addition of KI solution to AgNO3 solution in slight excess ensures the presence of excess Ag+ ions. This excess of Ag+ ions will combine with the I- ions from KI to form AgI, resulting in a positively charged solution.
c) Mixing equal volumes of equimolar solutions of AgNO3 and KI:
- This option does not fulfill the requirement of having an excess of Ag+ ions. The equal volumes of equimolar solutions would result in the formation of AgI, but it would not provide the desired positively charged solution.
d) None of these:
- This option is incorrect as option B is the correct answer.
Therefore, the correct answer is option B: Adding a little KI solution to AgNO3 solution in slight excess. This method ensures the presence of excess Ag+ ions, leading to the formation of a positively charged solution of silver iodide.
To prepare a positively charged solution of silver iodide, we need to consider the solubility and dissociation of the compounds involved.
Solubility and Dissociation:
- AgNO3 (silver nitrate) is a soluble compound that dissociates into Ag+ and NO3- ions.
- KI (potassium iodide) is also a soluble compound that dissociates into K+ and I- ions.
- AgI (silver iodide) is a sparingly soluble compound that dissociates into Ag+ and I- ions.
Formation of Positively Charged Solution:
In order to prepare a positively charged solution of silver iodide, we need to have an excess of Ag+ ions in the solution. This can be achieved by adding a little KI solution to AgNO3 solution in slight excess.
Explanation of Options:
a) Adding a little AgNO3 solution to KI solution in slight excess:
- This option would result in the formation of AgI, but it would not ensure the presence of excess Ag+ ions. Therefore, it does not fulfill the requirement of preparing a positively charged solution of silver iodide.
b) Adding a little KI solution to AgNO3 solution in slight excess:
- This option is correct because the addition of KI solution to AgNO3 solution in slight excess ensures the presence of excess Ag+ ions. This excess of Ag+ ions will combine with the I- ions from KI to form AgI, resulting in a positively charged solution.
c) Mixing equal volumes of equimolar solutions of AgNO3 and KI:
- This option does not fulfill the requirement of having an excess of Ag+ ions. The equal volumes of equimolar solutions would result in the formation of AgI, but it would not provide the desired positively charged solution.
d) None of these:
- This option is incorrect as option B is the correct answer.
Therefore, the correct answer is option B: Adding a little KI solution to AgNO3 solution in slight excess. This method ensures the presence of excess Ag+ ions, leading to the formation of a positively charged solution of silver iodide.
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One desires to prepare a positively charged solution of silver iodide. This can be achieved bya)Adding a little AgNO3solution to KI solution in slight excessb)Adding a little KI solution to AgNO3solution in slight excessc)Mixing equal volumes of equimolar solutions of AgNO3and KId)None of theseCorrect answer is option 'B'. Can you explain this answer?
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One desires to prepare a positively charged solution of silver iodide. This can be achieved bya)Adding a little AgNO3solution to KI solution in slight excessb)Adding a little KI solution to AgNO3solution in slight excessc)Mixing equal volumes of equimolar solutions of AgNO3and KId)None of theseCorrect 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 One desires to prepare a positively charged solution of silver iodide. This can be achieved bya)Adding a little AgNO3solution to KI solution in slight excessb)Adding a little KI solution to AgNO3solution in slight excessc)Mixing equal volumes of equimolar solutions of AgNO3and KId)None of theseCorrect 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 One desires to prepare a positively charged solution of silver iodide. This can be achieved bya)Adding a little AgNO3solution to KI solution in slight excessb)Adding a little KI solution to AgNO3solution in slight excessc)Mixing equal volumes of equimolar solutions of AgNO3and KId)None of theseCorrect answer is option 'B'. Can you explain this answer?.
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