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The minimum number of moles of solid KCl added to one liter contents of a standard silver …… silver ion electrode to convert it to standard silver …. silver chloride, electrode. [E° Ag+/Ag = 0.8V, Ksp (AgCl) = 10–10] are
Correct answer is '2'. Can you explain this answer?
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The minimum number of moles of solid KCl added to one liter contents o...
Ksp(AgCl)=[Ag⊕][Clc−],KCl=1.00M
∴[Clc−]=1.00M
∴[Ag⊕]=Ksp[Clc−]=1.0�10−101.00=1.0=10−10
Ag⊕+e−→Ag Ec−.Ag⊕∣Ag=0.799V
∴E=Ec−−0.0591log.1[Ag⊕]
=0.799−0.0591log.1(0.10�10−10)
=0.799=0.592=0.207V
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The minimum number of moles of solid KCl added to one liter contents o...
The minimum number of moles of solid KCl added to one liter of a standard silver nitrate solution depends on the desired concentration of KCl in the final solution.
To calculate the minimum number of moles of KCl, we need to know the concentration of silver nitrate solution and the desired concentration of KCl.
Let's assume the concentration of the silver nitrate solution is C1 (in moles/L) and the desired concentration of KCl is C2 (in moles/L).
The balanced chemical equation for the reaction between silver nitrate (AgNO3) and potassium chloride (KCl) is:
AgNO3 + KCl → AgCl + KNO3
From the equation, we can see that the molar ratio between AgNO3 and KCl is 1:1.
Therefore, the minimum number of moles of KCl needed to react with the silver nitrate solution is equal to the number of moles of AgNO3 in the solution.
The number of moles of AgNO3 in one liter of the solution is given by:
moles of AgNO3 = C1 * 1 L
So, the minimum number of moles of KCl needed is also given by:
moles of KCl = moles of AgNO3 = C1 * 1 L
Therefore, the minimum number of moles of solid KCl needed to add to one liter of the silver nitrate solution is equal to the concentration of the silver nitrate solution in moles per liter.
To calculate the minimum number of moles of KCl, we need to know the concentration of silver nitrate solution and the desired concentration of KCl.
Let's assume the concentration of the silver nitrate solution is C1 (in moles/L) and the desired concentration of KCl is C2 (in moles/L).
The balanced chemical equation for the reaction between silver nitrate (AgNO3) and potassium chloride (KCl) is:
AgNO3 + KCl → AgCl + KNO3
From the equation, we can see that the molar ratio between AgNO3 and KCl is 1:1.
Therefore, the minimum number of moles of KCl needed to react with the silver nitrate solution is equal to the number of moles of AgNO3 in the solution.
The number of moles of AgNO3 in one liter of the solution is given by:
moles of AgNO3 = C1 * 1 L
So, the minimum number of moles of KCl needed is also given by:
moles of KCl = moles of AgNO3 = C1 * 1 L
Therefore, the minimum number of moles of solid KCl needed to add to one liter of the silver nitrate solution is equal to the concentration of the silver nitrate solution in moles per liter.
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The minimum number of moles of solid KCl added to one liter contents of a standard silver …… silver ion electrode to convert it to standard silver …. silver chloride, electrode. [E° Ag+/Ag = 0.8V, Ksp(AgCl) = 10–10] areCorrect answer is '2'. Can you explain this answer?
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The minimum number of moles of solid KCl added to one liter contents of a standard silver …… silver ion electrode to convert it to standard silver …. silver chloride, electrode. [E° Ag+/Ag = 0.8V, Ksp(AgCl) = 10–10] areCorrect answer is '2'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about The minimum number of moles of solid KCl added to one liter contents of a standard silver …… silver ion electrode to convert it to standard silver …. silver chloride, electrode. [E° Ag+/Ag = 0.8V, Ksp(AgCl) = 10–10] areCorrect answer is '2'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The minimum number of moles of solid KCl added to one liter contents of a standard silver …… silver ion electrode to convert it to standard silver …. silver chloride, electrode. [E° Ag+/Ag = 0.8V, Ksp(AgCl) = 10–10] areCorrect answer is '2'. Can you explain this answer?.
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