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The strength of an aqueous NaOH solution is most accurately determined by titrating:
(Note: Consider that an appropriate indicator is used.)
  • a)
    Aq. NaOH in a pipette and aqueous oxalic acid in a burette
  • b)
    Aq. NaOH in a burette and aqueous oxalic acid in a conical flask
  • c)
    Aq. NaOH in a burette and concentrated H2SO4 in a conical flask
  • d)
    Aq. NaOH in a volumetric flask and concentrated H2SO4 in a conical flask
Correct answer is option 'B'. Can you explain this answer?
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Most Upvoted Answer
The strength of an aqueous NaOH solution is most accurately determined...
The strength of an aqueous NaOH solution is most accurately determined by titrating:

To accurately determine the strength of an aqueous NaOH solution, a titration method is commonly used. In titration, a solution of known concentration is added to a solution of unknown concentration until the reaction between the two is complete. The point at which the reaction is complete is called the equivalence point, and it can be determined using an appropriate indicator.

a) Aq. NaOH in a pipette and aqueous oxalic acid in a burette:
In this setup, the concentration of NaOH is determined by adding a known volume of the NaOH solution to a burette and then titrating it with a solution of oxalic acid of known concentration. However, this method is not the most accurate because it is difficult to accurately measure the volume of the NaOH solution in a pipette.

b) Aq. NaOH in a burette and aqueous oxalic acid in a conical flask:
In this setup, the concentration of NaOH is determined by adding a known volume of the NaOH solution to a burette and then titrating it with a solution of oxalic acid of known concentration. The conical flask allows for better mixing of the solutions and provides a larger surface area for the indicator to react with the solutions. This setup is more accurate because the volumes can be measured more accurately in the burette.

c) Aq. NaOH in a burette and concentrated H2SO4 in a conical flask:
In this setup, concentrated sulfuric acid (H2SO4) is used instead of oxalic acid. While this setup can also be used for titration, it is not the most accurate for determining the strength of an aqueous NaOH solution. Concentrated H2SO4 can be hazardous to handle, and it may react differently with NaOH compared to oxalic acid.

d) Aq. NaOH in a volumetric flask and concentrated H2SO4 in a conical flask:
In this setup, the NaOH solution is prepared in a volumetric flask of known volume, and then a known volume of the NaOH solution is transferred to a conical flask for titration with concentrated H2SO4. While this setup may provide accurate results, it requires additional steps and equipment for preparing the NaOH solution in a volumetric flask.

Conclusion:
Out of the given options, option B (Aq. NaOH in a burette and aqueous oxalic acid in a conical flask) is the most accurate and commonly used method for determining the strength of an aqueous NaOH solution. The setup allows for precise measurement of volumes and provides better mixing of the solutions, leading to more accurate results.
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The strength of an aqueous NaOH solution is most accurately determined...
In the titration of oxalic acid (weak acid) with a strong base like NaOH, oxalic acid is taken in a conical flask and NaOH is taken in a burette.
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Titrations are one of the methods we can use to discover the precise concentrations of solution. A typical titration involves adding a solution from a burette to another solution in a flask. The endpoint of the titration is found by watching a colour change taking place. However, a problem arises when a suitable indicator cannot be found, or when the colour changes involved are unclear. In cases redox potential may sometimes come to the rescue.A particularly well known example (Fig.1) is a method of discovering the concentration of iron in a solution by titrating them with a solution of cerium (IV). The redox potential that areof interest here are EFe3+/Fe2+ = + 0.77 V and ECe4+/Ce3+ = + 1.61 V. These tell us that cercium (IV) ions are the oxidizing agents, and iron (II) ions are the reducing agent. They should react according to the equationFe2+ (aq) + Ce4+ (aq) Fe3+ (aq) + Ce3+ (aq)Now imagine that we know the concentration of the cerium (IV) ions solution in the burette. We want to measure the concentration of the iron (II) solution. If we add just one drop of the cerium (IV) solution from the bruette, some of the iron (II) ions will be oxidised. As a consequence the beaker would now contain a large number of unreacted ions, but also some iron (III) ions as well. All of the cerium (III). The solution in the beaker now represents an iron(III)/iron(II) half cell, although not at standard conditions. Thus the e.m.f. of the cell will be near, but not equal, to EFe3+/Fe2+.to ad cerium (IV) solution, the number of iron (II) ions is gradually reduced and eventually only a very few are left (Tabl e).At this stage the next few drops of cerium (IV) solution convert all the remaining iron (II) ions into iron (III), and some of the cerium (IV) ions are left unreacted. Once this happens we no longer ions and a smaller number of cerium (IV) ions. The solution in the beaker now behaves as a cerium (IV)/cerium (III) half-cell (although not a standard one).Just before all the iron (II) ions are converted into iron (III) we have a cell with an e.m.f.of around + 0.77 V. After all the iron (II) ions are oxidised, we have a cell with an e.m.f. of about + 1.61 V. This rapid rise in e.m.f. occurs with the addition of hust one drop of cerium (IV) solution. You should be able to understand why a graph of cell e.m.f. against volume ofcerium (IV) solution added looks like that of Fig. 2. The end point of the titration can be read from the graph and the concentration of the iron (II) solution calculated in the usual wayQ.Imagine you were given a solution of potassium dichromate (VI) in a beaker, and a solution of iron (II) sulphate in a burette. You do not know the concentration of dichromate (VI) ions, but the concentration of the iron (II) solution is known. Your task is to carry out a redox titration using the two solutions in order to determine the concentration of dichromate(VI) ions. Sketch a graph how the e.m.f. changes in the course of above titration. E Cr2O2-7/Cr3+ = 1.33 V, EFe3+/Fe2+ = 0.77 V.

Titrations are one of the methods we can use to discover the precise concentrations of solution. A typical titration involves adding a solution from a burette to another solution in a flask. The endpoint of the titration is found by watching a colour change taking place. However, a problem arises when a suitable indicator cannot be found, or when the colour changes involved are unclear. In cases redox potential may sometimes come to the rescue.A particularly well known example (Fig.1) is a method of discovering the concentration of iron in a solution by titrating them with a solution of cerium (IV). The redox potential that areof interest here are EFe3+/Fe2+ = + 0.77 V and ECe4+/Ce3+ = + 1.61 V. These tell us that cercium (IV) ions are the oxidizing agents, and iron (II) ions are the reducing agent. They should react according to the equationFe2+ (aq) + Ce4+ (aq) Fe3+ (aq) + Ce3+ (aq)Now imagine that we know the concentration of the cerium (IV) ions solution in the burette. We want to measure the concentration of the iron (II) solution. If we add just one drop of the cerium (IV) solution from the bruette, some of the iron (II) ions will be oxidised. As a consequence the beaker would now contain a large number of unreacted ions, but also some iron (III) ions as well. All of the cerium (III). The solution in the beaker now represents an iron(III)/iron(II) half cell, although not at standard conditions. Thus the e.m.f. of the cell will be near, but not equal, to EFe3+/Fe2+.to ad cerium (IV) solution, the number of iron (II) ions is gradually reduced and eventually only a very few are left (Tabl e).At this stage the next few drops of cerium (IV) solution convert all the remaining iron (II) ions into iron (III), and some of the cerium (IV) ions are left unreacted. Once this happens we no longer ions and a smaller number of cerium (IV) ions. The solution in the beaker now behaves as a cerium (IV)/cerium (III) half-cell (although not a standard one).Just before all the iron (II) ions are converted into iron (III) we have a cell with an e.m.f.of around + 0.77 V. After all the iron (II) ions are oxidised, we have a cell with an e.m.f. of about + 1.61 V. This rapid rise in e.m.f. occurs with the addition of hust one drop of cerium (IV) solution. You should be able to understand why a graph of cell e.m.f. against volume ofcerium (IV) solution added looks like that of Fig. 2. The end point of the titration can be read from the graph and the concentration of the iron (II) solution calculated in the usual wayQ.The cell shown below was set upWhat would be the cell e.m.f.? If potassium cyanide solution were added to the left hand half cell (with due care!), what would you expect to happen to the e.m.f. of the cell? E Br2/Br- = 1.07V and use data of previousquestion, if required.

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The strength of an aqueous NaOH solution is most accurately determined by titrating:(Note: Consider that an appropriate indicator is used.)a)Aq. NaOH in a pipette and aqueous oxalic acid in a buretteb)Aq. NaOH in a burette and aqueous oxalic acid in a conical flaskc)Aq. NaOH in a burette and concentrated H2SO4 in a conical flaskd)Aq. NaOH in a volumetric flask and concentrated H2SO4 in a conical flaskCorrect answer is option 'B'. Can you explain this answer?
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The strength of an aqueous NaOH solution is most accurately determined by titrating:(Note: Consider that an appropriate indicator is used.)a)Aq. NaOH in a pipette and aqueous oxalic acid in a buretteb)Aq. NaOH in a burette and aqueous oxalic acid in a conical flaskc)Aq. NaOH in a burette and concentrated H2SO4 in a conical flaskd)Aq. NaOH in a volumetric flask and concentrated H2SO4 in a conical flaskCorrect answer is option 'B'. 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 strength of an aqueous NaOH solution is most accurately determined by titrating:(Note: Consider that an appropriate indicator is used.)a)Aq. NaOH in a pipette and aqueous oxalic acid in a buretteb)Aq. NaOH in a burette and aqueous oxalic acid in a conical flaskc)Aq. NaOH in a burette and concentrated H2SO4 in a conical flaskd)Aq. NaOH in a volumetric flask and concentrated H2SO4 in a conical flaskCorrect answer is option 'B'. 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 strength of an aqueous NaOH solution is most accurately determined by titrating:(Note: Consider that an appropriate indicator is used.)a)Aq. NaOH in a pipette and aqueous oxalic acid in a buretteb)Aq. NaOH in a burette and aqueous oxalic acid in a conical flaskc)Aq. NaOH in a burette and concentrated H2SO4 in a conical flaskd)Aq. NaOH in a volumetric flask and concentrated H2SO4 in a conical flaskCorrect answer is option 'B'. Can you explain this answer?.
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