A permanganate solution was standardized by titrating with sodium oxalate. A primary standard...
Question:
A permanganate solution was standardized by titrating with sodium oxalate. A primary standard sodium oxalate {eq}(Na_2C_2O_4) {/eq} was accurately weighed into a conical flask and dissolved with 100 mL of 3 M sulphuric acid. Then the solution was titrated with the permanganate solution. The weight of sodium oxalate used was 0.2408 grams, and the volume of permanganate solution in this titration was 17.76 mL. Calculate the molarity of the standard potassium permanganate solution.
{eq}2MnO_4^- + 5C_2O_4^{2-} + 16H^+ \to 2Mn^{2+} + 10CO_2 + 8H_2O {/eq}
Equivalence Point:
Any type of titration experiment is always performed until an equivalence point is reached. Sometimes this is referred to as the "endpoint" if some form of indicator chemical is used. The equivalence point is important because at this point the titrant and analyte reactants fully consume each other. Therefore only the products remain and you can relate the known moles of your standardized component to the unknown moles of your other component.
Answer and Explanation: 1
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This is a redox titration experiment between the oxalate ion and permanganate ion. The main products formed are manganese (II) cation and carbon...
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Equivalence Point: Definition & Calculation
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Chapter 12 / Lesson 11
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Learn about equivalence point and end point in titrations. Examine how to find equivalence points in a variety of ways, and discover the steps to do so.
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