Solving Stoichiometry Problems: Titrating Fe(NH4)2(SO4)2*6H2O with KMnO4

In summary, we discussed various aspects of titration, including how to determine the amount of KMnO4 needed to titrate a given amount of Fe(NH4)2(SO4)2*6H2O, writing a balanced net ionic equation using half reactions, calculating the molarity of a KMnO4 solution based on titration results, and the use of indicators in titrations. We also addressed why it is impossible to determine an accurate reading of the solution level in a buret if it is above the first mark or below the last mark, and the importance of recording the volume in the buret to the correct place value.
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3) how many mL of the 0.10M KMnO4 are needed to titrate 0.5g of Fe(NH4)2(SO4)2*6H2O

4) Using half reactions, write the balanced Net Ionic Equation for the following in a basicls solution:
KMnO4(aq) + Na2SO3(aq) + H2O(l) -> MnO2(s) + Na2SO4(aq) + KOH (aq)
Reduction: ??
Oxidation: ??

5) If 13.5 mL of a KMnO4 solution is titrated to the equivalence point with 8.75 mL of a 0.15M Na2SO3solution. What is the Molarity of the KMnO4 solution?

6) Why do we use an indicator in a titration and why is no indicator used in the titration of permanganate ion with iron (ii) ion?

7) During a titration, if the level of the solution in a 50 mL buret is above the first mark or below the last mark, why is it impossible to determine the precise reading?

8) To What place value should the volume in the 50 mL buret be recorded (included units)
 
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FAQ: Solving Stoichiometry Problems: Titrating Fe(NH4)2(SO4)2*6H2O with KMnO4

1. How do you determine the molarity of Fe(NH4)2(SO4)2*6H2O solution using titration with KMnO4?

In order to determine the molarity of Fe(NH4)2(SO4)2*6H2O solution, you will need to perform a titration with a known concentration of KMnO4. The titration involves adding KMnO4 solution to the Fe(NH4)2(SO4)2*6H2O solution until the reaction is complete. The endpoint is reached when the KMnO4 solution turns the solution a permanent light pink color. The moles of KMnO4 used can then be used to calculate the molarity of the Fe(NH4)2(SO4)2*6H2O solution.

2. What is the stoichiometric ratio between Fe(NH4)2(SO4)2*6H2O and KMnO4 in this titration?

The stoichiometric ratio between Fe(NH4)2(SO4)2*6H2O and KMnO4 can be determined from the balanced chemical equation for the reaction. In this case, the ratio is 1:5, meaning that for every 1 mole of Fe(NH4)2(SO4)2*6H2O, 5 moles of KMnO4 are required for the reaction to reach completion.

3. How do you calculate the mass of Fe(NH4)2(SO4)2*6H2O in a given sample using the molarity determined from titration?

To calculate the mass of Fe(NH4)2(SO4)2*6H2O in a given sample, you will need to use the molarity determined from the titration and the volume of the sample. Use the formula molarity = moles/volume to calculate the moles of Fe(NH4)2(SO4)2*6H2O. Then, use the molar mass of Fe(NH4)2(SO4)2*6H2O to convert moles to grams.

4. What is the purpose of using a standardized solution of KMnO4 in this titration?

The purpose of using a standardized solution of KMnO4 is to accurately determine the concentration of Fe(NH4)2(SO4)2*6H2O in a given sample. By using a solution with a known concentration of KMnO4, we can accurately measure the amount of KMnO4 used in the titration and use this information to calculate the concentration of Fe(NH4)2(SO4)2*6H2O in the original sample.

5. How do you handle sources of error in this titration, such as air bubbles or overtitration?

To minimize sources of error in this titration, it is important to take precise measurements and to perform the titration slowly and carefully. Air bubbles can be removed from the burette and other equipment before beginning the titration. If overtitration occurs, it is important to note the volume of KMnO4 used and to perform a back titration to accurately determine the endpoint. It is also important to perform multiple trials and calculate an average to reduce the impact of any potential errors.

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