In standardization of potassium tetraoxomaganate VII with ammonium iron II tetraoxosulphate VI , how do you find the molarity of the potassium tetraoxomanganate VII.
Can you answer these questions?
Question1
Ammonium chloride has the ability to
change directly from the solid to the gas state without using the heat.
A-True
B-False
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QUESTION 2
Which technique do you use to dry out the wet sand?
A/Filtration.
B/Decantation.
C/Using heat for sublimation.
D/Using heat for evaporation.
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QUESTION 3
When heating a mixture of salt, and ammonium chloride, which substance will be affected?
A/All of them.
B/Sand and salt only.
C/Sand only.
D/Ammonium chloride only.
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QUESTION 4
The chemical NH4Cl has the ability to:
A/Dissolves in water.
B/Sublimate when heated.
C/Melt when heated.
D/Evaporate when heated.
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QUESTION 5
A-Sand has the ability to
B-Dissolves in water
C-Sublimate when heated
D-Evaporate when heated
E-None of the above
To find the molarity of potassium tetraoxomanganate VII (KMnO4) using ammonium iron II tetraoxosulphate VI (Mohr's salt), you can follow the steps outlined below:
Step 1: Prepare a standard solution of Mohr's salt (Fe(NH4)2(SO4)2·6H2O) with a known concentration. This solution will be used to titrate the KMnO4 solution.
Step 2: Weigh a known mass of Mohr's salt and dissolve it in a volumetric flask with a specific volume of water. For example, if you have 0.2 moles of Mohr's salt dissolved in 1 liter (1000 mL) of water, it will give you a 0.2 M solution.
Step 3: Measure a specific volume of the prepared Mohr's salt solution using a pipette and transfer it to a conical flask. Let's say you measure 25 mL of the Mohr's salt solution.
Step 4: Add a few drops of concentrated sulfuric acid (H2SO4) to the conical flask. Sulfuric acid is added to create an acidic medium for the reaction to take place.
Step 5: Start titrating the Mohr's salt solution by adding KMnO4 solution from a burette in a slow and controlled manner. The reaction between the two is as follows:
Fe(NH4)2(SO4)2 + 6KMnO4 + 8H2SO4 -> K2SO4 + 4MnSO4 + 6H2O + Fe2(SO4)3 + 2(NH4)2SO4
The pink color of the KMnO4 solution will start to fade as the reaction proceeds.
Step 6: Continue adding KMnO4 solution drop by drop until the solution in the conical flask turns a pale pink color, indicating the endpoint of the reaction.
Step 7: Record the volume of KMnO4 solution used from the burette to reach the endpoint. Let's assume you used 15 mL of KMnO4 solution.
Step 8: Now, you can calculate the molarity of the KMnO4 solution using the following formula:
C1V1 = C2V2,
where C1 is the molarity of the Mohr's salt solution, V1 is the volume of Mohr's salt solution used (in liters), C2 is the molarity of KMnO4 solution, and V2 is the volume of KMnO4 solution used (in liters).
In this example, if you used 0.025 liters (25 mL) of the Mohr's salt solution and 0.015 liters (15 mL) of the KMnO4 solution, and the molarity of the Mohr's salt solution is 0.2 M, the calculation would be as follows:
(0.2 M) * (0.025 L) = (C2) * (0.015 L)
C2 = (0.2 M * 0.025 L) / (0.015 L)
C2 = 0.333 M
Therefore, the molarity of the KMnO4 solution is approximately 0.333 M.
To find the molarity of potassium tetraoxomanganate(VII) (also known as potassium permanganate) during its standardization with ammonium iron(II) tetraoxosulphate(VI) (also known as Mohr's salt), you generally use a redox titration method. Here's a step-by-step explanation:
1. Prepare a standard solution of Mohr's salt by accurately weighing a known mass of Mohr's salt crystals (Fe(NH₄)₂(SO₄)₂·6H₂O). Dissolve the crystals in distilled water and make up to a known volume in a volumetric flask (for example, 250 mL). Calculate the exact concentration of Mohr's salt using its molar mass and the total volume of the solution.
2. Prepare a solution of potassium permanganate (KMnO₄) of unknown concentration. This can be done by weighing a known mass of potassium permanganate and dissolving it in distilled water. Use the same volume of water as used for Mohr's salt solution (for example, 250 mL). The concentration of potassium permanganate is the value you are trying to determine.
3. Perform the redox titration by adding the potassium permanganate solution (unknown concentration) drop-wise to a measured volume of the Mohr's salt solution. The reaction between the two solutions is as follows:
5 Fe(NH₄)₂(SO₄)₂ + 2 KMnO₄ + 8 H₂SO₄ → 5 FeSO₄ + 2 MnSO₄ + K₂SO₄ + 10 NH₄HSO₄ + 8 H₂O
4. The reaction is complete when the pink color of the permanganate disappears, indicating the formation of a colorless manganese(II) sulfate. This indicates that all the Fe²⁺ ions have been oxidized to Fe³⁺ by the potassium permanganate.
5. Record the volume of the potassium permanganate solution used in the titration. This volume is required to calculate the molarity of the potassium permanganate.
6. Use the balanced equation to determine the mole ratio between the Mohr's salt and potassium permanganate. From this ratio and the volume of the potassium permanganate solution used, you can calculate the number of moles of potassium permanganate.
7. Finally, calculate the molarity of the potassium permanganate solution by dividing the number of moles of potassium permanganate by the volume of the solution used in the titration.
It is important to handle chemicals and perform titrations with care, following appropriate safety protocols and using the necessary equipment.