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Formula weight of KMnO4 is 158.04. The equivalent weight depends on the reaction involved. In acidic media it is (formula weight) /5, in neutral although this is more difficult to control it is the formula weight.
Knowing which type it is usually acidic as it is easier, you will need 158.04/5 X 0.2 = 6.32g.
Sulfuric acid is usually added in the titration to ensure the correct oxidation reaction is carried out.
Also note KMnO4 is not considered a primary standard so you should really filter the solution to remove any MnO2 caused by oxidation of organic impurites in the water you are using, and standardise the solution by titration against say oxalic acid. K
What else can I help you with?
How much grams of kmno4 to prepare 1000 ppm solution?
To prepare a 1000 ppm (parts per million) solution of KMnO4 (potassium permanganate), you need 1000 mg of KMnO4 per liter of solution. Since 1 gram equals 1000 mg, you would need 1 gram of KMnO4 dissolved in enough water to make a final volume of 1 liter. Therefore, to prepare a 1000 ppm solution, dissolve 1 gram of KMnO4 in 1 liter of water.
How many grams of KMnO4 should be used to prepare 2L of a 5M solution?
To prepare 2L of a 5M solution, you should put in 4.6575grams of KMnO4. It is important to make sure that you add them in that order. K should be added first, then Mn.
How do you prepare 0.05 N solution of KMnO4?
To prepare a 0.05 N solution of KMnO4, you would need to weigh out the appropriate amount of KMnO4 based on its molar mass. Dissolve this calculated amount in a known volume of water, usually in a volumetric flask, and make up the volume to the desired final volume with more water. Thoroughly mix the solution to ensure uniform concentration.
What mass of KMnO4 is required to prepare 3.00 liters of a 0.05253 M solution of KMnO4?
To find the mass of KMnO4 needed, you can use the formula: mass = molarity x volume x molar mass. First, calculate the moles of KMnO4 using moles = molarity x volume. Then, multiply the moles by the molar mass of KMnO4 to find the mass needed.
How do you prepare 120 N solution of kmno4?
To prepare a 120 N (normal) solution of potassium permanganate (KMnO4), you need to calculate the required mass based on the desired volume of the solution. The normality (N) refers to the number of equivalents per liter; for KMnO4, one equivalent corresponds to one mole since it acts as a strong oxidizing agent. First, determine the molar mass of KMnO4 (approximately 158.04 g/mol), then calculate the mass needed using the formula: mass (g) = normality (N) × equivalent weight (g/equiv) × volume (L). Finally, dissolve the calculated mass of KMnO4 in distilled water to achieve the final volume.
You have .2 n kmno4 which you have to dilute it to 0.05n kmno4 how can you dilute that?
To dilute 0.2N KMnO4 to 0.05N KMnO4, you can add 4 times the volume of water to the original volume of KMnO4 solution. For example, if you have 100 mL of 0.2N KMnO4, you would add 400 mL of water to achieve a 0.05N KMnO4 solution. Mix thoroughly to ensure uniform dilution.
What is molarity of a solution that contains 0.798 g KMnO4 in 50.0 mL solution?
The molar mass of KMnO4 is 158,3415 g.The molarity of this solution is 0,1 M.
Why is it permissible to use a wet bottle when first obtaining your KMnO4 solution?
It is permissible to use a wet bottle when first obtaining your KMnO4 solution because the potassium permanganate (KMnO4) is not affected by water and will still dissolve properly in the solution.
What happens when ethanol is oxidised with acidified kmno4 solution?
When ethanol is oxidized with acidified KMnO4 solution, it undergoes complete oxidation to form ethanoic acid (acetic acid). The purple KMnO4 solution is reduced to green Mn2+ ions in the process.
Is KMnO4 soluble or not soluble is cyclohexane?
No the purple solid KMnO4 is only very slightly soluble in the organic liquid cyclohexane.
How do you prepare 100 ml of 1 in 1000 KMnO4?
700gram = 0.7 kilogram
How to prepare 100 ppm solution of KMnO4?
I will assume that you will start from the crystals of permanganate: Calculations: M.M. potassium permanganate: 158.04 g/mol mol KMnO4 in 10mL sol'n: 1.5 mol/L x 10 mL x (1 L / 1000 mL) = 0.015 mol grams potassium permanganate: 0.015 mol x 158.04 g/mol = 2.3706 g / 10 mL sol'n Preparation: 1. Weigh out analytically 2.3706g KMnO4 into a 10 mL volumetric flask. 2. Dilute to the mark with dH2O.
