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2.538g in 1000ml.

If you are making this for a titration, like for SO2 or thiosulfate, you need also to add iodide:

1. dissolve 8 g potassium iodide in about 250 mL water.

2. add 2.538 g iodine to the water solution. Stir until dissolved.

3. transfer to a 1000 mL volumetric flask and Q.S. to 1000 mL

You should standardize vs. thiosulfate or arsenious oxide.

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What is the reason behind using 40 g of potassium iodide and 12.7 g of iodine to prepare 0.1 N of iodine?

- The atomic weight of iodine is 126,90447; for a 0,1 N solution, dividing by 10 the result is 12,69. - The iodide (KI) is added to increase the solubility of iodine in water or alcohol.


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Prepare 500ml of 0.12N HCL solution?

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What is the chemical name for Nitrogen Hydrogen and Iodine?

if by chemical name you mean element then: Nitrogen = N Hydrogen = H Iodine = I

Related Questions

How many grams of iodine would you weigh out to prepare 50 mL of a 0.200 N iodine solution?

To calculate the mass of iodine needed to prepare a 0.200 N solution in 50 mL, you can use the formula: Mass (g) = molarity (mol/L) * volume (L) * molar mass (g/mol). First, convert 50 mL to L (50 mL = 0.050 L). Then, substitute the values: Mass (g) = 0.200 mol/L * 0.050 L * 253.8 g/mol = 2.538 g of iodine. Therefore, you would weigh out 2.538 grams of iodine.


How do you make 1 liters of 0.02 N iodine solution?

To prepare 1 liter of a 0.02 N iodine solution, first calculate the amount of iodine (I2) needed. Since the normality of the solution is based on the equivalent weight of iodine, and considering that 1 equivalent of iodine corresponds to 1 mole of I2, you need 0.02 equivalents in 1 liter. This translates to 0.02 moles of I2, which is approximately 5.12 grams (molar mass of I2 is about 253.8 g/mol). Dissolve this amount of iodine in enough distilled water to make a final volume of 1 liter.


What is the reason behind using 40 g of potassium iodide and 12.7 g of iodine to prepare 0.1 N of iodine?

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Who to calculated normality of iodine?

Normality of iodine ((I_2)) can be calculated using the formula: Normality = Molarity x n, where n is the oxidation state of iodine in the reaction. For example, if you are using a 0.1 M (I_2) solution in a redox reaction where iodine is being reduced to iodide ions ((I^-)), then the normality of iodine would be 0.1 N.


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How do you prepare standard 0.1 N 100 ml Na2CO3 solution?

To prepare a 0.1 N 100 ml Na2CO3 solution, dissolve 5.3 grams of Na2CO3 in water and dilute to 100 ml. This will give you a solution with a concentration of 0.1 normal (N) for the 100 ml volume.


How do you prepare 1 N sodium bicarbonate?

To prepare a 1 N solution of sodium bicarbonate, dissolve 84 grams of sodium bicarbonate in enough water to make 1 liter of solution. This will give you a 1 N (equivalent to 1 mol/L) concentration.


How prepare 0.1 N oxalic acid?

To prepare 0.1 N oxalic acid solution, you would need to dissolve 0.634 g of oxalic acid dihydrate (H2C2O4·2H2O) in distilled water and make up the solution to a final volume of 1 liter. This will give you a 0.1 N (normality) solution of oxalic acid.


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To prepare a 0.02 N potassium permanganate solution, you would need to dissolve 1.58 grams of potassium permanganate (KMnO4) in 1 liter of distilled water. This will give you a solution with a molarity of 0.02 N. Remember to wear appropriate personal protective equipment when handling potassium permanganate, as it can be harmful.


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To prepare a 0.5 N acetic acid solution, first calculate the molarity needed using the formula Molarity (M) = Normality (N) x Equivalent weight. Then, use this information to dissolve the appropriate amount of acetic acid in water to make 1 liter of solution. Finally, adjust the volume with water as needed.


How many grams of iodine dissolved in water for 0.02 n iodine?

To calculate the grams of iodine dissolved in water for 0.02 N iodine, you need the molar mass of iodine, which is approximately 254 g/mol. With this information, you can use the formula: Grams = Normality (N) * Equivalent weight. Therefore, for 0.02 N iodine: Grams = 0.02 * 254 = 5.08 grams of iodine.


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