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.
- 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.
Iodine Value of Activated Carbon Apparatus: Volumetric flask, conical flask, beaker, burette, pipette, filter paper Reagents: * 0.1N Iodine solution ( 40 gm KI in 1 Ltr of Distilled water ). * 0.05N Sodium Thiosulphate solution (12.5 gm Na2S2O3.5H2O in 1 Ltr Distilled water) * 1% Starch solution * Activated carbon Procedure: I Standardisation of Iodine solution * Take 10c.c of 0.1N Iodine solution in conical flask. * Add 2 drops of Starch solution. * The pale yellow colour of Iodine Soln turns Blue. * Titrate with 0.05 N Sodium Thiosulphate till it becomes Colourless. * Burette reading corresponds to blank reading.(B) II * Weigh very accurately 0.2 gm of Activated carbon * Introduce it into the Iodine flask which should be completely dry * Add 40cc of 0.1N Iodine solution * Shake the flask for 4 minutes and filter it * Collect the filterate in a dry flask and Titrate 10cc of the filtrate against Standard Sodium thiosulphate solution using starch as indicator * Burette reading corresponds to (A) Calculations: Iodine value: C x Conversion factor; mg/gm Factor:Mol wt. of iodine (127) x normality of iodine x 40 / Wt. of carbon x Blank reading C=B-A This is dry basis test From Ishan Udyog Bhilai
Prepare 200 ml of 0.1 N / 0.1 M Ethyl Acetate1.96 ml pure ethyl acetate (M.W. 88.1, Sp. Gr. 0.9005 g/ml at 20°C) and make it up to 200 ml volume with distilled water.Your solution will be ready....
To prepare 500ml of 0.12N HCl solution, you will need to dilute a concentrated hydrochloric acid solution. To do this, measure out 2.5ml of concentrated HCl (37% w/w) and dilute it to 500ml with distilled water. Be sure to wear appropriate safety equipment and handle the acid with caution.
if by chemical name you mean element then: Nitrogen = N Hydrogen = H Iodine = I
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.
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.
- 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.
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.
To prepare 1 N ferrous ammonium sulfate solution, dissolve 392.15 g of the compound in distilled water and dilute to 1 L. This will yield a solution with a concentration of 1 N.
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.
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.
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.
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.
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.
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.
Add 100 mL of HCl 1 N in a 1 L volumetric flask, class A or B; add ca. 850 mL distilled water to the flask. Place the flask in a thermostat at 20 0C. After 30 min add slowly distilled water to the mark (1 L) and stir well the closed flask. Pour the solution in a bottle. Place a label with the date, concentration, name of the solution on the bottle.