What would be the formula or procedure to get iodine crystals from 3% tincture iodine?
407688
Couldn't you evaporate the solvent? I think it's water or ethanol.
168138
no it isn't. Iodine is the central atom and has 3 bonding pair and 2 nonbonding pair, a total of 5 pairs of electrons.\nthat would make it trigonal bipyramidal, more specifically we call it T shaped.
1053429
Iodine is the element.\n\nMixture of iodine? quite vague ha.\n\nWell, you've got a lot of choices:\n\nIodine Topical Solution and Iodine Tincture = contains, in each 100 mL, not less than 1.8 g and not more than 2.2 g of iodine (I), and not less than 2.1 g and not more than 2.6 g of Sodium Iodide (NaI).\n\nStrong Iodine Solution and Strong Iodine Tincture = contains, in each 100 mL, not less than 4.5 g and not more than 5.5 g of iodine (I), and not less than 9.5 g and not more than 10.5 g of Potassium Iodide (KI).\n\nNote: Of course these would have different solvents.
809008
is this your school homework,  are there suppossed to be other questions before these because my computer shows them starting from No. 4.\nnway,\n4.  filter the solution while still hot because as the soltion cools crystallization occurs, and you will nloose your product on the fiolter paper.\n5. crystallization can be induced by reduction in temperature i.e put in an ice bath or you can use a technique called seeding where you put a few crystals of the expected substance in the solution, the other method is to increase the concentration of the solution by evaporating it, to saturation point, ensure you do not evaporate it dry.\n6.i do not know what you started with so i can not tell.\n7.slow cooling will definately give bigger crystalls.\n8.sodium chloride reacts with silver nitrate to form a white precipitate, actually silver nitrate solution is used to analyse NaCl in industrial setting.\n\nope you will find these information sufficient.
302226
Name: iodine \nSymbol: I \nAtomic number: 53 \nAtomic weight: 126.90447 (3) \nCAS Registry ID: 7553-56-2 \n Group number: 17 \nGroup name: Halogen \nPeriod number: 5 \nBlock: p-block \n \nHere is a brief description of iodine.\n\nStandard state: solid at 298 K \nColour: violet-dark grey, lustrous \nClassification: Non-metallic \nIodine is a bluish-black, lustrous solid. It volatilises at ambient temperatures into a pretty blue-violet gas with an irritating odour.\n\nIt forms compounds with most elements, but is less reactive than the other halogens, which displace it from iodides. Iodine exhibits some metallic-like properties. It dissolves readily in chloroform, carbon tetrachloride, or carbon disulphide to form beautiful purple solutions. It is only slightly soluble in water. Iodine compounds are important in organic chemistry and very useful in medicine and photography. Lack of iodine is the cause of goitre (Derbyshire neck). The deep blue colour with starch solution is characteristic of the free element. It is assimilated by seaweeds from which it may be recovered, and is found in Chilean saltpetre, caliche, old salt brines, and salt wells.\n\nYou can never know too much :)
175854
http://en.wikipedia.org/wiki/Seed_crystal
934102
I know the answer......but I'm not going to give it. This line of questioning smacks of activities I'd rather not involve myself.\n\nIf you have a bonafide need for potassium iodide then purchasing it through legitimate channels is the easiest way.
288705
Iodine is a vital nutrient.  It is necessary for the function of the thyroid gland.  Since not everyone eats shellfish, which is a natural source, someone decided it would be a good idea to add it to table salt.\n\nSodium iodide is given for radiation exposure.  There are some communities near some nuclear reactors where the people are given sodium iodide tablets to take in case of a radiation release.  Although I am not sure of the exact mechanism, I believe that it is given because the iodine can bind with certain radioactive isotopes you may have inhaled (or otherwise gotten into your body) and help you eliminate it from your body before it can do a lot of harm.
862240
Depends on the ingredient.  Usual procedure is to chop the plant in a blender and extract the active principle with a suitable solvent, and then refine the extract with fractional crystallization, distillation, or other such means.
282140
iodine, prevents goiter and enhance the mind
853747
“Making your own Crystals”\n\nA crystal is a special kind of rock. Different crystals have different beautiful shapes and colors. \n\nWhat you'll need\n\n Your magnifying glass \n Table salt \n Epsom salt \n Honey jar \n Measuring cups and spoons \n Paper cut into circles \n Scissors \n Pencil \n String \n 1 3/4 cups of sugar \n 2 or 3 paper clips \n A glass jar or drinking glass \n Your science journal\n\nWhat to do\n\n \n\n1. Use your magnifying glass to look for crystals. Inspect: \n1. The table salt and Epsom salt; \n\nThe honey jar (particularly if it has been open for awhile) and \n\nThe walls of the freezer (if it's not the frost-free kind). \n\n1. Draw pictures of what you see in your science journal. \n1. Do all of the crystals look the same? \n1. If not, how are they different? \n1. Try dissolving salt crystals and forming new ones: \n1. Dissolve 1 teaspoon of salt in 1 cup of water\n1. Grown-up alert! \n\nHeat the mixture over a low flame to evaporate the water. \n\nWhat's left? \n\nWhat shape are these crystals? \n\n1. Snowflakes are made of ice crystals and are beautiful, but they are hard to see clearly. You can make paper snowflakes. \n1. Take a circle of paper (use thin paper) and fold it in half. Then fan fold it. \nMake cuts along all the edges. Unfold them. \n1. Grow rock candy crystals from dissolved sugar. \n\nGrown-up alert! \n\nPour a cup of boiling water into a dish and add 1 3/4 cups of sugar. Stir until the sugar is completely dissolved. Prepare a jar or glass as shown. \n\n\n\nWash the paper clips and use clean string. When the sugar water is cool, pour it into the jar and put it where no one will move it. Hang the paperclips in the water and put the pencil on top of the jar. \n\nSome crystals may form in a few hours. Some may grow to be half an inch on each side. To save them, take them out of the water and keep them dry. But they may disappear--they are good to eat. \n\nWhen certain liquids and gases cool and lose water, crystals are formed. Crystals are made up of molecules that fit neatly together in an orderly package. All crystals of the same material have the same shape, regardless of the size.
248245
Iodine is the least likely to form an iodide anion because it is the lest electronegative of the halogens. \n \nTHe halogens tend to want to draw and electron towards their neucleus.  Fluorine has the highest electronegativity.  It has a small electron cloud, so the outer most electrons are close to the nucleus and are more strongly pulled there.  Iodine has a large electron cloud.  The outer most electrons of iodine are much further away from the neuleus, so it can't pull electrons in as close.\n\nHope that helps.\n\nPS.  F, Cl, Br, and I all are diatomic, so they all form F2, Cl2, Br2, and I2.
340211
Yes. In fact you can buy iodine crystals in some sporting goods stores for use in water purification. These are not the tablets of NaI. They are crystals in a bottle, and must be soaked in the bottle, then the solution added to a quart of water, because iodine has a low solubility (0.03g/100g water).
991807
uh a pH meter will help with the hydrogen iodide because it's a strong acid.  As for the I2 I have no idea...
803319
Potassium Permanganate dissolves easily in water.  Iodine is only slightly soluble in water, but it dissolves really well in non-polar solvents such as ethanol, dichoromethane, etc.
767795
Pb2+ + 2I- <----> PbI2 (s)? \nMost often this reaction is shown as a double replacement reaction as follows:\n\nPb(NO3)2 + 2 KI ==> PbI2¯ + 2 KNO3   \nSince both solutions have to be heated before mixing, you might think it is an endothermic reaction requiring heat. However, the Lead Iodide precipitate will not form till the mixture is cooled. This would imply the reaction is actually endothermic since cooling or removing heat energy from the solution results in the precipitate.
1001051
Iodine is already diatomic in its solid state and same is true with bromine which is already diatomic in its liquid state.