Would solid Iodine dissolve in water? why or why not?
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).
135415
That's a difficult question to answer because magnesium hydroxide is practically insoluble in water with a ksp value of like 1.8 x 10^-11 so very little magnesium hydroxide is dissolved in water.  But if you were to compare the solubility of magnesium hydroxide at 25C with 80C my guess is that it would be more soluble at a higher temperature but only by an almost insignificant amount.  \n\nIn short, Mg(OH)2 is pretty much insoluble in water so my direct answer after all the reasoning would probably be: no, Mg(OH)2 does not fit the pattern due to its extremely low solubility.
6303
Silver iodide is released into the clouds which baically grabs hold of supercooled water droplets (water that is colder than ice but still liquid) and if the conditions are right, the supercooled water droplets will freeze, attract more water droplets and eventually form snowflakes....\n\nPlease understand that this is a very basic description but gives the idea...
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.
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.
874059
I think that isolating potassium is the wrong approach.  Potassium metal reacts with atmospheric water to form KOH and hydrogen gas.  If you accidentally get water on the metal the reaction is so vigourous that the metal will catch fire, which will be dangerous.  \n\nTry a different approach.  Dissolve KCl in water and add a molar equivalence of Silver iodide, AgI, also dissolved in water..  AgCl is nearly insoluble in water (~0.9 mg/L at 10C)  and will precipitate out, leaving KI in solution.  Filter out the AgCl and evaporate the water, leaving solid KI.  \n\nThe two biggest problems starting with KNO3 are:  It will be nearly impossible to salt out the nitrate because of its high solubility in salt form, and two, many nitrate salts, particularlyof metals, are highly explosive and dangerous.  KCl is cheap and plentiful, so why not just buy some?
44675
For starters, these bubbles are not coming from the oxygen present in H2O, or any transition from gas to liquid state. The amount of activation energy it would take to break the H2O bond (plus the surrounding hydrogen bonds) to send liquid Oxygen to gas form is not going to come from room temperature. More likely, the gas bubbles you see are dissolved air. Your water has gone through many filtration stops and a multitude of meshes, all of which can dissolve small microscopic bubbles of air in the water. These either come out to the water-air interface or combine with neighboring bubbles (I would guess this reduces surface tension). You see the larger air bubbles.
196494
No. It is not possible for the following reasons...\n1) Water is a compound, so it can only have molecules adn not atoms.\n2) The only atoms that you will get when you break down a water molecule are two atoms of hyderogen and one of oxygen\n3) What we get thru electric lines is only electrical energy. This is transferred by the vibration of the atoms in the cables used to supply electricity. So no atoms are actually sent accross\n4) Even if all these were possible, the procedure will be extremely expensive.
663838
I agree with Thinkstoomuch's Answers in most part.  \n\nSolid Cu, C will not be soluble in water.  However glucose and  CuBr2 will be soluble in water.  At STP solubility of glucose (C6H12O6) is about 90g/ml.  That eliminates choice 1 and 3.\n\nWhen a compound ionizes in soln it makes electrolyte.  Glucose will not ionize but CuBr2 will ionize to Cu++ and 2Br-, choice 4 can be eliminated.\n\nThe third clue is just there to confirm your answer and CuBr2 being an ionic compound will indeed have a relatively high melting point.  498°C to be exact.  \n\nClearly, Cupric Bromide should be your Answer.\n\nI hope this helps.
5530
Arsenic is the metal, but at temperatures much lower than its melting point (not boiling point).  It sublimes at 614 degrees C and melts under pressure at 817 degrees C.\n\nAlthough Iodine has a metallic luster, it is not a metal.  It sublimes (evaporates) near its \nMelting Point of 114 degrees C.\n\nSee the reference below:
986564
I'm not 100% sure, but it seems like this procedure would neutralize any acids in the solution.  The Hydroxide would turn acid to water.  Any remaining hydroxide would combine with Calcium to form Calcium Hydroxide, which has a low solubility.  This would then precipitate out of the solution.  If the solution is mostly organic, it would also adsorb most of the water and remove it form the organic phase.
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 :)
429392
i'd say you have a basic understanding of molecular chemistry, micki.\n\nhowever, to improve your hypothesis, have it say:  I think the lower temperature the slower the salt will dissolve.  This is because the ions in a salt crystal require energy to dissolve away from the rigid crystal form the are in.  there is less energy present in cold water, therefore, the cold water will take longer to dissolve the salt crystals.
789424
The answer depends on what that substance it is and what the solvent is. Generally in nature, like dissolves in like. If you have a polar substance, it generally dissolves in any polar solvent. For example, salt (NaCl) is an ionic compund, it dissolves well in a polar solvent, such as water. However, you may find it difficult to dissolve NaCl in an organic solvent, such as hexane. On the other hand, many marker use some sort of organic ink, therefore, they can not be dissolved by water. However, you can try to dissolve them using alcohol.\nHaving said that, it is not absolute that all polar substances can not be dissolved in organic solvent or vice versa. If you have a compound, such as ethanol (which is organic substance), it can dissolve in water (which is a polar solvent). This is because ethanol molecule has a structure (the OH group) that can interact with the water molecule to form hydrogen bonding. However, if you use a much heavier organic compound, you will find it very difficult or even impossible to dissolve it in polar solvent.
869943
You could dissolve the crystal compound in water and measure the temperature change and specify whether there is an endothermic or exothermic change.  \n\nYou will need a thermometer.  Be careful as some crystal compounds are violently exothermic when dissolved in water.\n\nAndy
560067
According to the solubility rules, it is insoluble.\n\nHere are the solubility rules\n1. All common compounds of Group I and ammonium ions are soluble. \n\n2. All nitrates, acetates, and chlorates are soluble. \n\n3. All binary compounds of the halogens (other than F) with metals are soluble, except those of Ag, Hg(I), and Pb. Pb halides are soluble in hot water.) \n\n4. All sulfates are soluble, except those of barium, strontium, calcium, lead, silver, and mercury (I). The latter three are slightly soluble. \n\n5. Except for rule 1, carbonates, hydroxides, oxides, silicates, and phosphates are insoluble. \n\n6.Sulfides are insoluble except for calcium, barium, strontium, magnesium, sodium, potassium, and ammonium.
508324
First off... dihydrogen monoxide is ....WATER!!!!!!!!!\n\nThe smaller the salt crystals you are trying to dissolve, the more rapidly they will dissolve... due to increased surface area.