Are ions soluble or insoluble?
98382
You will not find ions along by themselves, they are paired with other ions, forming ionic compounds.\nSome ionic compounds are soluble, some are.  The ones that are can range in solubility based on the solvent, temperature, and other ions in solution.\n\nFor instance, NaCl is very soluble in water at room temperature, where as under the same conditions, Silver Chloride is considered insoluble.\n\nTherre are actually a set of solubility rules to determine whether an ionic compound is or is not soluble in water based on the ions that make it up.\nhttp://www.csudh.edu/oliver/chemdata/solrules.htm
944444
Both calcium chloride and silver nitrate are soluble in water. If you swap the names you get silver chloride and calcium nitrate. Silver chloride is insoluble and calcium nitrate is soluble. So if you mix a solution of calcium chloride and a solution of silver nitrate, an insoluble precipitate of silver chloride will form and calcium nitrate will remain in solution. The balanced equation is \n\nCaCl2(aq) + 2AgNO3(aq) -----> 2AgCl(s) + Ca(NO3)2 (aq)
159409
the rule of thumb is "like dissolves like" \nWater is polar so if it dissolves a substance, that substance is also polar.
738381
Oil only.  Lipids are very much insoluble in water, because water is a polar solvent while lipids are highly nonpolar.  The rule of thumb for solutions is "like dissolves like," so a nonpolar lipid will not dissolve in polar water.  Lipids are also insoluble in salt water, because the presence of other solutes in the solvent does not affect its solubility for other solutes.  But oil is a nonpolar solvent, and is in fact a lipid itself, so lipids will dissolve in it.
327351
The previous answer is correct if an equal number of moles is dissolved.  If you were looking at a saturated solution, it would be LiCl, which can dissolve in greater quantities than any other salt, even greater than NaCl. (36 g of NaCL will dissolve in 100 ml water compared to 55 grams LiCl per 100 ml water). The Li+ ion is very very small-it's only larger than hydrogen and helium. For an equal weight of LiCl and Al(NO3)3 dissolved in water, LiCl would also have a greater effect, because of the greater number of ions per gram.  Thus, in either a saturated solution or a weight to volume solution, LiCl would produce the greater number of ions, whereas it would not in a equamolar solution.  LiCl is used a great deal in density experiments, because you can make a very dense aqueous solution of it, and in reducing freezing point, since you can get the maximum number of ions of any aqueous solution, so the questioner is probably looking for LiCl.
705134
Refer to the reference for the structures.  The indigo is a relatively nonpolar molecule so it is insoluble in water.  The leuco form is a disodium salt and therefore soluble in water.
811655
If by 'undissolved' you mean why are some salts insoluble in water, then I think we are in business.\n\nIn order for a salt to be soluble it has to be energetically favorable for the ions to separate. This requires a negative gibbs free energy. G = H - TS So you have to find the H and S values for the solid to aqueous solution and see if G will be negative for a given temperature.\n\nA method I recently learned to make insolube salts more soluble is to add other ions to the water...but you have to be careful to not add a common ion...or Le Chantliear will come into play.
14648
Most acids form ions in solutions by _protolysis_ (transferring a hydrogen ion to the solvent), and most bases form ions in solution by disassociation (if they contain OH-ions) or by accepting a hydrogen ion from the solvent.\n\nExample: Na3PO4 + H2O --> 3 Na+ +HPO4(2-) + OH-
916529
d) Cu I\n\nChromic and phosphoric acid are polyprotic acids and the salts will show a decreasing solubility with increasing pH as the higher pH favours the formation of chromate and phosphate.\n\nHydroIodic acid is a strong acid and is fully dissociated and the the amount of iodide formed depends on concentration and not pH. Thus CuI solubility will show no dependence on pH.
118913
Only some of the milk proteins are water soluble, most are only in colloidal suspension.\n\nSimilar with chicken egg proteins: a few might be soluble, most won't be.
265572
Yes. An electrolyte is defined as a species that dissolves in water and produces electrically conducive ions. Stomach acid is concentrated hydrochloric acid. Chloride ions are electrically conductive, so stomach acid is an electrolyte.\n\n>>No, it is not.\nElectrolytes are SALTS. Salts have a perfectly neutral pH. Acid.....well it's acid.<<\n\nMost electrolytes are salts. And no, salts don't have a perfectly neutral pH. Nothing has a perfectly neutral pH, and some salts are most definitely acidic or basic.
218353
It depends.\nThe salt has to dissolve in water.\nThe more ions / cm3 in te water (never mind the kind),\nthe better the electric conductivity.
482786
Isopropyl alcohol is completely miscible with water, as it can hydrogen bond to water.\n\nCalcium chloride is soluble because water is polar and the attractive forces between the calcium ions and chloride ions can be overcome by water.
573070
Water, sugar water, then salt water.\n\nSalt dissolves into 2 ions Na+ and Cl- per molecule, whereas sugar only dissolves into one sugar molecue. The greater the number of particles in solution, the lower the freezing point goes.
95222
Potassium Chloride (KCl) has a solubility of .4 g/mL in Ethanol (at room 25 C I would assume), yes, it does dissolve, but barely.
924596
The KCl, definitely.  Conductivity in water is greatly enhanced by the presence of ions.  Deionized water actually has fewer ions in it than ordivnary tap water, so it's a really terrible conductor.  KCl, on the other hand, dissolves into K+ and Cl- in water, so there are a whole lot of ions in a solution of KCl.
898270
Calcium Phosphate is insoluble, so it will precipitate.\n\nThere is no all the time rules, just trends\nNa, Li, K, are almost always soluble.\nCL, F, I, Br, NO3 are almost always.\n\nAs you move towards the middle of the periodic table, it becomes less soluble