This article will discuss 6 chemical solubility rules and when they apply. These are some of the most important concepts in chemistry, so you should start reading! Rule #0: As a general rule, molecules that are polar tend to be more soluble in water than non-polar molecules. This is because the polarity of these compounds causes them to dissolve within the water and form hydrogen bonds with one another. Polarity can be determined by looking at how many electrons there are between two atoms. When you have an uneven number of electrons (such as when oxygen has six), then this means it will want to bond with something else so that it becomes evenly charged again—which leads us back to why solubility generally increases for substances which contain more electronegative elements like Oxygen. Non-polar molecules don’t do much since they aren’t very attracted or repelled by water.

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Rule #01: A compound will only dissolve in a certain solvent if it has an ionic charge, and this usually means the substance is charged when dissolved. For example, sodium chloride (NaCl) dissolves well because Na+ and Cl- ions are created which can form hydrogen bonds with one another. Other examples of substances that tend to be soluble due to their ionization include sodium sulfate (NaSO*), potassium nitrate (KNO*), barium chloride (BaCl*). Crystals like these are often used as indicators for solubility tests since they change color when dissolved—check out Chemistry Rocks! for more information on how you can do your own experiment at home. Rule

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