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How Does Hf Exist In An Aqueous Solution

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Chem question reguarding molecular form vs ions vs a mixture of ions and molecules?
Indicate whether the substance exists in aqueous solution (a) in , (b) as , (c) or as a mixture of molecules and . Substances: NaClO4, HF, Ba(OH)2, CH3CN. I have no idea what this even means or how to figure it out, please explain

Lots of chemicals dissolve in water, but only some will ionize. Generally, soluble salts split apart into ions in water. NaClO4 is such a soluble salt and completely splits apart to form Na+ ions and ClO4^- ions. HF is a weak acid. The definition of a weak acid is that is ionizes to a slight degree. Therefore, a solution of HF there will be mostly HF(aq) molecules and a very small number of H+ and F- ions. Ba(OH)2 is not very soluble in water, but what little does dissolve, completely ionizes to form Ba2+ and OH- ions. Therefore, barium hydroxide is considered a strong base. CH4CN, acetonitrile, is completely miscible with water, which means that the two liquids mix, but CH4CN does not ionize. It exists as molecules mixed with water molecules.

What determines a strong or weak electrolyte?
For instance, Calcium Chloride is a strong electrolyte. How would one determine that?

Hello, Budd. When a compound dissolutes in aqueous solution (when it breaks apart in water), it usually separates into its individual components. For example, NaNO3 would dissolute into Na (+1 charge) and NO3 (-1 charge) ions. Another interesting fact about dissolution to note is that one ion of a compound like yours, CaCl2, actually forms THREE ions when it dissolutes: one ion of Ca (+2 charge) and TWO ions of Cl (-1 charge). Now, to address the matter of electrolytes and their strength... first, let's establish what an electrolyte IS. According to (, an electrolyte is "A substance which forms ions in an aqueous solution". Therefore, any substance that dissolutes to form ions is an electrolyte. However, there are varying degrees of strength in electrolytes. The strength of an electrolyte is determined by whether or not the substance "completely dissociates into ions in water." In a strong electrolyte, "The acid or base molecule does not exist in aqueous solution, only ions. Weak electrolytes are incompletely dissociated. (" For example, HCl is a strong electrolyte because it leaves behind no molecules in the solution, but HF is a weak electrolyte because some of the ions are left incompletely dissocaited. It is difficult to determine at a glance whether or not a substance will be a strong or weak electrolyte. However, there are some simple acids that you would do well to commit to memory. To view them and read more about the strength of electrolytes, try ( ) I hope this helps you. Best of luck! ~The Tigress

Which of the following substances as an acid, base, salt, or none. decide whether the subs?
Label each of the following substances as an acid, base, salt, or none of the above. Indicate whether the substance exists in aqueous solution entirely in molecular form, entirely as ions, or as a mixture of molecules and ions. HF CH3CN NAClO4 Ba(OH)2

HF is an acid, as a mixture of molecules and ions CH3CN is none of the above, entirely in molecular form NaCIO4 is a salt, entirely as ions Ba(OH)2 is a base, entirely as ions

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