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## Main Question or Discussion Point

I know that a "strong acid" is one that ionizes completely in water. For example, hydrochloric acid, sulfuric acid, nitric acid, etc are considered strong acids because they all completely neutralize. Now, this leads me to two questions:

1) Is the concentration of a strong acid irrelevant in determining whether or not it completely ionizes? So for example, would 95% sulfuric acid ionize completely?

2) This question is applicable only if the answer to the above question is no. So suppose that the concentration IS a determining factor in ionization %, even if the acid is strong. Would neutralizing the acid induce further ionization? Let me give a concrete example. Suppose we had 1 mole of concentrated hydrochloric acid. Suppose that at this concentration, 50% of the HCl ionized. Then 0.50 moles of HCl is ionized and the 0.50 moles exists in solution as molecular HCl. Now suppose we added 0.50 moles of NaOH. This completely neutralizes the 0.50 moles of ionized HCl, correct? So now we have, in solution, 0.50 moles of NaCL and 0.50 moles of HCl. Now, does more HCl ionize since the concentration of HCl has decreased? Does the NaCl in the solution effect how much further the remaining HCl ionizes? (if it does actually ionize)

1) Is the concentration of a strong acid irrelevant in determining whether or not it completely ionizes? So for example, would 95% sulfuric acid ionize completely?

2) This question is applicable only if the answer to the above question is no. So suppose that the concentration IS a determining factor in ionization %, even if the acid is strong. Would neutralizing the acid induce further ionization? Let me give a concrete example. Suppose we had 1 mole of concentrated hydrochloric acid. Suppose that at this concentration, 50% of the HCl ionized. Then 0.50 moles of HCl is ionized and the 0.50 moles exists in solution as molecular HCl. Now suppose we added 0.50 moles of NaOH. This completely neutralizes the 0.50 moles of ionized HCl, correct? So now we have, in solution, 0.50 moles of NaCL and 0.50 moles of HCl. Now, does more HCl ionize since the concentration of HCl has decreased? Does the NaCl in the solution effect how much further the remaining HCl ionizes? (if it does actually ionize)