Calculate [H3O ], [ClO4–], and [OH–] in an aqueous solution that is 0.175 M in HClO4(aq) at 25 °C.?
If some one could show me the steps to doing this, it would really help. Thanks :)
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If some one could show me the steps to doing this, it would really help. Thanks :)
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HClO4 is a very strong acid that should be close to l00% ionized or dissociated in a water solution at 25 degrees C, so .175 molar HClO4 should produce .l75 molar H3O+ and .l75 molar ClO4-
Now to get the concentration of (OH) in the same solution, knowing that in any water based acid or basic solution that the (H3O+) molar concentration times the (OH-) ion concentration in moles per liter of each always equals l x l0-l4, just solve for the (OH-) concentration in this equation.
l x l0-l4 = (.l75 molar H3O+) times (OH-) The (OH-) concentration is X