Can anyone help me with the following 2 questions???
In lab we determined the number of drops of 0.1 M NaOH required to neutralize 2 mL samples of 0.1 M HCl and 0.1 M HC2H3O2.
Although HCl is a strong acid and HC2H3O2 is a weak acid, approximately the same volume of NaOH should have been required for both neutralizations. WHAT WOULD BE THE EXPLANATION FOR THIS??
How does the change in pH during addition of NaOH differ when using a weak acid (acetic acid) in place of a strong acid (HCl)? SAME HERE. DOES ANYONE KNOW WHY? I HAVE NO CLUE.
Help with chem questions: acid bases
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Help with chem questions: acid bases
achosen1
Both acids only have 1 titratable hydrogen. The acid base reaction is stoichiometric.
in the first reaction the base is reaction directly with H3O+ and in the second is reacting stoichiometrically with acetic acid
CH3CHOOH + OH-
because each reaction produced water...the pH whenver you stop titrating (before or at the endpoint) is determined by the acid that remains in the water
the acetic acid is calculated as weak acid
and HCl as a strong acid so the pHs will be different
in the first reaction the base is reaction directly with H3O+ and in the second is reacting stoichiometrically with acetic acid
CH3CHOOH + OH-
because each reaction produced water...the pH whenver you stop titrating (before or at the endpoint) is determined by the acid that remains in the water
the acetic acid is calculated as weak acid
and HCl as a strong acid so the pHs will be different