Question #63492
Suppose our unknown acid was acetic acid, CH3COOH (Ka = 1.8 x 10-5) and that your initial aqueous solution contained 0.100 mol of acetic acid in total volume of 100 mL.
To this acetic acid solution you begin adding a 1.0 mol/L NaOH solution. Let's see what happens after adding different amounts of NaOH.
Suppose you have added a total of 20.0 mL of NaOH solution since the beginning of the titration. How many mol of acetate ions (CH3COO–) are present in the reaction mixture at this point?
To this acetic acid solution you begin adding a 1.0 mol/L NaOH solution. Let's see what happens after adding different amounts of NaOH.
Suppose you have added a total of 20.0 mL of NaOH solution since the beginning of the titration. How many mol of acetate ions (CH3COO–) are present in the reaction mixture at this point?
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