A student titrates a weak acid with 0.100 M NaOH, adding 31.65 mL before a dark pink color is seen. Realizing that the end point has been passed, he then adds 3.19 mL 0.0500 M HCl until the solution is neutralized. How many moles of H+ were present in the initial weak acid solution?

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A student titrates a weak acid with 0.100 M NaOH, adding 31.65 mL before a dark pink color is seen. Realizing that the end point has been passed, he then adds 3.19 mL 0.0500 M HCl until the solution is neutralized.

How many moles of H+ were present in the initial weak acid solution?

Expert Solution
Step 1

The mole of H+ ion the weak acid is equal to the mole of NaOH used in the titration. 

The molarity of NaOH = 0.100 M

The volume of NaOH is = 31.65 mL

The excess NaOH used is neutralized by the HCl.

The molarity of HCl is = 0.0500 M

The volume of the HCl is = 3.19 mL

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