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A student titrates a weak acid with 0.100 M NaOH, adding 34.84 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?

A student titrates a weak acid with 0.100 M NaOH, adding 34.84 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?

Chemistry: Principles and Practice
Chemistry: Principles and Practice
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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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A student titrates a weak acid with 0.100 M NaOH, adding 34.84 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

Calculation of no. of mol of NaOH:

No. of mol=Molarity×Volume=0.100 mol/L×34.84×10-3 L=3.484 ×10-3 mol

Calculation of no. of mol of HCl added:

No. of mol=Molarity×Volume=0.0500 mol/L×3.19×10-3 L=0.1595×10-3 mol

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