Short Answer Titration Lab Experiment 1: Perform a Coarse Titration Lab Results

Question

Short Answer

Titration Lab

Experiment 1: Perform a Coarse Titration

Lab Results

For your coarse titration record the following results.

volume of NaOH solution in the burette at the start (mL)

volume of NaOH solution in the burette at the end (mL)

volume of NaOH solution dispensed (mL)

volume of HCl solution in the flask (mL)

Data Analysis

Calculate the molarity of the HCl concentration using your coarse titration results.

Experiment 2: Perform a Fine Titration

Lab Results

For your fine titration record the following results.

volume of NaOH solution in the burette at the start (mL)

volume of NaOH solution in the burette at the end (mL)

volume of NaOH solution dispensed (mL)

volume of HCl solution in the flask (mL)

Data Analysis

Calculate the molarity of the HCl concentration using your fine titration results.

Conclusions

What do you expect to happen if you forget to add phenolphthalein to the Erlenmeyer flask?

Suppose you had to titrate a solution of NaOH of unknown concentration with a solution of HCl of known concentration using phenolphthalein as an indicator. How will you determine the color change?

Suppose you titrated a sample of acetic acid (monoprotic acid) with a 0.125 M solution of NaOH. Given the data in the table below, what is the concentration of the acetic acid solution?

volume of NaOH solution in the burette at the start (mL)

volume of NaOH solution in the burette at the end (mL)

volume of NaOH solution dispensed (mL)

volume of HCl solution in the flask (mL)

Explanation / Answer

If the indicator phenolphthalein is not added, we wold not be able to identify the end point of the acid-base titration.

When NaOH is titrated with HCl using phenolphthalein indicator, the color changes from pink (basic) to colorless (acidic) at the end point.

Titration : Acetic acid + NaOH

moles NaOH used = 0.125 M x 22.40 ml = 2.8 mmol

concentration of acetic acid = 2.8 mmol/15 ml = 0.187 M

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