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A student place 2 mL of a hydrochloric acid solution in an Erlenmeyer flask. She then added 23.3 mL DI water and 2 drops 0.2% phenolphthalein solution. During the titration, a faint, pale pink color was observed when 21.38 mL of 0.272 M barium hydroxide had been added. Calculate the concentration (in M) of the original hydrochloric acid solution.

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Related questions

A chemist had a bottle of HCl (aq) of unknown concentration. Sheperformed a titration experiment in order to determine itsconcentration. She pipeted 15.00 mL of the HCl solution into anErlenmeyer flask. She then added about 20 mL of deionized water and3 drops of phenolphthalein indicator dye to the flask. She titratedthis mixture with 0.07269 M NaOH (aq), and obtained a permanent,pale pink endpoint after the addition of 24.33 mL of NaOH (aq).Given that the density of the HCl solution was 1.095 g/mL,determine the concentration of the original HCl acid solution inunits of:

A. Molarity

B.Percent by mass

Thanks!!


1. What is the difference between equivalence point and endpoint?

2. In a titration with a strong acid and a strong base, why used phenolphthalein as the indicator?

3. If the color remains clear, then is the solution acidic or basic?

Data.

Trial Initial volume Final volume moles of base moles of acid concentration of acid

1 0.14mL 15.74mL

2 0.02mL 14.40mL

3 0.05mL 15.11mL

Average of the acid concentration:

Procedure.

A student added 20.00mL of acid to a Erlenmeyer flask along with 2-3 drops of indicator. Then using a 0.106 M base, the student titrated the solution. The color will change from clear to pink as you add the base. Once, you observe a faint pink color for 10 seconds, then you are complete. The data above is taken from 3 trials of titrations after adding the necessary base. (HCl - acid and NaOH -base) This neutralization is a 1:1 mole ratio.

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