A student carried out an acid-base titration by adding NaOH solution from a buret to an Erlenmeyer flask containing HCl solution and using phenolphthalein as an indicator. At the equivalence point, she observed a faint reddish-pink color. However, after a few minutes, the solution gradually turned colorless. What do you suppose happened? Explain.

Q: Determine the pH during the titration of 14.9 mL of 0.149 M nitric acid by 7.12x10-2 M potassium…

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Q: Why the shapes of strong acid–strong base, weak acid–strong base, and weak base–strong acid…

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Q: Determine the pH during the titration of 19.4 mL of 0.250 M hydrochloric acid by 6.87×10-2 M barium…

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Q: The student Louise continued the analysis of acetic acid using half - neutralization technique. She…

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Q: A student accidently titrated the acetic acid with 1.00 M NaOH solution instead of 0.10 M NaOH. Draw…

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Q: A student attempts to determine the buffer capacity of a solution by titrating 40.0 mL of solution…

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Q: would result in a buffer situation. Select all correct

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Q: Volume of acetic acid (HC2H3O2) in the first titration (L)     10 mL Volume of acetic acid…

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Q: Addition of 15 mL 0.1 M NaOH solution to 25 mL 0.1 M CH3COOH solution produces a buffer solution.…

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.