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siylens or no tnevtd er 670 to 200 A 0.397 g sample of potassium hydrogen phthalate, KHC3H404 (molar mass dissolved with 50 mL of deionized water in a 125-mL Erlenmeyer flask. The san phenolphthalein endpoint with 16.22 mL of a sodium hydroxide solution (see E the molar concentration of the NaOH solution? dgur beanegaio ed

siylens or no tnevtd er 670 to 200 A 0.397 g sample of potassium hydrogen phthalate, KHC3H404 (molar mass dissolved with 50 mL of deionized water in a 125-mL Erlenmeyer flask. The san phenolphthalein endpoint with 16.22 mL of a sodium hydroxide solution (see E the molar concentration of the NaOH solution? dgur beanegaio ed

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Titration of Potassium Hydrogen Phthalate with Sodium Hydroxide** **Objective:** To determine the molar concentration of a sodium hydroxide (NaOH) solution by titrating it against a known mass of potassium hydrogen phthalate (KHP). **Procedure:** 1. **Sample Preparation:** - A 0.397 g sample of potassium hydrogen phthalate (KHP, chemical formula: KHC₈H₄O₄, molar mass = 204.44 g/mol) is used. - The sample is dissolved in 50 mL of deionized water and placed into a 125-mL Erlenmeyer flask. 2. **Titration Process:** - The KHP solution is titrated with a sodium hydroxide solution. - Phenolphthalein is used as an indicator to detect the endpoint of the titration. - The endpoint of the titration is reached when phenolphthalein changes color, indicating that the acid has been completely neutralized by the base. 3. **Volume of NaOH Used:** - The titration requires 16.22 mL of NaOH solution to reach the endpoint. **Calculations:** - Calculate the molar concentration of the NaOH solution using the known mass of KHP, its molar mass, and the volume of NaOH used. The balanced reaction between KHP and NaOH is in a 1:1 molar ratio, hence the moles of KHP will equal the moles of NaOH at the endpoint. **Conclusion:** This experiment is a common laboratory procedure to find the concentration of a base solution using a primary standard acid. By understanding and following this process, one can determine the molarity of an unknown NaOH solution effectively.
Transcribed Image Text:**Titration of Potassium Hydrogen Phthalate with Sodium Hydroxide** **Objective:** To determine the molar concentration of a sodium hydroxide (NaOH) solution by titrating it against a known mass of potassium hydrogen phthalate (KHP). **Procedure:** 1. **Sample Preparation:** - A 0.397 g sample of potassium hydrogen phthalate (KHP, chemical formula: KHC₈H₄O₄, molar mass = 204.44 g/mol) is used. - The sample is dissolved in 50 mL of deionized water and placed into a 125-mL Erlenmeyer flask. 2. **Titration Process:** - The KHP solution is titrated with a sodium hydroxide solution. - Phenolphthalein is used as an indicator to detect the endpoint of the titration. - The endpoint of the titration is reached when phenolphthalein changes color, indicating that the acid has been completely neutralized by the base. 3. **Volume of NaOH Used:** - The titration requires 16.22 mL of NaOH solution to reach the endpoint. **Calculations:** - Calculate the molar concentration of the NaOH solution using the known mass of KHP, its molar mass, and the volume of NaOH used. The balanced reaction between KHP and NaOH is in a 1:1 molar ratio, hence the moles of KHP will equal the moles of NaOH at the endpoint. **Conclusion:** This experiment is a common laboratory procedure to find the concentration of a base solution using a primary standard acid. By understanding and following this process, one can determine the molarity of an unknown NaOH solution effectively.
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