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Determine the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H5NH2, Kb = 4.3x10-4) by 0.333 M HCIO4 at the following points. (a) Before the addition of any HCIO4| (b) After the addition of 13.5 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 49.1 mL of HCIO4

Determine the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H5NH2, Kb = 4.3x10-4) by 0.333 M HCIO4 at the following points. (a) Before the addition of any HCIO4| (b) After the addition of 13.5 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 49.1 mL of HCIO4

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
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**Titration of Ethylamine with Perchloric Acid: Calculating pH at Key Points** This experiment involves determining the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H₅NH₂), which has a base dissociation constant (Kb) of 4.3×10⁻⁴, using 0.333 M perchloric acid (HClO₄). The pH is to be calculated at the following key points: (a) **Before the Addition of Any HClO₄** - Calculate the initial pH of the ethylamine solution. (b) **After the Addition of 13.5 mL of HClO₄** - Determine the pH after adding the indicated volume of the acid. (c) **At the Titration Midpoint** - Find the pH at the halfway point to the equivalence. (d) **At the Equivalence Point** - Calculate the pH when the moles of acid equal the moles of base. (e) **After Adding 49.1 mL of HClO₄** - Determine the final pH after this amount of acid is added. **Note**: No graphs or diagrams are present. Solutions require calculations based on stoichiometry and equilibrium chemistry principles.
Transcribed Image Text:**Titration of Ethylamine with Perchloric Acid: Calculating pH at Key Points** This experiment involves determining the pH during the titration of 32.5 mL of 0.333 M ethylamine (C₂H₅NH₂), which has a base dissociation constant (Kb) of 4.3×10⁻⁴, using 0.333 M perchloric acid (HClO₄). The pH is to be calculated at the following key points: (a) **Before the Addition of Any HClO₄** - Calculate the initial pH of the ethylamine solution. (b) **After the Addition of 13.5 mL of HClO₄** - Determine the pH after adding the indicated volume of the acid. (c) **At the Titration Midpoint** - Find the pH at the halfway point to the equivalence. (d) **At the Equivalence Point** - Calculate the pH when the moles of acid equal the moles of base. (e) **After Adding 49.1 mL of HClO₄** - Determine the final pH after this amount of acid is added. **Note**: No graphs or diagrams are present. Solutions require calculations based on stoichiometry and equilibrium chemistry principles.
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