A 10.00 mL solution of 0.1900 M NH4Cl is titrated with 0.1300 M NaOH to the equivalence point. Volume of NaOH = 14.62mL Calculate the pH of the solution at the equivalence point. Calculate the pH of a simple 0.0772 M aqueous solution of ammonia.

A 10.00 mL solution of 0.1900 M NH4Cl is titrated with 0.1300 M NaOH to the equivalence point. Volume of NaOH = 14.62mL Calculate the pH of the solution at the equivalence point. Calculate the pH of a simple 0.0772 M aqueous solution of ammonia.

Chemistry

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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

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Concept explainers

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.

Question

A 10.00 mL solution of 0.1900 M
NH4Cl is titrated with 0.1300 M NaOH
to the equivalence point.
Volume of NaOH = 14.62mL
Calculate the pH of the solution at
the equivalence point.
Calculate the pH of a simple 0.0772
M aqueous solution of ammonia.

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Step 1: Determination of concentration of NH3 at equivalence point

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Step 2: Determination of the OH- ion concentration given by NH3 and pH of solution

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Step 3: Determination of the OH- ion concentration given by 0.0772 M NH3 and pH of solution

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