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A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.15 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 17.72 3.31 Equivalence point 35.44 8.37 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following reaction occurs HA + NaOH = NaA + H2O What is the concentration of A (the conjugate base of the weak acid) at the equivalence point? Use [A]and the pH at the equivalence point to estimate Ka of the weak acid (this is the hard way of estimating Ka) Use the pH at the half-way point to estimate Ką of the weak acid (this is the easier way)

A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.15 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 17.72 3.31 Equivalence point 35.44 8.37 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following reaction occurs HA + NaOH = NaA + H2O What is the concentration of A (the conjugate base of the weak acid) at the equivalence point? Use [A]and the pH at the equivalence point to estimate Ka of the weak acid (this is the hard way of estimating Ka) Use the pH at the half-way point to estimate Ką of the weak acid (this is the easier way)

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 57P
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A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.15 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 17.72 3.31 Equivalence point 35.44 8.37 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following reaction occurs HA + NaOH = NaA + H2O What is the concentration of A (the conjugate base of the weak acid) at the equivalence point? Use [A]and the pH at the equivalence point to estimate Ka of the weak acid (this is the hard way of estimating Ka) Use the pH at the half-way point to estimate Ką of the weak acid (this is the easier way)
Transcribed Image Text:A student peforms a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.15 M solution of NaOH. They collect data, plot a titration curve and determine the values given in the below table. ml NaOH added pH Half-way Point 17.72 3.31 Equivalence point 35.44 8.37 How many moles of NaOH have been added at the equivalence point? mol What is the total volume of the solution at the equivalence point? mL During the titration the following reaction occurs HA + NaOH = NaA + H2O What is the concentration of A (the conjugate base of the weak acid) at the equivalence point? Use [A]and the pH at the equivalence point to estimate Ka of the weak acid (this is the hard way of estimating Ka) Use the pH at the half-way point to estimate Ką of the weak acid (this is the easier way)
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