Four solutions of unknown NaOH concentration are titrated with solutions of HCI. The following table lists the volume of each unknown NaOH solution, the volume of HCl solution required to reach the equivalence point, and the concentration of each HCl solution. Calculate the concentration (in M) of the unknown NaOH solution in each case. Sample (a) (b) (c) (d) NaOH volume (mL) 5.00 15.00 10.00 30.00 concentration of sodium hydroxide = HCI volume (mL) 9.77 11.34 10.55 36.18 Express your answers in molarity to three or four significant figures, separate your answers with commas. VE ΑΣΦ [HCI] (M) 0.1599 0.1311 0.0889 0.1021 ? MNaOH

Four solutions of unknown NaOH concentration are titrated with solutions of HCI. The following table lists the volume of each unknown NaOH solution, the volume of HCl solution required to reach the equivalence point, and the concentration of each HCl solution. Calculate the concentration (in M) of the unknown NaOH solution in each case. Sample (a) (b) (c) (d) NaOH volume (mL) 5.00 15.00 10.00 30.00 concentration of sodium hydroxide = HCI volume (mL) 9.77 11.34 10.55 36.18 Express your answers in molarity to three or four significant figures, separate your answers with commas. VE ΑΣΦ [HCI] (M) 0.1599 0.1311 0.0889 0.1021 ? MNaOH

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 1P

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Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
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