a) The pH solution is 5.28 at equivalence point. Identify the correct type of acid-base pair titration with the correct examples. b) An analytical chemist need to determine the content of calcium carbonate present in a 0.125 g eggshell sample. The sample was dissolved in a 50.00 mL of 0.200 M of hydrochloric acid, first standard reagent. The next analysis is titration of the excess acid which required 32.12 mL of 0.250 M sodium hydroxide, the second reagent. Calculate the percentage by weight the purity of calcium carbonate in the eggshell sample. CaCO3 + 2HCl → CaCl₂ + CO₂ + H₂O

a) The pH solution is 5.28 at equivalence point. Identify the correct type of acid-base pair titration with the correct examples. b) An analytical chemist need to determine the content of calcium carbonate present in a 0.125 g eggshell sample. The sample was dissolved in a 50.00 mL of 0.200 M of hydrochloric acid, first standard reagent. The next analysis is titration of the excess acid which required 32.12 mL of 0.250 M sodium hydroxide, the second reagent. Calculate the percentage by weight the purity of calcium carbonate in the eggshell sample. CaCO3 + 2HCl → CaCl₂ + CO₂ + H₂O

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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Similar questions

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.
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
. 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.
Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?
A 25.0-mL sample of hydroxylamine is titrated to the equivalence point with 35.8 mL of 0.150 M HCl. a What was the concentration of the original hydroxylamine solution? b What is the pH at the equivalence point? c Which indicators, bromphenol blue, methyl red, or phenolphthalein, should be used to detect the end point of the titration? Why?
You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.

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