Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN: 9781305079113
Author: David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher: Cengage Learning
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Chapter 15, Problem 102AP
Interpretation Introduction

Interpretation:The chemist who explained the correct procedure for the interview question by the chief chemist regarding the analysis of the exact percentage of acetic acid in the vinegar needs to be determined.

Concept Introduction:

The reaction in which acid reacts with base and form water and salt is known as neutralization reaction.

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Petanoic (or valeric) acid is a weak organic acid with an unpleasant odour. Like other small carboxylic acids, it is used to make pleasant smelling esters that are used in perfumes, cosmetics, and food additives. Completed Part D In Part B, a 20.00 mL aliquot of a 0.195 mol L-1 pentanoic acid solution was titrated to its equivalence point with 19.7 mL of 0.198 mol L- 1 NaOH solution. At the equivalence point, all of the weak acid, pentanoic acid, is converted to its weak conjugate base, pentanoate. In part A, the Ka for pentanoic acid was determined to be 1.48×10-5. What is the pH at this equivalence point? 5.089 6.997 pentanoic acid 9.170 4.830 The pka of pentanoic acid is 4.830. 8.911
The chief chemist of Victory Vinegar Works, Ltd., inter- views two chemists for employment. He states, “Qual- ity control requires that our high-grade vinegar contain 5.00 ± 0.01% acetic acid by mass. How would you analyze our product to ensure that it meets this specification?" Anne Dalton says, "I would titrate a 50.00-11L sample of the vinegar with 1.000 M NaOH, using phe- nolphthalein to detect the equivalence point to within ±0.02 mL of base." Charlie Cannizzarro says, "I would use a pH meter to determine the pH to ±0.01 pH units and interface it with a computer to print out the mass percentage of acetic acid." Which candidate did the chief chemist hire? Why?
✓ ?? 14. Two groups of students were asked to check the concentration of ammonia in a particular brand of cleaning product because there had been complaints about that brand. The students placed a 25.0mL sample of cleaning product in a volumetric flask and made it up to 250mL using distilled water. They then performed a titration by using 25.0mL of the diluted ammonia solution in a conical flask and 0.10 moll-¹ standardised hydrochloric acid in a burette. One group used bromocresol green (pH range 4.0-5.6) as the indicator and obtained the following results: Titration Volume of acid 1st 23.2 added (mL) 2nd 22.9 3rd 22.8 4th 22.9 a) Calculate the concentration of the diluted sample. b) Calculate the concentration of ammonia in 1L of the original sample.
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Acid-Base Titration | Acids, Bases & Alkalis | Chemistry | FuseSchool; Author: FuseSchool - Global Education;https://www.youtube.com/watch?v=yFqx6_Y6c2M;License: Standard YouTube License, CC-BY