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.
Chapter 15 Solutions
Principles of Modern Chemistry
Ch. 15 - Vitamin C is ascorbic acid (HC6H7O6), for which Ka...Ch. 15 - Suppose a 0.100 M solution of each of the...Ch. 15 - Sulfanilic acid (NH2C6H4SO3H) is used in...Ch. 15 - Phthalic acid ( H2C8H4O4, abbreviated H2Ph ) is a...Ch. 15 - Prob. 88APCh. 15 - Prob. 94APCh. 15 - Prob. 100APCh. 15 - Prob. 102AP
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- Suppose that you want to titrate a sample of vinegar with standard sodium hydroxide solution to determine the concentration of acetic acid in it, and you want to use an indicator to help you determine the end-point. Which of the following indicator would be suitable? (A) Bromocresol Green (Ka ~ 2.0 x 10–5; color: yellow in acid; blue in base) (B) Methyl Red (Ka ~ 5.0 x 10–6; color: red in acid; yellow in base) (C) Bromothymol Blue (Ka ~ 6.0 x 10–8; color: yellow in acid; blue in base) (D) Any of themarrow_forwardMake sure has a correct significant digarrow_forward3 A 0.6423 g sample that might contain NaOH, Na₂CO₃, NaHCO₃, or a permissible mixture of the bases is titrated with 0.1062 M HCl by the double indicator method. It is found that 40.83 mL of the acid are required to reach the phenolphthalein end point. Methyl orange is then added to the solution and the titration continued using an additional 12.38 mL of the acid. Calculate the percentage of each component in the sample.arrow_forward
- I need the answer as soon as possiblearrow_forwardFind the molarity of a sulfuric acid solution when 25.00 mL of this solution is titrated to a slight pink end point with 13.93 mL of 0.5609 M NaOH.arrow_forward1. You will use 0.5mM PNPP, 0.2M Tris-HCl, and 1mM P; stock solutions to prepare two sets of five samples (Sets A and B), each with varying P; concentrations. The PNPP concentration for all samples in Set A will be 0.05mM; and 0.150mM for all samples in Set B. Fill out the tables below and use them to prepare your samples. Be aware of the following: • Prepare the samples directly in cuvettes. Prepare one sample at a time to minimize exposing PNPP to air. You can prepare the next sample while the current one is being measured. • Each sample before adding enzyme (i.e., the cuvette only contains PNPP, Pi, and Tris-HCI) is its own blank. In other words, you add the appropriate amounts of PNPP, Pi, and Tris- HCI to a cuvette, press "Measure Blank", then add 100μL of AP to the same cuvette, mix, and press "Measure Sample". • You must blank the instrument (before adding the enzyme) each time you prepare a new sample. Table 1. Sample Set A (PNPP concentration = 0.05mM) Final [Pi] (μM) Vol of…arrow_forward
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