PRINCIPLES OF MODERN CHEMISTRY-OWLV2
8th Edition
ISBN: 9781305271609
Author: OXTOBY
Publisher: CENGAGE L
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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-OWLV2
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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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- 4. Complete neutralization of 10 mL of hydrochloric acid solution by NaOH 0.1 N in the presence of phenol phthalein until the appearance of purple color (pHf= 9) 15 mL of NaOH is consumed. (a) What is the concentration of hydrochloric acid? (b) Calculate the indicator error.arrow_forward:///((((arrow_forwardCalculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g, NaOH used = 43.00 ml ; 0.600 N H2SO4 used for back titration =0.250 ml ; 1.00ml NaOH is equivalent to 0.0315 g H2C2O4. 2H2O.arrow_forward
- A 50.00 mL aliquot from a 1.50 L ferrous sulfate (FeSO4) stock solution is titrated with 20.00 mL potassium dichromate (K2Cr2O7) to reach the green-to-purple diphenylamine endpoint. If the concentration of K2Cr2O7 is 2.50 mM, calculate the FeSO4 concentration of the stock solution. Enclose in a box your final answer. Use correct significant figures. 6 FeSO4 + K2Cr2O7 +7 H2SO43 Fe2(SO4)3 + Cr2(SO4)3 + K2SO4 + 7 H₂Oarrow_forwardA 50.00-mL sample of white wine required 24.57 mL of 0.03291M NaOH to achieve a phenolphthalein end point. Express the acidity of the wine in grams of tartaric acid (H2C4H4O6; 150.09 g/mol) per 100 mL. (Assume that two hydrogens of the acid are titrated.)arrow_forwardA 0.5843-g sample of a plant food preparation was analyzed for its N content by the Kjeldahl method, the liberated NH3 being collected in 50.00 mL of 0.1062 M HCl. The excess acid required an 11.89 mL back-titration with 0.0925 M NaOH. Express the results of this analysis in terms of (a) %N (b) %urea, H2NCONH2 (c) %(NH4)2SO4 (d) %(NH4)3PO4arrow_forward
- Give handwritten answer. ASAParrow_forwardPRE-LAB QUESTIONS Calculate the volume, in mL, of a 0.50 M NaOH solution that will be required to titrate 1.2 g of potassium hydrogen phthalate to the phenolphthalein end point. The molar mass of KHP is 204.2 g/mol. 1.arrow_forwardSuppose 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_forward
- Make 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_forwardOxaloacetic acid (C4H5O5, pKa1 = 2.56, pKa2 = 4.37), a diprotic acid, is part of the citric acid cycle. What is the concentration of hydrogenoxaloacetate (C4H4O5–) in a 0.5000 M solution of sodium oxaloacetate (Na2C4H3O5)?arrow_forward
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