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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Students have asked these similar questions
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
Calculate the volume in liters of 0.545 M KOH necessary to titrate 0.0113 moles of hydrochloric acid, HCl, to a phenolphthalein end-point. Report the answer with three significant figures.
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?
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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- Ethanol is needed as solvent when preparing phenolphthalein color indicator in volumetric titrations. What class of ethanol best suits the intended purpose? Explain your answer.arrow_forward4. 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_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 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_forwardCalculate the volume in milliliters of 0.362 M KOH necessary to titrate 28.38 mL of 0.279 M diprotic sulfuric acid, H2SO4, to a phenolphthalein end-point. Report the answer to a precision of 2 decimal places.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
- 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_forwardYou are asked to prepare a pH = 4.00 buffer startingfrom 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and any amount you need of sodium benzoate(C6H5COONa). (a) What is the pH of the benzoic acidsolution prior to adding sodium benzoate? (b) How manygrams of sodium benzoate should be added to prepare thebuffer? Neglect the small volume change that occurs whenthe sodium benzoate is added.arrow_forwardA local company sent you their green alternative for window cleaner to be tested for percent (w/v) acetic acid content. For your experiment, you first standardized your NaOH titrant with 0.8053 g of (99.80 % purity) KHP. You used 40.60 mL of NaOH for your standardization. After that you then analyzed a 10.00 mL sample and found that you needed 43.20 mL NaOH to reach the end point. Summary of results: Standardization Sample analysis KHP Weight (g) 0.8053 g Volume of sample 50.00 mL Purity 99.80% NaOH (mL) used 33.20 mL NaOH (mL) used 40.60 mL Determine the following: Molarity of NaOH % (w/v) acetic acidarrow_forward
- 1. 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_forwardFormulate a hypothesis regarding the solubility of aspirin at different pH.The experimentA) Three teaspoons of water (approx. 15 ml) were added to one tablet said to contain 300 mg of aspirin. Fizzingwas observed. Most of the tablet dissolved, but there were some solid particles. By heating the mug in amicrowave for 10 second increments until the water came to the boil (approx. 3x), all of the solid particlesdissolved. The solution was left to cool to room temperature and then placed in a fridge and NOTHINGHAPPENED. Try this yourself if you can spare two aspirin tablets, your results might look different.• Questions to ask:1. What might the fizzing bubbles be?2. Can you give a chemical explanation?3. Can you write a chemical reaction equation with aspirin reacting with something to give a gas and aspirinin another form?4. What might be the formulation (what the manufacturer mixes with aspirin in making the tablet) “trick”for aspirin to improve solubility?5. How does this compare with…arrow_forwardA local company sent you their green alternative for window cleaner to be tested for percent (w/v) acetic acid content. For your experiment, you first standardized your NaOH titrant with 0.8053 g of (99.80 % purity) KHP. You used 40.60 mL of NaOH for your standardization. After that you then analyzed a 50.00 mL sample and found that you needed 33.20 ml NaOH to reach the end point. Summary of results: Standardization Sample analysis KHP Weight (g) Purity NaOH (mL) used Determine the following: 0.8053 g Volume of sample 50.00 mL 99.80% NaOH (mL) used 33.20 mL 40.60 mL a. Molarity of NaOH b. % (w/v) acetic acidarrow_forward
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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