Answered: PKa of benzene: 43 pka of acetone: 19.2…

Science

Chemistry

PKa of benzene: 43 pka of acetone: 19.2 pka of acetic acid: 4.75

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter24: Nuclear Chemistry

Section: Chapter Questions

Problem 103A

See similar textbooks

Similar questions

The observed yield; acetaminophen
Alkaloids are basic nitrogen-containing compounds of plant origin, many of which are physiologically active when administered to humans. Ingestion of coniine, isolated from water hemlock, can cause weakness, labored respiration, paralysis, and eventually death. Coniine is the toxic substance in the “poison hemlock” used in the death of Socrates. In small doses, nicotine is an addictive stimulant. In larger doses, it causes depression, nausea, and vomiting. In still larger doses, it is a deadly poison. Solutions of nicotine in water are used as insecticides. Cocaine is a central nervous system stimulant obtained from the leaves of the coca plant.Classify each amino group in these alkaloids according to type (primary, secondary, tertiary, aliphatic, aromatic, heterocyclic).
The amount of tartaric acid is responsible for the tartness of wine and controls the acidity of the wine. Tartaric acid also plays a very significant role in the overall taste, feel and color of a wine. Tartaric acid is a diprotic organic acid The chemical formula for tartaric acid is C4H6O6 and its structural formula is HO2CCH(OH)CH(OH)CO2H. A 50.00 mL sample of a white dinner wine required 21.48 mL of 0.03776 M NaOH to achieve a faint pink color. Express the acidity of the wine in terms of grams of tartaric acid, H2C4H4O6 (M. M. = 150.10) per 100 mL of wine. Assume that the two acidic hydrogens are titrated at the end point. MM H2C4H4O6 = 150.10 MM NaOH = 40.00 Below is the balanced chemical equation for this titration.
Ascorbic acid, H₂C6H6O6, is a diprotic acid usually known as vitamin C. For this acid, pk1 is 4.10 and pKa2 is 11.79. When 125 mL of a solution of ascorbic acid was evaporated to dryness, the residue of pure ascorbic acid had a mass of 3.30 g. Calculate the molar concentration of ascorbic acid in the solution before it was evaporated. i What was the pH of the ascorbic acid solution before it was evaporated? pH = i What was the concentration of the ascorbate ion, C6H6062, before the solution was evaporated? i M M
Cyclohexanone is oxidized to adipic acid with the following equation. Twenty gram (20g) of cyclohexanone is used and 15 g of product is obtained in this reaction. Calculate the percentage of yield of product in this reaction. * HO. HO. (0) (0) OH он
Organic Chemistry II: When nitrating Methyl benzoate, which compound is the limiting reactant?
Use the following reagent table for the reaction of : cyclohexanol + H2 SO4 → cyclohexene Chemical MW (g/mol) Density (g/mL) mmols used Amount used cyclohexanol 100.16 0.9624 1.50 mL Sulfuric Acid 98.08 1.83 1.00 mL cyclohexene 82.14 Using the information from the previous questions, if 0.95 g of cyclohexene were formed during the reaction, determine the % yield. Answer with 2 decimal places.
2.5 grams of methyl orange was synthesized by using sulfanilic acid dihydrate, 3 g of anhydrous Na2CO3, 3.5 g of NaNO2, 12 mL of HCl and 6 mL of N,N-dimethylaniline and other necessary chemicals. Write down all the reaction steps and calculate the % yield of methyl orange synthesized
theoretical yield for reaction theoretical mass for stilbene, acetic acid, and pyridinium tribomide stilbene: 0.5 g acetic acid: 10 mL pyridinium: 1.0 g
3) When acetic anhydride is dissolved in water, it forms acetic acid according to the balanced chemical reaction shown below. Calculate the theoretical yield (in grams of acetic acid, FW 60.05 g/mol) if 10.43 mL of acetic anhydride (FW 102.09 g/mol, d. 1.08 g/mL) is used. You can assume that the water is present in excess. H2O 2 HO, acetic anhydride acetic acid
1. For the following reaction, OEt ethyl 2-phenylacetate C10H12O2 164.20 g/mol 1. NaOEt 2. H3O+ алд OEt ethyl 3-oxo-2,4-diphenylbutanoate C18H1803 282.34 g/mol b. What is the theoretical yield, using the amounts given in part a? c. What is the percent yield if 0.328 g of product are isolated? EtOH a. What is the limiting reagent when 0.495 g of ethyl 2-phenylacetate is combined with 1.20 g of sodium ethoxide (NaOEt, 68.05 g/mol)? ethanol C₂H6O 46.07 g/mol
1-butanol yields 1-bromobutane in the presence of concentrated sulfuric acid and an excess of sodium bromide. CH3CH2CH2CH2OH (l) → CH3 CH2CH2CH2Br (l) If 15.89 mL of 1-butanol produced 12.23 g of 1-bromobutane, the percentage yield of the product equals: (Assume the density of 1-butanol is 0.81 g/mL, the molar mass of 1-butanol is 74 g/mol, and the molar mass of 1-bromobutane is 137 g/mol.) %