Concept explainers
(a)
Interpretation: The structure of the conjugate acid of monosodium phosphate (base) needs to be determined.
Concept Introduction:Bronsted and Lowry purposed the Bronsted-Lowry acid-base theory. It states that acid can give
(b)
Interpretation: The reason of ineffective use of an aqueous solution of monosodium phosphate for extracting benzoic acid from a diethyl ether solution needs to be explained, if the pKa of conjugate acid of monosodium phosphate is 2.1.
Concept Introduction:Bronsted and Lowry purposed the Bronsted-Lowry acid-base theory. It states that acid can give
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EBK EXPERIMENTAL ORGANIC CHEMISTRY: A M
- What is the pH of an aqueous solution containing 0.50 mol L–1 ethanoic acid, 0.30 mol L–1 sodium ethanoate, and 0.10 mol L–1 HCl? [The pKa of ethanoic acid is 4.75.]arrow_forward(HC(CH₂), CO₂) is 9.33 × 106. x Calculate the pH of a 2.8 M solution of trimethylacetic acid. Round your answer to 1 decimal place. The acid dissociation constant K of trimethylacetic acid pH = 0 X 5arrow_forwardWrite the chemical equation for the acid dissociation of acetaminophen, C8H9O2N. Write the Ka expression for the acid dissociation of acetaminophen.arrow_forward
- (a) Predict the products of the following acid-base reactions using curved-arrow mechanisms to indicate electron flow. (b) Indicate the acid, base, conjugate acid, and conjugate base of each reaction. (c) Indicate whether the reactants or products are favored at equilibrium a) CH,COOH CH3O b) CH,CH,OH H2Narrow_forwardWhat is the conjugate acid of H2C6H7O5 -1aq2? What is its conjugate base?arrow_forwardThe pH of a 0.12 M solution of acetic acid (HCH3CO2) is measured to be 2.83. Calculate the acid dissociation contant Ka of acetic acid.arrow_forward
- Calculate the pH of a 0.020 M solution of phenylacetic acid, C6H5CH2COOH. What will be the pH if the solution is made 0.050 M with its sodium salt, C6H5CH2COONa? Ka= 4.9 x 10-5.arrow_forwardPhenylamine is an aromatic amine that is used in the manufacture of dyes. When absorbed through the skin itcauses the Fe+2 in hemoglobin to become oxidized into Fe+3, resulting in the formation of methemoglobin whichcannot bind to or transport oxygen. Phenylamine is soluble in water and acts as a weak base.C6H5NH2 (aq) + H2O (ℓ) ⇋ C6H5NH3+ (aq) + OH- (aq)a. When you measure the concentrations of the ionized substances you find them to be:[C6H5NH2] = 0.234 mol/L [C6H5NH3+] = 2.8 x 10-5 mol/L [OH-]= 2.8 x 10-5 mol/LIf the Kb is 4.27 x 10-10, is the reaction at equilibrium? If not, which direction does it need to move (rightor left) to reach equilibrium? Explain. b. At equilibrium the concentrations of the ionized substances are:[C6H5NH2] = 0.0537 mol/L [C6H5NH3+] = 4.79 x 10-6 mol/L [OH-]= 4.79 x 10-6 mol/LIf this reaction is taking place in a 2.0L container, and 1.5 moles of phenylamine were added to thereaction, what will the new concentrations of the three ionic species be when…arrow_forwardWrite a net ionic equation to show that piperidine, C5H11N, behaves as a Bronsted-Lowry base in water.arrow_forward
- 2,4-Pentanedione is a considerably stronger acid than is acetone (Chapter 19). Write a structural formula for the conjugate base of each acid and account for the greater stability of the conjugate base from 2,4-pentanedione.arrow_forwardAscorbic acid, H2C6H6O6, is a diprotic acid usually known as vitamin C. For this acid, pKa1 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 3.64 g. Your answer is correct. Calculate the molar concentration of ascorbic acid in the solution before it was evaporated. 0.164 Hint Your answer is partially correct. What was the pH of the ascorbic acid solution before it was evaporated? pH = 2.44 What was the concentration of the ascorbate ion, C6H6062, before the solution was evaporated? i M Marrow_forwardThe acid dissociation constant K of trimethylacetic acid (HC(CH³)₂CO₂) is 9.33 × 10¯6. a Calculate the pH of a 3.6M solution of trimethylacetic acid. Round your answer to 1 decimal place. pH = - 0 X Śarrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning