Physiological pH in humans is pH = 7.3. At this pH, would cellular carboxylic acid citric acid (Ka1 7.08 x 104) exist primarily as the undissociated free acid or as its dissociated carboxylate form? %3D From the choices provided below, indicate whether the carboxylic acid will exist primarily in its protonated form as a Free Acid or in its deprotonated form as a Carboxylate Anion by clicking on the corresponding button. At equilibrium in this pH, the concentration of the preferred form of the acid is approximately | times higher than the concentration of its conjugate form.

Physiological pH in humans is pH = 7.3. At this pH, would cellular carboxylic acid citric acid (Ka1 7.08 x 104) exist primarily as the undissociated free acid or as its dissociated carboxylate form? %3D From the choices provided below, indicate whether the carboxylic acid will exist primarily in its protonated form as a Free Acid or in its deprotonated form as a Carboxylate Anion by clicking on the corresponding button. At equilibrium in this pH, the concentration of the preferred form of the acid is approximately | times higher than the concentration of its conjugate form.

Organic Chemistry

8th Edition

ISBN:9781305580350

Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Publisher:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. Foote

Chapter4: Acids And Bases

Section4.6: Molecular Structure And Acidity

Problem 1Q: Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity,...

See similar textbooks

Similar questions

Acid-Base Equilibria Many factors contribute to the acidity of organic compounds. Electronegativity, resonance, induction, hybridization, aromaticity, and atomic size, all play a role. In the following comparisons, you are asked to identify the factor(s) that would be most important to analyze when predicting relative acidity, and then to predict the trend in acidity and pKa values. For each of the following pairs of compounds answer the following two multiple-choice questions. 1. What factor(s) are the most important to consider when predicting the relative acidity of the two compounds? a. Electronegativity of the atom possessing the hydrogen. b. Resonance stabilization of the anionic conjugate base. c. Inductive stabilization of the anionic conjugate base. d. Hybridization of the atom possessing the hydrogen. e. The atomic size of the atom possessing the hydrogen.
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.
A 0.119 M solution of Covidenol, a weak acid, has a measured pH of 3.45. Determine the pka of Covidenol.
Determine the principal species at the following pH levels for Nitrilotriacetic acid. The most protonated form is C6H10NO6+. pH= 1,2,3,4,10. pK1 = 1.0, pK2 = 1.81, pK3 = 2.52, pK4 = 9.46.
What is the conjugate acid of H2C6H7O5 -1aq2? What is its conjugate base?
The acid dissociation constant K, of trimethylacetic acid (HC (CH3) CO2 is 9.33 × 10 *. Calculate the pH of a 6.1M solution of trimethylacetic acid. Round your answer to 1 decimal place. PH
Consider the following data on some weak acids and weak bases: acid base Ka K, name formula name formula C;H,N |1.7 × 10~9 4 hydrofluoric acid HF 6.8 × 10 pyridine 10 4.9 x 10 alo 4 hydrocyanic acid НCN ethylamine C2H,NH, | 6.4 × 10 Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a 'l' next to the sofution t will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M C2H5NH3B choose one 0.1 M C5H5NHCI choose one v 0.1 М KI choose one v 0.1 M KF choose one
Determine the direction of equilibrium when acetylene (HC≡CH) reacts with−NH2 in a proton transfer reaction ?
Ascorbic 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 M
A 20 ml solution of 0.1 M glycine hydrochloride has been prepared. How many moles of the weak acid and conjugate base forms of glycine are present after the addition of 620 µl of 1.0 M NaOH? What is the pH of the resulting solution?
For the following acid-base reaction, (1) predict the products, showing both reactants and products complete Lewis structures and arrows showing electron flow; (2) label each structure with the lowing: Bronsted acid, Bronsted base, conjugate acid, conjugate base; (3) give a brief definition of a ronsted acid and Bronsted base; (4) predict the direction of the equilibrium and justify your answer. HC0OH + CH3 Nta PRん106Y pkb = 3.36
1. Solid NH4NO3 dissolves in water and then reacts with KOH (aq). The container releases a smell as the reaction proceeds. (a) Write the acid-base reaction products for this reaction. (b) Write the decomposition reaction that happens immediately after the acid-base reaction that is responsible for the smell observed. 2. Write the complete and balanced Bronsted- Lowry acid-base reaction for the following. Choose the correct arrows to indicate if the reaction goes 100% to completion or is a reversible reaction using equilibrium arrows. (a) H₂S(aq) + NH4OH(aq) (b) HC₂H3O2(aq) + Ca(OH)2 (aq) 3. Use dimensional analysis, proper significant figures & show units. A nicotine-like compound found in tobacco has an empirical formula of C5H7O1 and a molar mass of 160 g/mol. What is the molecular formula of this compound?