Rank the following organic acids in order of acidity, from strongest to weakest. (Hint: consider how resonance and electronegativity will influence the stability of the conjugate base.) Rank from strongest to weakest. To rank items as equivalent, overlap them. Reset Help Н.С — s— он H,C H,C NH, HO,

Rank the following organic acids in order of acidity, from strongest to weakest. (Hint: consider how resonance and electronegativity will influence the stability of the conjugate base.) Rank from strongest to weakest. To rank items as equivalent, overlap them. Reset Help Н.С — s— он H,C H,C NH, HO,

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. For the following acid - base reaction, (a) predict the products; (b) identify the Bronsted acid, Bronsted base, conjugate acid, and conjugate base; (c) use curved arrows to show the flow of electron pairs in the reaction. CH3 CH2C-OH + NaNHa
4. A student has prepared 0.05 M solution of CH3-C=CH and has added to it 0.05 M solution of potassium tert-butoxide (K" O-C(CH3)3). (i) Write the equation for the acid-base reaction that might occur. (ii) With curved arrows track the movements of electron pairs. (iii) Assign Base, Acid, Conjugate acid for the base, Conjugate base for the acid. (iv) Calculate the percentage of deprotonated methyl acetylene taking into account that pKa of the conjugate acid of potassium tert-butoxide equals 18 and pKa of methyl acetylene equals 24.
What is the expected order of decreasing acidity for the following molecules? HO OO I ||| > |V > | > || | > | > | > h || > | > ||| > |V || > | > IV > ||| * ) III > IV > `|| > | HO II HO CI III HO IV Cl
Consider the following equilibrium between pentanoic acid and its conjugate base: | CH3CH,CH,CH2C0- H20 + H30+ CH;CH2CH,CH,C-OH Will lowering the pH shift the equilibrium to the right or to the left?
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
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3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.
My book says, "Weak bases fall into two general categories. The first category is neutral substances that have an atom with a nonbonding pair of electrons that can accept a proton." Then at the end of the chapter, it asks "Which of the following molecules will act as a weak base?" Among the options on the list that are not weak bases is CH3CH2CH2CH2OH, with an O atom singly bonded to a C and an H (see picture). So it should have 2 nonbonding electron pairs, right? So why doesn't the O on this molecule act as a base by letting an H+ ion share its non-bonded electron?
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