### Acids and pKa Values**Acetic Acid and Trifluoroacetic Acid:**Chemical structures:- **Acetic Acid**: H₃C—C(=O)—OH- **Trifluoroacetic Acid**: F₃C—C(=O)—OHThe pKa of acetic acid is 4.75. **Question:** Which of the following statements is false?1. The pKa of trifluoroacetic acid is larger than 4.75.2. The conjugate base of trifluoroacetic acid is stabilized inductively.3. The conjugate base of acetic acid is stabilized by resonance.4. The pKa of trifluoroacetic acid is lower than 4.75.5. The conjugate base of trifluoroacetic acid is stabilized by resonance.### Explanation:- **Inductive Effect**: Refers to electron withdrawing by electronegative atoms, which stabilizes the conjugate base.- **Resonance**: Involves delocalization of electrons that stabilizes molecules.### Practice Question for Deeper Understanding:**Question 40:** What product(s) is/are formed in the following reaction?*(The specific reaction is not visible in the image)*

Note: a,b are false because pka valude of trifluoroacetic acid is lower than acetic acid. The…

Consider acid acid and trifluoroacetic acid. The pKa of acetic acid is 4.75. VWhich of the statements below is false? H3C OH F3C HO. acetic acid trifluoroacetic acid O The pka of trifluoroacetic acid is larger than 4.75 O The conjugate base of trifluoroacetic acid is stabilized inductively O The conjugate base of acetic acid is stabilized by resonance O The pka of trifluoroacetic acid is lower than 4.75 O The conjugate base of trifluoroacetic acid is stabilized by resonance

Consider acid acid and trifluoroacetic acid. The pKa of acetic acid is 4.75. VWhich of the statements below is false? H3C OH F3C HO. acetic acid trifluoroacetic acid O The pka of trifluoroacetic acid is larger than 4.75 O The conjugate base of trifluoroacetic acid is stabilized inductively O The conjugate base of acetic acid is stabilized by resonance O The pka of trifluoroacetic acid is lower than 4.75 O The conjugate base of trifluoroacetic acid is stabilized by resonance

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...

See similar textbooks

Similar questions

Upload an image that you found useful to explain the concept of pKa (acid dissociation constant), and answer the following: 1. What does the image tell you about pKa? Explain in 1-2 sentences. 2. Where did you find the image? 3. Do you think the source of the image is reliable? Explain in 1-2 sentences why or why not the source is reliable.
1. If a drug is a weak acid pka = 3.5; absorbed in the non-ionized form. What % is absorbed in the stomach (pH 1 -2), duodenum (pH 6.5) ?
A chemical reaction does not occur for Submit Request Answer Part D Enter the conjugate acid for HCO3. Express your answer as a chemical formul. ΑΣΦ A chemical reaction does not occur for this q Submit Request Answer
Consider the following five weak acids: Succinic acid: pKa = 4.16 НOBr: Ka%3D 2.06 х 10°9 Dinicotinic: pKą = 2.08 Nitrobenzoic: Ka = 6.95 x 10-3 Saccharin: pKa = 11.68 Order these acids from the strongest (1) to the weakest (5) Dinicotinic [Choose] Saccharin [ Choose] Nitrobenzoic [Choose] НOBr [Choose] Succinic acid [Choose]
Which of the compounds shown below is the most acidic hydrogen and what is the approximate pKa value?
Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid B C Ka M 0 7.28 x 10 pK 1.17 11.3 0 relative strength (Choose one) ✓ (Choose one) ✓ (Choose one) ✓ O *10 X ?
Provide your view on this? Strong bases have weak conjugate acids with high pKa values, usually > 12.
Extra credit. Which of the following approximate pKa ranges for the following acids is correct? You don't need a calculator (i.e., between 3 and 4, between 9 and 10 etc. There may be more than one correct answer. HNO2 Ka = 4.0 x 10-4 pKa between 3 and 4 HCO3- Ka = 6.3 x 10-11 pKa between 10 and 11 HCO2H Ka = 2.0 x 10-4 pKa between 3 and 4 HCN Ka = 7.9 x 10-10 pKa between 8 and 9
1. What is the value of Kb for H2PO4-? A. 1.3 x 10-12 B. 1.6 x 10-7 C. 6.2 x 10-8 D. 7.5 x 10-3 2. Which of the equations has a Bronsted-Lowry conjugate acid-base pair? A. 2H2 + O2 ß à H2O C. Zn + 2HCl à H2 + ZnCl2 B. NaOH à Na+ + OH- D. H2O + HCN ßà H3O+ + CN- 3. What is the conjugate base of HSO4-(aq)? A. OH-(aq) B. H2SO4(aq) C. H3O + (aq) D. SO4 2-(aq) 4. Which term describes a substance that acts as a proton donor and a proton acceptor? A. amphoteric B. monoprotic C. polyprotic D. acid-base 5. What is t What is the concentration of hydroxide ions in a solution of 0.350 mol/L HCl(aq)? A. 0.350 mol/L B. 0.175 mol/L C. 2.86 x 10-14 mol/L D. 0.650 mol/L 6. A solution contains 3.3 x10-8 M hydroxide ions. What is the pH of the solution? A. 3.25 B. 6.51 C. 7.49 D. 8.00 7. A solution has a pH of…
Complete the following table, which lists information about the measured acid dissociation constants of three unknown weak acids. Note: be sure each number you put in the table has the correct number of significant digits. acid K pK relative strength x10 A ✓ (Choose one) X S ? 1 (strongest) B 2 3 (weakest) с (Choose one) Ba -5 8. × 10 5.89 × 10 -9 7.02 1 0
15. Dimethylamine (CH3)2NH is a weak base with a pKą of 11.0 Calculate the pH of a solution of dimethylamine at 0.40 mol.L-1. b. Calculate the pH of a solution of dimethylamine at 4.0 x 10-2 mol.L-¹.
What is Ka for the conjugate acid of C5H§N (Kb = 1.7 x 10-°)? 1 2 3 C 7 9. +/- x 10 0 LO 00