15. The compounds below are the conjugate bases of the acidslisted on the right. Using the pKa values on the right, state whichof the following is the strongest base?pkaAcidCH3CH3 51NH3H-C=C-H3825A) H-C=C B) CH3CH2C) NH3D) NHàE) CH3COO¯CH3COOH 4.8NH4+9.2

From the pKa value how strong the acid is can be predicted. Higher is the pKa value, weaker is the…

Answered: 15. The compounds below are the…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 93AP

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Define or illustrate the meaning of the following terms: a. Ka reaction b. Ka equilibrium constant c. Kb reaction d. Kb equilibrium constant e. conjugate acidbase pair
What is the conjugate acid of each of the following? What is the conjugate base of each?. (a) OH-. (b) H2O. (c) HCO3-. (d) NH3. (e) HSO4-. (f) H2O2. (g) HS-. (h) H5N2+
Calculate Ka for the weak acids that have the following PKa values. (a) 3.9(b) 10.12 (c) 13.07
What is the conjugate acid of each of the following? What is the conjugate base of each?. (a) H2S. (b) H2 PO4-. (c) PH3. (d) HS-. (e) HSO3-. (f) H3O2+. (g) H4N2. (h) CH3OH
Predict which acid in each of the following pairs is the stronger and explain your reasoning for each.. (a) H2O or HF. (b) B(OH)3 or Al(OH)3. (c) HSO3- or HSO4-. (d) NH3 or H2S. (e) H2O or H2Te
Several acids and their respective equilibrium constants are: Which is the strongest acid? Which is the weakest acid? Which acid has the weakest conjugate base? Which acid has the strongest conjugate base?
Calculate the [OH] of each of the following solutions at 25C. Identify each solution as neutral, acidic, or basic. a. [H+] = 1.0 107 M b. [H+] = 8.3 1016 M c. [H+] = 12 M d. [H+] = 5.4 105 M 46. Calculate the [H+] of each of the following solutions at 25C. Identify each solution as neutral, acidic, or basic. a. [OH] = 1.5 M b. [OH] = 3.6 1015 M c. [OH] = 1.0 107 M d. [OH] = 7.3 104 M 49. Calculate the pH and pOH of the solutions in Exercises 45 and 46.
Use Table 13-3 to help answer the following questions. a. Which is the stronger base, ClO4 or C6H5NH2? b. Which is the stronger base, H2O or C6H5NH2? c. Which is the stronger base, OH or C6H5NH2? d. Which is the stronger base, C6H5NH2 or CH3NH2?
Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow of electron pairs in each reaction. In addition, write Lewis structures for all starting materials and products. Label the original acid and its conjugate base; label the original base and its conjugate acid. If you are uncertain about which substance in each equation is the proton donor, refer to Table 4.1 for the relative strengths of proton acids. (a) NH3+HCl (b) CH3CH2O+HCl (c) HCO3+OH (d) CH3COO+NH4+
A very strong base can remove a proton from methylamine:
Answer true or false to the following statements about the mechanism of acid-base reactions. (a) The acid and base must encounter each other by a collision in order for the proton to transfer. (b) All collisions between acids and bases result in proton transfer. (c) During an acid-base reaction the lone pair on the base fills the A-H antibonding sigma orbital.
The butylammonium ion, C4H9NH3+, has a Ka of 2.3 1011. C4H9NH3+(aq) + H2O() H3O+(aq) + C4H9NH2(aq) a) Calculate Kb for the conjugate base, C4H9NH2 (butyl amine). b) Place the butylammonium ion and its conjugate base in Table 16.2. Name an acid weaker than C4H9NH3+ and a base stronger than C4H9NH3. c) What is the pH of a 0.015M solution of butylammonium chloride?

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15. The compounds below are the conjugate bases of the acids listed on the right. Using the pKa values on the right, state which of the following is the strongest base? pka Acid CH3CH3 51 NH3 H-C=C-H 38 25 A) H-C=C B) CH3CH2 C) NH3 D) NHà E) CH3COO¯ CH3COOH 4.8 NH4+ 9.2