The undissociated base (B) is present in the greatest concentration, with theproducts being present in relatively smaller amounts in this equilibrium mixture.How would this affect the magnitude of Kb? Do you expect it to be small or large?Which is the strongest base?Name of baseAmmonia (NH3)Methylamine (CH3NH2)Ethylamine (C2H5NH2)Diethylamine (C2H5)2NHPyridine (CSH5N)Kb value1.76 x 10-5Why?4.4 x 10-45.6 x 10-4Which is the weakest base?1.3 x 10-31.7 x 10-9Why?The larger the Kb the(stronger/weaker) the base.Since a weak base dissociates incompletely setting up an equilibrium, what methodcould you think of that you could use to determine the concentration of [OH"] ionsgiven the initial concentration of the acid and its Kb?

Answer: This question is based on the study of relative strength of weak bases where by comparing…

The undissociated base (B) is present in the greatest concentration, with the products being present in relatively smaller amounts in this equilibrium mixture. How would this affect the magnitude of Kb? Do you expect it to be small or large? Which is the strongest base? Name of base Ammonia (NH3) Methylamine (CH3NH2) Ethylamine (C2HSNH2) Diethylamine (C2Hs)2NH Pyridine (CsHsN) Kb value 1.76 x 105 Why? 4.4 x 104 5.6 x 104 Which is the weakest base? 1.3 x 10-3 1.7 x 109 Why? The larger the Kb the. (stronger/weaker) the base. Since a weak base dissociates incompletely setting up an equilibrium, what method could you think of that you could use to determine the concentration of (OH"] ions given the initial concentration of the acid and its Kb?

The undissociated base (B) is present in the greatest concentration, with the products being present in relatively smaller amounts in this equilibrium mixture. How would this affect the magnitude of Kb? Do you expect it to be small or large? Which is the strongest base? Name of base Ammonia (NH3) Methylamine (CH3NH2) Ethylamine (C2HSNH2) Diethylamine (C2Hs)2NH Pyridine (CsHsN) Kb value 1.76 x 105 Why? 4.4 x 104 5.6 x 104 Which is the weakest base? 1.3 x 10-3 1.7 x 109 Why? The larger the Kb the. (stronger/weaker) the base. Since a weak base dissociates incompletely setting up an equilibrium, what method could you think of that you could use to determine the concentration of (OH"] ions given the initial concentration of the acid and its Kb?

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

Section: Chapter Questions

Problem 4.21P: Answer true or false to the following statements about the mechanism of acid-base reactions. (a) The...

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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.
Predict the position of equilibrium for this acid-base reaction.
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?
Complete the equation for the reaction between each Lewis acid-base pair. In each equation, label which starting material is the Lewis acid and which is the Lewis base; use curved arrows to show the flow of electrons in each reaction. In doing this problem, it is essential that you show valence electrons for all atoms participating in each reaction. (a) (b) (c) (d)
5. Given the general equation illustrating the reaction of the acid HA in water, HA(aq)+H2O(l)H3O+(aq)+A(aq)explain why water is considered a base in the Brønsted-Lowry model.
Will acetylene react with sodium hydride according to the following equation to form a salt and hydrogen, H2? Using pKa values given in Table 4.1, calculate Keq for this equilibrium.
Which of the following two acids has the stronger conjugate base? Nitrous acid, Ka = 7.1 x 10–4 Phenol, Ka = 1.0 x 10–10 The strength of the conjugate base cannot be obtained from the information given. Nitrous acid, because it has a larger Ka value. Nitrous acid, because it has a smaller Ka value. Phenol, because it has a larger Ka value. Phenol, because it has a smaller Ka value.
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If 0.100 mol of phenol, C6H5OH, were dissolved in pure water to make 1.000 L of total solution, what would the concentration of C6H5O- be at equilibrium? What would the acid’s percent dissociation be?
Benzoic acid (C6H5COOH) and aniline (C6H5NH2) areboth derivatives of benzene. Benzoic acid is an acid withKa = 6.3 x10-5 and aniline is a base with Ka = 4.3 x10-10. (a) What are the conjugate base of benzoic acid andthe conjugate acid of aniline? (b) Anilinium chloride(C6H5NH3Cl) is a strong electrolyte that dissociates intoanilinium ions (C6H5NH3+) and chloride ions. Which willbe more acidic, a 0.10 M solution of benzoic acid or a 0.10M solution of anilinium chloride? (c) What is the value ofthe equilibrium constant for the following equilibrium?C6H5COOH(aq) + C6H5NH2(aq) ⇌ C6H5COO-(aq) + C6H5NH3+(aq)
Which of the following has the strongest conjugate base? Group of answer choices benzoic acid (Ka = 6.5 x 10-5) hydrazoic acid (Ka = 1.9 x 10-5) chlorous acid (Ka = 1.1 x 10-2) carbonic acid (Ka = 4.3 x 10-7) chloroacetic acid (Ka = 1.4 x 10-3)
1) Complete the following reactions and identify the acid, base, conjugate acid and conjugate base. CH;CH,NH2 (aq) + H2O (1) a) CH;COOH (aq) + H,O (I) b) c) Identify the conjugate base and conjugate acid of each of the following. Conjugate Base Molecule Conjugate Acid HCO3 H20 HSO4- H2PO4