A ka of weak acid is 1 E-6, this means that For 1 million unionized acid, there is just one molecule is ionized .a O The concentration of hydronium ion equals the square root of its pKa value .b O For 1 million ionized acid, there is just one molecule is unionized .c O The concentration of hydroxyl ion equals the square root of its pka value .d O

A ka of weak acid is 1 E-6, this means that For 1 million unionized acid, there is just one molecule is ionized .a O The concentration of hydronium ion equals the square root of its pKa value .b O For 1 million ionized acid, there is just one molecule is unionized .c O The concentration of hydroxyl ion equals the square root of its pka value .d O

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 4.10P: Complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow...

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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
Use Table 13-2 to order the following from the strongest to the weakest acid. HClO2,H2O,NH4+,HClO4
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.
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:
16-27 Guanidine, p/Ca 13.6, is a very strong base, almost as basic as hydroxide ion. NH NH2+ II II H2N—C—NH2 + H2O H2N—C—NH2 + OH" Guanidine Guanidinium ion pKb = 13.6 Complete the Lewis structure for guanidine, showing all valence electrons. The remarkable basicity of guanidine is attributed to the fact that the positive charge on the guanidinium ion is delocalized by resonance over the three nitrogen atoms. This delocalization increases the stability of the guanidinium ion relative to the ammonium ion or substituted ammonium ions. Draw three equivalent contributing structures for the guanidinium ion and show by the use of curved arrows how these three contributors are related. Propose an explanation for the fact that protonation occurs on the C=NH nitrogen rather than on one of the —NH., nitrogens. (Hint: Consider the resonance stabilization of the structure formed by protonation on a —NH., nitrogen compared with the resonance stabilization of the structure formed by protonation on the =NH nitrogen.) Predict the N—C—N bond angles in the hybrid. Which is the stronger acid, the ammonium ion or the guanidinium ion?
. For each pair of concentrations, tell which represents the more basic solution. a. [H+]=2.02107Mor[OH-]=5.05105M b. [H+]=1.79105Mor[OH-]=4.21106M c. [H+]=1.251012Mor[OH-]=6.51103M
Calculate Ka for the weak acids that have the following PKa values. (a) 3.9(b) 10.12 (c) 13.07
Which of the following compounds or ions has the weakest conjugate base? Briefly explain your choice. a) HCN b) HClO c) NH4+