6. Which of the following bases are strong enough to remove a proton from the acid below?Justify your answer with approximate pKa values.iNH3acidNHOH

Carboxylate ion (fig. 1) cannot act as strong base because negative charge on oxygen atom is in…

Answered: 6. Which of the following bases are…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 37QAP

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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+
Write the base ionization constant expression for the ionization of each of the following bases. In each case, the nitrogen atom accepts the proton. a. CH3NH2 (methylamine) b. C2H5NH2 (ethylamine)
Which of the following compounds or ions has the weakest conjugate base? Briefly explain your choice. a) HCN b) HClO c) NH4+
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?
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) C2H5N(aq) + CH3CO2H(aq) C5H5NH+(aq) + CH3CO2(aq) (b) N2H4(aq) + HSO4(aq) N2H5+(aq) + SO42(aq) (c) [Al(H2O)6]3+ (aq) + OH(aq) [Al(H2O)5OH]2+ (aq) + H2O+()
How is acid strength related to the value of Ka? What is the difference between strong acids and weak acids (see Table 13-1)? As the strength of an acid increases, what happens to the strength of the conjugate base? How is base strength related to the value of Kb? As the strength of a base increases, what happens to the strength of the conjugate acid?
75. A conjugate acid-base pair Consists of two substances related by the donating and accepting of a(n) ________
What two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak acid?
Write the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HCN (hydrocyanic acid) b. HC6H7O6 (ascorbic acid)
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
Consider these acids (a) Arrange the acids in order of increasing acid strength from weakest to strongest. (b) Which acid has the smallest pKa value?
For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.

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6. Which of the following bases are strong enough to remove a proton from the acid below? Justify your answer with approximate pKa values. i NH3 acid NH OH