(Q8) The Ka of formic acid is 1.8 x 10-4, the Ka of hydrofluoric acid is 6.4 x 10-4 and the K, of hypobromous acid is 2.8 x 10-9. Which of the following statements is true? O Hypobromous acid is a base The weakest conjugate base is fluoride O Hydrofluoric acid is a strong acid The weakest conjugate base is hypobromite O The weakest conjugate base is formate

(Q8) The Ka of formic acid is 1.8 x 10-4, the Ka of hydrofluoric acid is 6.4 x 10-4 and the K, of hypobromous acid is 2.8 x 10-9. Which of the following statements is true? O Hypobromous acid is a base The weakest conjugate base is fluoride O Hydrofluoric acid is a strong acid The weakest conjugate base is hypobromite O The weakest conjugate base is formate

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter14: Acids And Bases

Section: Chapter Questions

Problem 94QRT: Several acids and their respective equilibrium constants are: Which is the strongest acid? Which...

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You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?
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?
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.
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?
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?
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
8-82 Assume that you have a dilute solution of HCI (0.10 M) and a concentrated solution of acetic acid (5.0 M). Which solution is more acidic? Explain.
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?
8-62 What is the pH of a buffer solution made by dissolving 0.10 mol of formic acid, HCOOH, and 0.10 mol of sodium formate, HCOONa, in 1 L of water?
How do the components of a conjugate acid—base pair differ from one another4? Give an example of a conjugate acid—base pair to illustrate your answer.
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