Consider a weak acid "HA". What is the percent ionization of a 0.635 mol L-1 solution of HA? Just enter the percentage as a number and do not include the "%" sign. Report your answer to at least 1 decimal place. The KA of HA is 2.01 x 10-6 . For partial credit, enter the equilibrium [H3O+] (in M) instead.

Consider a weak acid "HA". What is the percent ionization of a 0.635 mol L-1 solution of HA? Just enter the percentage as a number and do not include the "%" sign. Report your answer to at least 1 decimal place. The KA of HA is 2.01 x 10-6 . For partial credit, enter the equilibrium [H3O+] (in M) instead.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 29Q

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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.)
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?
8-112 Consider an initial 0.040 M hypobromous acid (HOBr) solution at a certain temperature. At equilibrium after partial dissociation, its pH is found to be 5.05. What is the acid ionization constant, Ka, for hypobromous acid at this temperature?
Consider the following mathematical expressions. a. [H+] = [HA]0 b. [H+] = (Ka [HA]0)1/2 c. [OH] = 2[B]0 d. [OH] = (Kb [B]0)1/2 For each expression, give three solutions where the mathematical expression would give a good approximation for the [H+] or [OH]. [HA]0 and [B]0 represent initial concentrations of an acid or a base.
Rank the compounds in each of the following groups in order of increasing acidity or basicity, as indicated, and explain the order you assign. (a) acidity: HCI, HBr, HI. (b)basicity: H2O, OH-, H-, CI-. (c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (Hint: Formula could also be written as HCIO4). (d) acidity: HF, H2O, NH3, CH4
If the pH of a solution containing the strong base Sr(OH)2 is 10.46 at 25C, what is the concentration of Sr(OH)2? (a) 3.5 1011 M (b) 2.9 104 M (c) 6.9 104 M (d) 1.4 104 M
The Kb values for ammonia and methylamine are 1.8 105 and 4.4 104, respectively. Which is the stronger acid, NH4+ or CH3NH3+?
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.
What two common assumptions can simplify calculation of equilibrium concentrations in a solution of a weak acid?
Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OCl
The pH of a 0.15-M solution of HSO4- is 1.43. Determine Ka for HSO4- from these data.
Show by suitable net ionic equations that each of the following species can act as a Bronsted-Lowry base: (a) H2O. (b) OH-. (c) NH3. (d) CN-. (e) S2-. (f) H2PO4-