(a)
Interpretation:
From the given
Concept introduction:
The weak acid does not dissociate completely in a
For a general reaction of ionization of weak acid as follows:
The expression for dissociation constant of the reaction is as follows:
The
(b)
Interpretation:
From the given
Concept introduction:
The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.
For a general reaction of ionization of weak acid as follows:
The expression for dissociation constant of the reaction is as follows:
The
(c)
Interpretation:
From the given
Concept introduction:
The weak acid does not dissociate completely in a chemical reaction thus, the ionization equation is in equilibrium.
For a general reaction of ionization of weak acid as follows:
The expression for dissociation constant of the reaction is as follows:
The
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Chemistry: Principles and Reactions
- 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.)arrow_forwardThe pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.arrow_forwardThe following reactions illustrate Brnsted acid-base behavior. Complete each equation. a.HI(aq)+?H3O+(aq)+I(aq) b.NH3(l)+?NH4++NH2 c.H2C2O4(aq)+H2O(l)?+HC2O4(aq) d.H2N2O2(aq)+H2O(l)H3O+(aq)+? e.?+H2O(l)H3O+(aq)+CO32(aq)arrow_forward
- Calculate Ka for the weak acids that have the following PKa values. (a) 3.9(b) 10.12 (c) 13.07arrow_forwardConsider these acids (a) Arrange the acids in order of increasing acid strength from weakest to strongest. (b) Which acid has the smallest pKa value?arrow_forwardDefine 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 pairarrow_forward
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- 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.arrow_forwardWhich of the following compounds or ions has the weakest conjugate base? Briefly explain your choice. a) HCN b) HClO c) NH4+arrow_forwardYou 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?arrow_forward
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