(a)
Interpretation:
The dissociation reactions and
Concept introduction:
The strength of acids and bases can be determined on the basis of their dissociation reactions and their dissociation constants. Those acids or bases which dissociate almost completely are strong acids or strong bases and those which dissociate to smaller extents are weak or moderately weak acids and weak bases.
Answer to Problem 9.84E
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
Explanation of Solution
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
The
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
(b)
Interpretation:
The dissociation reactions and
Concept introduction:
The strength of acids and bases can be determined on the basis of their dissociation reactions and their dissociation constants. Those acids or bases which dissociate almost completely are strong acids or strong bases and those which dissociate to smaller extents are weak or moderately weak acids and weak bases.
Answer to Problem 9.84E
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
Explanation of Solution
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
The
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
(c)
Interpretation:
The dissociation reactions and
Concept introduction:
The strength of acids and bases can be determined on the basis of their dissociation reactions and their dissociation constants. Those acids or bases which dissociate almost completely are strong acids or strong bases and those which dissociate to smaller extents are weak or moderately weak acids and weak bases.
Answer to Problem 9.84E
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
Explanation of Solution
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
The
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
(d)
Interpretation:
The dissociation reactions and
Concept introduction:
The strength of acids and bases can be determined on the basis of their dissociation reactions and their dissociation constants. Those acids or bases which dissociate almost completely are strong acids or strong bases and those which dissociate to smaller extents are weak or moderately weak acids and weak bases.
Answer to Problem 9.84E
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
Explanation of Solution
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
The
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
(e)
Interpretation:
The dissociation reactions and
Concept introduction:
The strength of acids and bases can be determined on the basis of their dissociation reactions and their dissociation constants. Those acids or bases which dissociate almost completely are strong acids or strong bases and those which dissociate to smaller extents are weak or moderately weak acids and weak bases.
Answer to Problem 9.84E
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
Explanation of Solution
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
The
The dissociation reaction for the given weak acid,
The dissociation constant for the given reaction is,
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Chapter 9 Solutions
Study Guide with Student Solutions Manual for Seager/Slabaugh/Hansen's Chemistry for Today: General, Organic, and Biochemistry, 9th Edition
- Ionization of the first proton from H2SO4 is complete (H2SO4 is a strong acid); the acid-ionization constant for the second proton is 1.1 102. a What would be the approximate hydronium-ion concentration in 0.100 M H2SO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.100 M H2SO4, accounting for the ionization of both protons.arrow_forwardIn the following reaction of tetrafluoroboric acid, HBF4, with the acetate ion, C2H3O2, the formation of tetrafluoroborate ion, BF4 , and acetic acid, HC2H3O2 is favored. HBF4+C2H3O2BF4+HC2H3O2 Which is the weaker base, BF4 or acetate ion?arrow_forwardConsider 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.arrow_forward
- . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.arrow_forwardProve that Ka3 Kb1 = Kw for phosphoric acid, H3PO4, by adding the chemical equilibrium expressions that corresponds to the third ionization step of the acid in water with the first of the three successive steps of the reaction of phosphate ion, PO43, with water.arrow_forwardNicotine, C10H14N2, is a base that will accept two protons (K1=7107,K2=1.41011). What is the concentration of each species present in a 0.050-M solution of nicotine?arrow_forward
- 25. Which of the following acids have relatively strong conjugate bases? a. HCN b. H2S c. HBrO4 d. HNO3arrow_forwardHow 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?arrow_forwardFrom the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb, for each of the weak bases. (a). CH3CO2H:[H3O+]=1.34103M;[CH3CO2]=1.34103M;[CH3CO2H]=9.866102M; (b). ClO:[OH]=4.0104M;[HClO]=2.38105M;[ClO]=0.273M; (c). HCO2H:[HCO2H]=0.524M;[H3O+]=9.8103M;[HCO2]=9.8103M; (d). C6H5NH3+:[C6H5NH3+]=0.233M;[C6H5NH2]=2.3103M;[H3O+]=2.3103Marrow_forward
- 3. A solution is 0.5 M NH4OCl. a. Determine the major species in this solution. b. Identify the strongest acid and strongest base in the solution and write the equilibrium reaction between these two. c. Calculate the equilibrium constant for the reaction in (b) using the equilibrium constants from Table 14.2 and 14.3 in your textbook. Note that the reaction for the autodissociation of water may also be helpful here. d. Calculate the equilibrium concentrations of NH4 + , NH3, HOCl, and OCl- . e. Use the equilibrium constant(s) from (c) to calculate the pH of the solution. f. This problem generally reads “Calculate the pH of a 0.5 M NH4OCl solution.” Recap in general terms the steps taken to solve this problem.arrow_forward161.) A weak acid, HA, is a monoprotic acid. A solution that is 0.200 M in HA has a pH of 2.210 at 25°C.HA(aq) + H2O(l) ⇄ H3O+(aq) + A-(aq)What is the acid-ionization constant, Ka, for this acid? What is the degree of ionization of the acid in this solution? Ka = Degree of ionization =arrow_forwardFor each reaction shown below, indicate the Lewis Acids and the Lewis Bases: Ni2+(aq) + 6 H2O(l) => Ni(H2O)62+(aq) Fe2+(aq) + 6 CN-(aq) => Fe(CN)64-(aq)arrow_forward
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