Concept explainers
Using the equilibrium constants listed in Table 13.2, arrange the following 0.1 M aqueous solutions in order of increasing pH (from lowest to highest).
(a) NaNO2
(b) HCl
(c) NaF
(d) Zn(H2O)3(OH)(NO3)
Interpretation: The order of increasing pH value needs to be determined.
Concept Introduction: The dissociation reaction of a weak base is represented as follows:
The expression for the base dissociation constant will be as follows:
Here,
From hydroxide ion concentration, pOH of the solution can be calculated as follows:
From pOH, pH of the solution can be calculated as follows:
Answer to Problem 67QAP
0.1 M
Explanation of Solution
The given aqueous solutions are as follows:
M
Here, HCl is a strong acid thus, it completely dissociates in the solution.
From the table 13.2, the equilibrium constants for
(a)
The dissociation reaction of
The equilibrium constant can be calculated as follows:
Putting the values,
Thus,
Therefore, the value of
Thus,
The pOH of the solution can be calculated as follows:
Putting the values,
The pH of the solution can be calculated as follows:
Putting the values,
(b)
HCl is a strong acid, the dissociation can be represented as follows:
Since, molarity of HCl is 0.1 M thus, concentration of hydrogen ion is 0.1 M.
The pH of the solution can be calculated as follows:
Putting the value,
(c)
0.1 M
The dissociation reaction can be represented as follows:
The equilibrium constant for the reaction will be:
Putting the values,
Thus,
The value of x cannot be negative thus, it is equal to
Thus,
The pOH of the solution can be calculated as follows:
Putting the value,
The pH of the solution can be calculated as follows:
Putting the value,
(d)
0.1 M
The decomposition reaction can be represented as follows:
The equilibrium constant for the reaction will be:
Putting the values,
Thus,
Since, the value of x cannot be negative thus, it is equal to
Since,
The pH of the solution can be calculated as follows:
Putting the values,
The order of increasing pH value can be represented as follows:
0.1 M
Thus, the order of increasing pH value can be represented as follows:
0.1 M
Want to see more full solutions like this?
Chapter 13 Solutions
OWLV2 FOR MASTERTON/HURLEY'S CHEMISTRY:
- The weak base, CIO (hypochlorite ion), is used in the form of NaCIO as a disinfectant in swimming pools and water treatment plants. What are the concentrations of HCIO and OH and the pH of a 0.015 M solution of NaCIO?arrow_forwardEqual molar quantities of ammonia and sodium dihydrogen phosphate (NaH2PO4) are mixed. (a) Write a balanced, net ionic equation for the acid-base reaction that can, in principle, occur. (b) Does the equilibrium lie to the right or left?arrow_forwardWrite the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HF (hydrofluoric acid) b. HC2H3O2 (acetic acid)arrow_forward
- Aluminum chloride, AlCl3, reacts with trimethyl-amine, N(CH3)3. What would you guess to be the product of this reaction? Explain why you think so. Describe the reaction in terms of one of the acid base concepts. Write an appropriate equation to go with this description. Which substance is the acid according to this acidbase concept? Explain.arrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forwardTile pH of a solution of household ammonia, a 0.950 M solution of NH3 is 11.612. Determine Kb for NH3 from these data.arrow_forward
- What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.arrow_forwardBoric acid, B(OH)3, is used as a mild antiseptic. What is the pH of a 0.015 M aqueous solution of boric acid? What is the degree of ionization of boric acid in this solution? The hydronium ion arises principally from the reaction B(OH)3(aq)+2H2O(l)B(OH)4(aq)+H3O+(aq)arrow_forwardWhich of the diagrams in Problem 10-135 represents the substance that is the weakest electrolyte?arrow_forward
- A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?arrow_forwardWrite the acid ionization constant expression for the ionization of each of the following monoprotic acids. a. HCN (hydrocyanic acid) b. HC6H7O6 (ascorbic acid)arrow_forwardRank 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: HCl, HBr, HI(b) basicity: H2O, OH−, H−, Cl−(c) basicity: Mg(OH)2, Si(OH)4, ClO3(OH) (d) acidity: HF, H2O, NH3, CH4arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning