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Problem 37
Both H2O and H2PO4– are amphoteric. Write an equation to show how each substance can act as an acid and another equation to show how each can act as a base.
Problem 39a
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). a. HNO3
Problem 39b
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). b. HCl
Problem 39c
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). c. HBr
Problem 39d
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). d. H2SO3
Problem 40a
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). a. HF
Problem 40b
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). b. HCHO2
Problem 40c
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). c. H2SO4
Problem 40d
Classify each acid as strong or weak. If the acid is weak, write an expression for the acid ionization constant (Ka). d. H2CO3
- The three diagrams represent three different solutions of the binary acid HA. Water molecules have been omitted for clarity, and hydronium ions (H3O+) are represented by hydrogen ions (H+). Rank the acids in order of decreasing strength.
Problem 41
Problem 43
Rank the solutions in order of decreasing [H3O+]: 0.10 M HCl; 0.10 M HF; 0.10 M HClO; 0.10 M HC6H5O.
Problem 46c
Pick the stronger base from each pair. c. NO2– or NO3–
- Calculate the pH and pOH of each solution at 25 °C. a. [H3O+] = 1.7 × 10^-8 M b. [H3O+] = 1.0 × 10^-7 M c. [H3O+] = 2.2 × 10^-6 M
Problem 51
Problem 53a
Calculate [H3O+] and [OH–] for each solution at 25 °C. a. pH = 8.55
Problem 53b,c
Calculate [H3O+] and [OH–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87
Problem 55
Complete the table. (All solutions are at 25 °C.)
Problem 56
Complete the table. (All solutions are at 25 °C.)
Problem 57
Like all equilibrium constants, the value of Kw depends on temperature. At body temperature (37 °C), Kw = 2.4×10–14. What are the [H3O+] and pH of pure water at body temperature?
Problem 58
The value of Kw increases with increasing temperature. Is the autoionization of water endothermic or exothermic?
Problem 59
Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H3O+] = 0.044 M [H3O+] = 0.045 M [H3O+] = 0.046 M
Problem 60
Determine the concentration of H3O+ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52
Problem 61a
For each strong acid solution, determine [H3O+], [OH–], and pH. a. 0.25 M HCl
Problem 61b
For each strong acid solution, determine [H3O+], [OH–], and pH. b. 0.015 M HNO3
Problem 61c
For each strong acid solution, determine [H3O+], [OH–], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO3
Problem 61d
For each strong acid solution, determine [H3O+], [OH–], and pH. d. a solution that is 0.655% HNO3 by mass (assume a density of 1.01 g/mL for the solution)
Problem 63
What mass of HI must be present in 0.250 L of solution to obtain a solution with each pH value?
a. pH = 1.25 b. pH = 1.75 c. pH = 2.85
Problem 64
What mass of HClO4 must be present in 0.500 L of solution to obtain a solution with each pH value? a. pH = 2.50 b. pH = 1.50 c. pH = 0.50
Problem 65
What is the pH of a solution in which 121 mL of HCl(g), measured at and 0.855 atm, is dissolved in 1.5 L of aqueous solution?
Problem 67
Determine the [H3O+] and pH of a 0.200 M solution of benzoic acid.
Problem 68
Determine the [H3O+] and pH of a 0.100 M solution of formic acid.