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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.
Problem 69
Determine the pH of an HNO2 solution of each concentration. In which cases can you not make the simplifying assumption that x is small? a. 0.500 M b. 0.100 M c. 0.0100 M
Problem 70
Determine the pH of an HF solution of each concentration. In which cases can you not make the simplifying assumption that x is small? (Ka for HF is 6.8×10–4.) a. 0.250 M b. 0.0500 M c. 0.0250 M
Problem 73
A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka) for the acid.
Problem 75
Determine the percent ionization of a 0.100 M HCN solution.
Problem 76
Determine the percent ionization of a 0.250 M solution of benzoic acid.
- What is the percent ionization of an acetic acid solution at the following concentrations? a. 1.00 M b. 0.500 M c. 0.100 M d. 0.0500 M
Problem 77
Problem 78a
Calculate the percent ionization of a formic acid solution having the given concentration. a. 1.00 M
Problem 78b
Calculate the percent ionization of a formic acid solution having the given concentration. b. 0.500 M
Problem 78c
Calculate the percent ionization of a formic acid solution having the given concentration. c. 0.100 M
Problem 78d
Calculate the percent ionization of a formic acid solution having the given concentration. d. 0.0500 M
Problem 79
A 0.148 M solution of a monoprotic acid has a percent ionization of 1.55%. Determine the acid ionization constant (Ka) for the acid.
- Find the pH and percent ionization of each HF solution. (Ka for HF is 6.8 * 10^-4.) a. 0.250 M HF b. 0.100 M HF c. 0.050 M HF.
Problem 81
- Find the pH and percent ionization of a 0.100 M solution of a weak monoprotic acid given the following Ka values: a. Ka = 1.0 * 10^-5, b. Ka = 1.0 * 10^-3, c. Ka = 1.0 * 10^-1.
Problem 82
Problem 83a
Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO2