1) A solution of perchloric acid is prepared that has a molar concentration equal to the fourth and fifth digits of your Student ID Number divided by 105. What is the pH and pOH of that solution at 25 °C?
2) A solution of nitric acid is prepared that has a molar concentration equal to the fourth and fifth digits of your Student ID Number divided by 104. What is the pH and pOH of that solution at 25 °C?
3) A solution of potassium hydroxide is prepared that has a molar concentration equal to the fourth and fifth digits of your Student ID Number divided by 103. What is the pH and pOH of that solution at 25 °C?
4) A solution of barium hydroxide is prepared that has a molar concentration equal to the fourth and fifth digits of your Student ID Number divided by 105. What is the pH and pOH of that solution at 25 °C? Assume complete solubility and complete ionization.
1) For perchloric acid:
HClO4(aq) + H2O(l) → H3O+(aq) + ClO4–(aq)
So the [H3O+] = [HClO4] = ID/105 M
pH = –log[H3O+]
pOH = 14.00 – pH (at 25 °C)
2) For nitric acid:
HNO3(aq) + H2O(l) → H3O+(aq) + NO3–(aq)
So the [H3O+] = [HNO3] = ID/104 M
pH = –log[H3O+]
pOH = 14.00 – pH (at 25 °C)
3) For potassium hydroxide:
KOH(aq) → K+(aq) + OH–(aq)
So [OH–] = [KOH] = ID/103 M
pOH = –log[OH–]
pH = 14.00 – pOH (at 25 °C)
4) For barium hydroxide:
Ba(OH)2(aq) → Ba2+(aq) + 2 OH–(aq)
So [OH–] = 2×[Ba(OH)2] = 2×ID/105 M
pOH = –log[OH–]
pH = 14.00 – pOH (at 25 °C)
Since all concentrations are given to 2 significant figures, all pH and pOH values are found to 2 places past the decimal.
Specific answers:
Question 1 | Question 2 | Question 3 | Question 4 | ||||||||
[HClO4] (M) | pH | pOH | [HNO3] (M) | pH | pOH | [KOH] (M) | pH | pOH | [Ba(OH)2] (M) | pH | pOH |
0.00050 | 3.30 | 10.70 | 0.0050 | 2.30 | 11.70 | 0.050 | 12.70 | 1.30 | 0.00050 | 11.00 | 3.00 |
0.00052 | 3.28 | 10.72 | 0.0052 | 2.28 | 11.72 | 0.052 | 12.72 | 1.28 | 0.00052 | 11.02 | 2.98 |
0.00054 | 3.27 | 10.73 | 0.0054 | 2.27 | 11.73 | 0.054 | 12.73 | 1.27 | 0.00054 | 11.03 | 2.97 |
0.00055 | 3.26 | 10.74 | 0.0055 | 2.26 | 11.74 | 0.055 | 12.74 | 1.26 | 0.00055 | 11.04 | 2.96 |
0.00056 | 3.25 | 10.75 | 0.0056 | 2.25 | 11.75 | 0.056 | 12.75 | 1.25 | 0.00056 | 11.05 | 2.95 |
0.00057 | 3.24 | 10.76 | 0.0057 | 2.24 | 11.76 | 0.057 | 12.76 | 1.24 | 0.00057 | 11.06 | 2.94 |
0.00058 | 3.24 | 10.76 | 0.0058 | 2.24 | 11.76 | 0.058 | 12.76 | 1.24 | 0.00058 | 11.06 | 2.94 |
0.00059 | 3.23 | 10.77 | 0.0059 | 2.23 | 11.77 | 0.059 | 12.77 | 1.23 | 0.00059 | 11.07 | 2.93 |
0.00060 | 3.22 | 10.78 | 0.0060 | 2.22 | 11.78 | 0.060 | 12.78 | 1.22 | 0.00060 | 11.08 | 2.92 |
0.00061 | 3.21 | 10.79 | 0.0061 | 2.21 | 11.79 | 0.061 | 12.79 | 1.21 | 0.00061 | 11.09 | 2.91 |
0.00062 | 3.21 | 10.79 | 0.0062 | 2.21 | 11.79 | 0.062 | 12.79 | 1.21 | 0.00062 | 11.09 | 2.91 |
0.00063 | 3.20 | 10.80 | 0.0063 | 2.20 | 11.80 | 0.063 | 12.80 | 1.20 | 0.00063 | 11.10 | 2.90 |