17. Acid and Base Equilibrium
pH of Strong Acids and Bases
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
1
concept
Strong Acids and Bases
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example
pH of Strong Acids and Bases Example
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3
Problem
ProblemAn aqueous solution of HBrO4 has a pH of 4.34. Find the molar concentration of HBrO4 solution.
A
4.6 × 10−19 M
B
2.6 × 10−6 M
C
2.2 × 10−10 M
D
4.6 × 10−5 M
4
Problem
ProblemCalculate the pH of a 25 mL of 5.45 × 10−2 M LiOH solution.
A
1.264
B
12.736
C
0.338
D
11.134
5
Problem
ProblemHI is a strong acid (Ka = 3.2 × 109). Calculate [H+], [OH−], pH and pOH of a 7.1 × 10−2 M HI solution.
A
[H+] = 7.1 × 10−2 M
[OH−] = 1.4 × 10−13 M
pH = 1.15
pOH = 12.85
[OH−] = 1.4 × 10−13 M
pH = 1.15
pOH = 12.85
B
[H+] = 7.1 × 10−2 M
[OH−] = 1.4 × 10−13 M
pH = 8.50
pOH = 5.50
[OH−] = 1.4 × 10−13 M
pH = 8.50
pOH = 5.50
C
[H+] = 7.1 × 10−2 M
[OH−] = 7.1 × 10−16 M
pH = 1.15
pOH = 15.15
[OH−] = 7.1 × 10−16 M
pH = 1.15
pOH = 15.15
D
[H+] = 7.1 × 10−2 M
[OH−] = 7.1 × 10−12 M
pH = 1.15
pOH = 11.15
[OH−] = 7.1 × 10−12 M
pH = 1.15
pOH = 11.15