Multiple Choice
An aqueous solution of HBrO4 has a pH of 4.34. Find the molar concentration of HBrO4 solution.
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10. Acids and Bases
pH of Strong Acids and Bases
Multiple Choice
HI 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
B
[H+] = 7.1 × 10−2 M
[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
D
[H+] = 7.1 × 10−2 M
[OH−] = 7.1 × 10−12 M
pH = 1.15
pOH = 11.15
Verified step by step guidance1
Identify that HI is a strong acid, which means it completely dissociates in water. Therefore, the concentration of H+ ions is equal to the initial concentration of HI, which is 7.1 × 10^{-2} M.
Use the relationship between [H+] and [OH-] in water at 25°C, which is given by the ion product of water: Kw = [H+][OH-] = 1.0 × 10^{-14}. Substitute [H+] = 7.1 × 10^{-2} M into this equation to solve for [OH-].
Calculate the pH of the solution using the formula pH = -log[H+]. Substitute the value of [H+] = 7.1 × 10^{-2} M into this formula to find the pH.
Calculate the pOH of the solution using the relationship pOH = 14 - pH. Use the pH value obtained in the previous step to find the pOH.
Verify the consistency of your results by checking that the sum of pH and pOH equals 14, which is a characteristic of aqueous solutions at 25°C.
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