미해결 질문
Find the pH of each mixture of acids. a. 0.075 M in HNO3 and 0.175 M in HC7H5O2 b. 0.020 M in HBr and 0.015 M in HClO4 c. 0.095 M in HF and 0.225 M in HC6H5O d. 0.100 M in formic acid and 0.050 M in hypochlorous acid
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17. Acid and Base Equilibrium
pH of Weak Acids
Multiple Choice
A particular sample of vinegar has a pH of 2.90. If acetic acid is the only acid that vinegar contains, what is the concentration of acetic acid in the vinegar?
A
0.001 M
B
0.01 M
C
0.005 M
D
0.02 M
검증된 단계별 안내1
Understand that pH is a measure of the hydrogen ion concentration in a solution. The pH is given by the formula: \( \text{pH} = -\log[H^+] \).
Given the pH of the vinegar is 2.90, use the formula to find the concentration of hydrogen ions \([H^+]\). Rearrange the formula to solve for \([H^+]\): \([H^+] = 10^{-\text{pH}}\).
Substitute the given pH value into the equation: \([H^+] = 10^{-2.90}\). This will give you the concentration of hydrogen ions in the solution.
Recognize that acetic acid (CH₃COOH) is a weak acid and partially dissociates in water. The dissociation can be represented as: \( \text{CH}_3\text{COOH} \rightleftharpoons \text{CH}_3\text{COO}^- + \text{H}^+ \).
Assume that the concentration of \([H^+]\) is approximately equal to the initial concentration of acetic acid due to its weak dissociation. Compare the calculated \([H^+]\) with the given options to determine the concentration of acetic acid.
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