Multiple Choice
Consider the titration of a 35.0 mL sample of 0.175 M HBr with 0.200 M KOH. Determine the initial pH of the HBr solution before any KOH is added.
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17. Acid and Base Equilibrium
pH of Strong Acids and Bases
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Rank the following 0.100 M aqueous solutions in order of increasing pH (lowest to highest): NaOH, CH3COOH, HNO3, HClO2, CH3NH2.
A
HNO3 < HClO2 < CH3COOH < CH3NH2 < NaOH
B
HClO2 < CH3COOH < CH3NH2 < HNO3 < NaOH
C
HClO2 < HNO3 < CH3COOH < NaOH < CH3NH2
D
HNO3 < CH3COOH < HClO2 < CH3NH2 < NaOH
Verified step by step guidance1
Identify the nature of each compound: NaOH is a strong base, CH3COOH is a weak acid, HNO3 is a strong acid, HClO2 is a weak acid, and CH3NH2 is a weak base.
Understand that strong acids and bases dissociate completely in water, while weak acids and bases do not. This affects the pH of the solution.
Rank the strong acids and bases first: HNO3 (strong acid) will have the lowest pH, and NaOH (strong base) will have the highest pH.
Compare the weak acids: HClO2 and CH3COOH. Use their acid dissociation constants (Ka) to determine their relative strengths. The acid with the higher Ka value is stronger and will have a lower pH.
Consider the weak base CH3NH2. It will have a higher pH than the weak acids but lower than the strong base NaOH. Arrange the solutions in order of increasing pH based on these observations.
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