Multiple Choice
A buffer solution is comprised of 50.0 mL of a 0.100 M HC2H3O2 and 60.0 mL of a 0.100 M NaC2H3O2. Which of the following actions would completely destroy the buffer?
14. Acids and Bases
Buffers
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Which of the following combinations can result in the formation of a buffer?
A
50 mL of 0.10 M HF with 50 mL of 0.10 M NaOH.
B
50 mL of 0.10 M HNO2 with 25mL of 0.10 M Ca(OH)2
C
50 mL of 0.10 M CH3CO2H with 60 mL of 0.10 M NaOH
D
50 mL of 0.10 M HF with 30 mL of 0.10 M NaOH.
Verified step by step guidance1
Understand what a buffer solution is: A buffer solution resists changes in pH when small amounts of acid or base are added. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid.
Identify the components needed for a buffer: In this problem, we are looking for a combination that results in a weak acid and its conjugate base. Hydrofluoric acid (HF) is a weak acid, and its conjugate base is fluoride ion (F⁻).
Analyze the first combination: 50 mL of 0.10 M HF with 50 mL of 0.10 M NaOH. Calculate the moles of HF and NaOH. Since NaOH is a strong base, it will react with HF to form water and fluoride ions, potentially creating a buffer if the amounts are appropriate.
Consider the stoichiometry: The reaction between HF and NaOH is HF + NaOH → NaF + H₂O. Calculate the moles of HF and NaOH to determine if NaOH is enough to convert some HF to its conjugate base (F⁻) without completely neutralizing it.
Evaluate the correct answer: 50 mL of 0.10 M HF with 30 mL of 0.10 M NaOH. Calculate the moles of HF and NaOH in this combination. Ensure that NaOH is partially neutralizing HF to form a buffer consisting of HF and F⁻, without completely neutralizing the HF.
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