Determine whether or not the mixing of each pair of solutions results in a buffer. c. 50.0 mL of 0.15 M HF; 20.0 mL of 0.15 M NaOH

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Identify the components of the solutions: HF is a weak acid and NaOH is a strong base.

Calculate the moles of HF using the formula: moles = concentration \( \times \) volume. For HF, use 0.15 M and 50.0 mL.

Calculate the moles of NaOH using the formula: moles = concentration \( \times \) volume. For NaOH, use 0.15 M and 20.0 mL.

Determine the limiting reactant by comparing the moles of HF and NaOH. The limiting reactant will be completely consumed in the reaction.

Check if the remaining solution contains a weak acid and its conjugate base. If so, the solution is a buffer.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Buffer Solutions

A buffer solution is a system that resists changes in pH upon the addition of small amounts of acid or base. It typically consists of a weak acid and its conjugate base or a weak base and its conjugate acid. Buffers maintain pH stability, which is crucial in many chemical and biological processes.

Weak Acids and Bases

Weak acids, like hydrofluoric acid (HF), do not completely dissociate in solution, meaning they establish an equilibrium between the undissociated acid and its ions. In contrast, strong bases, such as sodium hydroxide (NaOH), fully dissociate in solution. The interaction between weak acids and strong bases is essential for buffer formation.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In the context of the given question, the reaction between HF and NaOH will lead to the formation of water and sodium fluoride (NaF). This reaction is critical in determining whether the resulting solution can act as a buffer.

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Textbook Question

A 100.0-mL buffer solution is 0.100 M in NH₃ and 0.125 M in NH₄Br. What mass of HCl can this buffer neutralize before the pH falls below 9.00?

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Textbook Question

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 100.0 mL of 0.10 M NH₃; 100.0 mL of 0.15 M NH₄Cl

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Determine whether or not the mixing of each pair of solutions results in a buffer. b. 50.0 mL of 0.10 M HCl; 35.0 mL of 0.150 M NaOH

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Determine whether or not the mixing of each pair of solutions results in a buffer. d. 175.0 mL of 0.10 M NH₃; 150.0 mL of 0.12 M NaOH

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Determine whether or not the mixing of each pair of solutions results in a buffer. e. 125.0 mL of 0.15 M NH₃; 150.0 mL of 0.20 M NaOH

Textbook Question

Determine whether or not the mixing of each pair of solutions results in a buffer. a. 75.0 mL of 0.10 M HF; 55.0 mL of 0.15 M NaF b. 150.0 mL of 0.10 M HF; 135.0 mL of 0.175 M HCl d. 125.0 mL of 0.15 M CH₃NH₂; 120.0 mL of 0.25 M CH₃NH₃Cl