Determine whether or not the mixing of each pair of solutions results in a buffer. b. 125.0 mL of 0.14 M HF; 195.0 mL of 0.070 M NaOH

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

Calculate the moles of HF using the formula: \( \text{moles of HF} = \text{volume (L)} \times \text{molarity (M)} \).

Calculate the moles of NaOH using the formula: \( \text{moles of NaOH} = \text{volume (L)} \times \text{molarity (M)} \).

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 in significant amounts to form a buffer.

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주요 개념

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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 HF (hydrofluoric acid), partially dissociate in solution, establishing an equilibrium between the undissociated acid and its ions. In contrast, strong bases, such as NaOH (sodium hydroxide), fully dissociate in solution. Understanding the behavior of weak acids and bases is essential for predicting the outcome of their interactions.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this context, the reaction between HF and NaOH will determine if a buffer is formed. The stoichiometry of the reactants is crucial to assess whether the resulting solution can maintain a stable pH.