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

Verified step by step guidance

1. Identify the components of the solutions: HCl is a strong acid and NaOH is a strong base.
2. Calculate the moles of HCl: \( \text{moles of HCl} = 0.10 \, M \times 0.050 \, L \).
3. Calculate the moles of NaOH: \( \text{moles of NaOH} = 0.150 \, M \times 0.035 \, L \).
4. Determine the limiting reactant by comparing the moles of HCl and NaOH.
5. Assess if there is an excess of either component after the reaction. A buffer forms if there is a weak acid or weak base and its conjugate present in significant amounts.

Key Concepts

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 are crucial in maintaining stable pH levels in various chemical and biological processes.

Strong Acids and Bases

Strong acids, like HCl, completely dissociate in water, releasing all their protons (H+), while strong bases, like NaOH, completely dissociate to produce hydroxide ions (OH-). The complete dissociation of these substances means they do not form a buffer solution when mixed, as they do not provide the weak acid/base pair necessary for buffering.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In the given scenario, mixing HCl and NaOH will lead to a neutralization reaction, resulting in the formation of water and sodium chloride (NaCl). This reaction will not create a buffer, as it consumes both the acid and base completely.