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

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

Calculate the moles of HCl: \( \text{moles of HCl} = 0.10 \, M \times 0.050 \, L \).

Calculate the moles of NaOH: \( \text{moles of NaOH} = 0.150 \, M \times 0.035 \, L \).

Determine the limiting reactant by comparing the moles of HCl and NaOH.

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.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

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 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.

Recommended video:

Guided course

05:56

Lewis Dot Structures: Neutral Compounds

Related Practice

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?

views

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

Textbook Question

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

Textbook Question

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

Textbook Question

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