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

검증된 단계별 안내

Identify the components needed for a buffer solution: a weak base and its conjugate acid, or a weak acid and its conjugate base.

Recognize that NH3 (ammonia) is a weak base, and NaOH (sodium hydroxide) is a strong base.

Calculate the moles of NH3 using the formula: moles = concentration (M) \(\times\) volume (L).

Calculate the moles of NaOH using the formula: moles = concentration (M) \(\times\) volume (L).

Determine if the strong base (NaOH) will convert some of the weak base (NH3) into its conjugate acid (NH4+), and check if there is enough NH3 left to form a buffer.

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이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

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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 Bases and Conjugate Acids

Weak bases, like ammonia (NH3), partially ionize in solution to form hydroxide ions (OH-) and their conjugate acids. The presence of both the weak base and its conjugate acid in a solution is essential for buffer action. In this case, NH3 can act as a weak base, while NH4+ (ammonium ion) would be its conjugate acid.

pH and Hydroxide Ion Concentration

The pH of a solution is a measure of its acidity or basicity, determined by the concentration of hydrogen ions (H+). When mixing solutions, the resulting pH depends on the concentrations of acids and bases present. In this scenario, the addition of NaOH, a strong base, will affect the overall pH and the potential for buffer formation with NH3.

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