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Ch.18 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 5th EditionCh.18 - Aqueous Ionic Equilibrium문제 54b
18장, 문제 54b

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

검증된 단계별 안내
1
Identify the components needed for a buffer solution: a weak acid and its conjugate base, or a weak base and its conjugate acid.
Recognize that HF is a weak acid, which is a potential component of a buffer solution.
Note that HCl is a strong acid, which will completely dissociate in solution and does not form a buffer with HF.
Calculate the moles of HF: \( \text{moles of HF} = 0.150 \text{ L} \times 0.10 \text{ M} \).
Calculate the moles of HCl: \( \text{moles of HCl} = 0.135 \text{ L} \times 0.175 \text{ M} \).

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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.
추천 영상:
가이드 코스
03:02
Buffer Solutions

Weak Acids and Strong Acids

Weak acids, like HF (hydrofluoric acid), partially dissociate in solution, establishing an equilibrium between the undissociated acid and its ions. In contrast, strong acids, such as HCl (hydrochloric acid), completely dissociate in solution. The presence of a strong acid can disrupt the equilibrium of a weak acid, affecting the buffer capacity.
추천 영상:
가이드 코스
01:15
Calculating Percent Ionization of Weak Acids

pH and Acid-Base Reactions

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. Acid-base reactions involve the transfer of protons (H+) between species, influencing the pH. Understanding how the mixing of different acids affects the overall pH is essential for determining whether a buffer is formed.
추천 영상:
가이드 코스
02:39
pH of Strong Acids and Bases
관련 실천
교과서 질문

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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교과서 질문

Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3- and 0.0012 M H2CO3 (pKa1 for H2CO3 at body temperature is 6.1).

c. Given the volume from part (b), what mass of NaOH can be neutralized before the pH rises above 7.8?

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교과서 질문

Determine whether or not the mixing of each pair of solutions results in a buffer. c. 165.0 mL of 0.10 M HF; 135.0 mL of 0.050 M KOH

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Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3- and 0.0012 M H2CO3 (pKa1 for H2CO3 at body temperature is 6.1).

a. What is the pH of blood plasma?

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교과서 질문

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

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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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