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Ch.17 - Aqueous Ionic Equilibrium
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.17 - Aqueous Ionic Equilibrium문제 42
17장, 문제 42

Calculate the pH of the solution that results from each mixture. a. 150.0 mL of 0.25 M HF with 225.0 mL of 0.30 M NaF b. 175.0 mL of 0.10 M C2H5NH2 with 275.0 mL of 0.20 M C2H5NH3Cl

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Identify the type of solution formed in each case. For part (a), mixing HF and NaF forms a buffer solution of a weak acid (HF) and its conjugate base (F⁻). For part (b), mixing C₂H₅NH₂ and C₂H₅NH₃Cl forms a buffer solution of a weak base (C₂H₅NH₂) and its conjugate acid (C₂H₅NH₃⁺).
Use the Henderson-Hasselbalch equation to calculate the pH of the buffer solutions. For part (a), use the equation: pH = pKa + log([A⁻]/[HA]), where [A⁻] is the concentration of F⁻ and [HA] is the concentration of HF. For part (b), use the equation: pH = pKa + log([B]/[BH⁺]), where [B] is the concentration of C₂H₅NH₂ and [BH⁺] is the concentration of C₂H₅NH₃⁺.
Calculate the moles of each component in the mixtures. For part (a), moles of HF = 0.25 M * 0.150 L and moles of NaF = 0.30 M * 0.225 L. For part (b), moles of C₂H₅NH₂ = 0.10 M * 0.175 L and moles of C₂H₅NH₃Cl = 0.20 M * 0.275 L.
Determine the concentrations of each component in the final solution by dividing the moles by the total volume of the mixture. For part (a), total volume = 150.0 mL + 225.0 mL. For part (b), total volume = 175.0 mL + 275.0 mL.
Substitute the concentrations into the Henderson-Hasselbalch equation to find the pH of each buffer solution.

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주요 개념

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

Buffer Solutions

Buffer solutions are mixtures of a weak acid and its conjugate base or a weak base and its conjugate acid. They resist changes in pH when small amounts of acid or base are added. In the given question, the mixtures of HF and NaF, as well as C2H5NH2 and C2H5NH3Cl, form buffer systems that can be analyzed using the Henderson-Hasselbalch equation.
추천 영상:
가이드 코스
03:02
Buffer Solutions

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of buffer solutions. It is expressed as pH = pKa + log([A-]/[HA]), where pKa is the negative logarithm of the acid dissociation constant, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the weak acid. This equation is essential for determining the pH of the mixtures in the question.
추천 영상:
가이드 코스
02:40
Henderson-Hasselbalch Equation

Dilution and Concentration Calculations

Dilution involves reducing the concentration of a solute in a solution, typically by adding more solvent. The total volume and concentrations of the components in the mixtures must be calculated to determine the final concentrations of the acid and base in the buffer solutions. Understanding dilution principles is crucial for accurately calculating the pH of the resulting solutions.
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가이드 코스
02:36
Dilution Calculation Example
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