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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 29b
18장, 문제 29b

Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution. b. a solution that is 0.16 M in NH3 and 0.22 M in NH4Cl

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1
Identify the equilibrium reaction: NH3 + H2O ⇌ NH4+ + OH−.
Write the expression for the base dissociation constant (Kb) for NH3: Kb = [NH4+][OH−] / [NH3].
Set up an ICE table (Initial, Change, Equilibrium) for the concentrations of NH3, NH4+, and OH−.
Use the initial concentrations: [NH3] = 0.16 M, [NH4+] = 0.22 M, and [OH−] = 0 M. Assume x is the change in concentration for NH4+ and OH−.
Substitute the equilibrium concentrations into the Kb expression and solve for x, which represents [OH−]. Then, calculate pOH and use it to find the pH.

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주요 개념

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

Equilibrium and ICE Tables

Equilibrium in chemistry refers to the state where the concentrations of reactants and products remain constant over time. An ICE table (Initial, Change, Equilibrium) is a tool used to organize the concentrations of species involved in a reaction at different stages. It helps in calculating the changes in concentration as the system reaches equilibrium, which is essential for solving equilibrium problems.
추천 영상:
가이드 코스
01:14
ICE Charts and Equilibrium Amount

Weak Bases and Conjugate Acids

Ammonia (NH3) is a weak base that partially ionizes in water to form hydroxide ions (OH-) and ammonium ions (NH4+). The presence of NH4Cl provides the conjugate acid (NH4+) of the weak base, which influences the pH of the solution. Understanding the relationship between weak bases and their conjugate acids is crucial for calculating the pH in buffer solutions.
추천 영상:
가이드 코스
01:46
Conjugate Acid-Base Relationships

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical formula used to calculate the pH of buffer solutions. It relates the pH of a solution to the pKa of the weak acid and the ratio of the concentrations of the conjugate base and acid. In this case, it can be applied to find the pH of the solution containing NH3 and NH4Cl, providing a quick way to determine the pH without extensive calculations.
추천 영상:
가이드 코스
02:40
Henderson-Hasselbalch Equation
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