교과서 질문
Like all equilibrium constants, the value of Kw depends on temperature. At body temperature (37 °C), Kw = 2.4×10–14. What are the [H3O+] and pH of pure water at body temperature?
4275
views
10
rank
Ch.17 - Acids and Bases
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371
당신이 사용하는 게 아니라요?교과서 변경다른 교과서를 선택하세요
TOC.tableOfContents
- Ch.1 - Matter, Measurement & Problem Solving117
- Ch.2 - Atoms & Elements106
- Ch.3 - Molecules and Compounds128
- Ch.4 - Chemical Reactions and Chemical Quantities56
- Ch.5 - Introduction to Solutions and Aqueous Solutions84
- Ch.6 - Gases112
- Ch.7 - Thermochemistry96
- Ch.8 - The Quantum-Mechanical Model of the Atom60
- Ch.9 - Periodic Properties of the Elements86
- Ch.10 - Chemical Bonding I: The Lewis Model91
- Ch.11 - Chemical Bonding II: Molecular Shapes, VSEPR & MO Theory85
- Ch.12 - Liquids, Solids & Intermolecular Forces51
- Ch.13 - Solids & Modern Materials48
- Ch.14 - Solutions93
- Ch.15 - Chemical Kinetics114
- Ch.16 - Chemical Equilibrium68
- Ch.17 - Acids and Bases137
- Ch.18 - Aqueous Ionic Equilibrium154
- Ch.19 - Free Energy & Thermodynamics91
- Ch.20 - Electrochemistry105
- Ch.21 - Radioactivity & Nuclear Chemistry74
- Ch.22 - Organic Chemistry141
17장, 문제 50b,c
Calculate [H3O+] and [OH–] for each solution at 25 °C. b. pH = 11.23 c. pH = 2.87
검증된 단계별 안내1
Start by recalling the relationship between pH and [H3O+]: \( \text{pH} = -\log[\text{H}_3\text{O}^+] \).
Rearrange the equation to solve for [H3O+]: \( [\text{H}_3\text{O}^+] = 10^{-\text{pH}} \).
Substitute the given pH value into the equation to find [H3O+].
Use the water dissociation constant at 25 °C, \( K_w = 1.0 \times 10^{-14} \), to find [OH-] using the relationship \( [\text{H}_3\text{O}^+] \times [\text{OH}^-] = K_w \).
Rearrange the equation to solve for [OH-]: \( [\text{OH}^-] = \frac{K_w}{[\text{H}_3\text{O}^+]} \) and substitute the value of [H3O+] to find [OH-].
비슷한 문제에 대한 검증된 영상 답변:
이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.
영상 길이:
1m도움이 되었나요?
주요 개념
질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.
pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is considered neutral, while values below 7 indicate acidity and values above 7 indicate basicity. The pH is defined as the negative logarithm of the hydrogen ion concentration, [H+], in a solution, which is crucial for determining the concentration of hydronium ions, [H3O+].
추천 영상:
가이드 코스
02:33
The pH Scale
Ion Product of Water (Kw)
The ion product of water, Kw, is the equilibrium constant for the self-ionization of water, defined as Kw = [H3O+][OH-] = 1.0 x 10^-14 at 25 °C. This relationship allows us to calculate the concentration of hydroxide ions, [OH-], when the concentration of hydronium ions, [H3O+], is known, and vice versa. Understanding Kw is essential for solving problems involving pH and pOH.
추천 영상:
가이드 코스
00:53Production of Hydrogen Example
Hydronium and Hydroxide Ion Concentrations
In aqueous solutions, the concentrations of hydronium ions, [H3O+], and hydroxide ions, [OH-], are inversely related due to the ion product of water. For a basic solution, like one with a pH of 11.23, [H3O+] will be lower than 1.0 x 10^-7 M, while [OH-] will be higher than 1.0 x 10^-7 M. Calculating these concentrations is essential for understanding the solution's properties and behavior.
추천 영상:
가이드 코스
06:25Hydronium Ion Concentration Example