Understanding Equilibrium and Partition: Simple Chemistry for Kids!

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Katie Rose

09/08/2022

Chemistry

Chemical Equilibrium

Subjects

Chemistry

Acids and Bases

PH and POH of Strong Acids and Bases

Understanding Equilibrium and Partition: Simple Chemistry for Kids!

Understanding chemical equilibrium, partition coefficients, and pH relationships is crucial in chemistry. This comprehensive guide covers key concepts including equilibrium constant Kc, partition coefficients, and the relationship between pH and hydrogen ion concentration.

The K constant Chemistry characterizes reaction equilibrium composition and indicates equilibrium position
Partition coefficients determine solute distribution between immiscible liquids
pH and hydrogen ion concentration have an inverse logarithmic relationship
Buffer solutions maintain stable pH despite small acid/base additions
Indicators change color based on pH, making them useful for titrations

09/08/2022

2a) Chemical Equilibrium
Equilibrium
A chemical reaction is in equilibrium when the composition of the reactants and
products remains consta

Partition Coefficients and Solvent Extraction

This page covers partition coefficients and their application in solvent extraction, an important purification technique in chemistry.

The partition coefficient describes how a solute distributes between two immiscible liquids. It is temperature-dependent but unaffected by adding more solvent or solute.

Example: The partition coefficient formula for sodium chloride between water and hexane is: K = $salt(hexane)$ / $salt(aq)$

Solvent extraction, a common application of partition coefficients, is used for purifying chemicals.

Highlight: It is more efficient to use small volumes of organic solvent in repeated extractions rather than one large volume in a single extraction.

The section also introduces acids and bases, explaining that hydrogen ions $H+$ form hydronium ions $H3O+$ in water. Water's amphoteric nature and its ionic product $Kw$ are discussed.

Vocabulary: Amphoteric substances can behave as both acids and bases.

View

pH and Hydrogen Ion Concentration

This section explores the relationship between pH and hydrogen ion concentration in water. It provides key formulas and definitions related to acids and bases.

Definition: pH = -log10 $H3O+$ and $H3O+$ = 10^-pH

These formulas show the inverse logarithmic relationship between pH and hydrogen ion concentration. In neutral water at 25°C, both $H3O+$ and $OH-$ are 10^-7 mol/L.

The Brønsted-Lowry definition of acids and bases is introduced:

Acids are proton donors
Bases are proton acceptors

Vocabulary: Conjugate base is the species left when an acid donates a proton. Conjugate acid is formed when a base accepts a proton.

The text distinguishes between strong and weak acids/bases:

Strong acids/bases fully dissociate in water $e.g., HCl, NaOH$
Weak acids/bases partially dissociate in water $e.g., ethanoic acid, ammonia$

A table compares properties of strong and weak acids/bases, including pH values, conductivity, and reaction rates.

View

Acid Dissociation Constants and Salt Solutions

This page delves deeper into weak acids and bases, introducing the concept of acid dissociation constants $Ka$ and their relationship to pH.

Definition: Ka is the equilibrium constant for the dissociation of a weak acid in water.

The Ka value measures the strength of a weak acid. A smaller Ka indicates a weaker acid. The pKa, defined as the negative logarithm of Ka, is often used in calculations.

Highlight: pH = pKa - log C $where C is the concentration of the weak acid$

The formation of salts from acid-base reactions is discussed. The pH of salt solutions depends on the strength of the parent acid and base:

Strong acid + strong base = neutral solution
Weak acid + strong base = alkaline solution
Strong acid + weak base = acidic solution

Example: NaCl $from HCl + NaOH$ produces a neutral solution, while CH3COONa $from CH3COOH + NaOH$ produces an alkaline solution.

This information helps in understanding the behavior of various salt solutions and their applications in chemistry and related fields.

View

Acid Dissociation Constants and pH Calculations

This section covers the mathematical relationships between acid strength, dissociation constants, and pH calculations.

Definition: Ka $acid dissociation constant$ measures the strength of weak acids.

Highlight: The pKa value converts Ka into a more manageable whole number for calculations.

Example: The relationship between pH and Ka is expressed as pH = pKa - logC

View

Buffer Solutions

This section explains buffer solution behavior and mechanisms.

Definition: Buffer solutions resist pH changes when small amounts of acid or base are added.

Example: In ethanoic acid buffers, adding alkali causes OH- ions to react with H+ ions while more acid dissociates to maintain equilibrium.

Highlight: Basic buffers work similarly but with weak bases and their conjugate acids.

View

Indicators and Equilibrium

This section covers indicator behavior and equilibrium constants.

Definition: The indicator equilibrium constant $KIn$ relates colored form concentrations to H+ concentration.

Example: KIn = $H+$ $In-$ / $HIn$ shows how indicator color depends on pH.

Highlight: Color change occurs theoretically when $HIn$ = $In-$ .

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Subjects

Chemistry

Acids and Bases

PH and POH of Strong Acids and Bases

Chemistry

•

361

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9 Aug 2022

•

7 pages

Understanding Equilibrium and Partition: Simple Chemistry for Kids!

Katie Rose

@katierose

The K constant Chemistrycharacterizes reaction... Show more

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Partition Coefficients and Solvent Extraction

This page covers partition coefficients and their application in solvent extraction, an important purification technique in chemistry.

The partition coefficient describes how a solute distributes between two immiscible liquids. It is temperature-dependent but unaffected by adding more solvent or solute.

Example: The partition coefficient formula for sodium chloride between water and hexane is: K = $salt(hexane)$ / $salt(aq)$

Solvent extraction, a common application of partition coefficients, is used for purifying chemicals.

Highlight: It is more efficient to use small volumes of organic solvent in repeated extractions rather than one large volume in a single extraction.

The section also introduces acids and bases, explaining that hydrogen ions $H+$ form hydronium ions $H3O+$ in water. Water's amphoteric nature and its ionic product $Kw$ are discussed.

Vocabulary: Amphoteric substances can behave as both acids and bases.

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pH and Hydrogen Ion Concentration

This section explores the relationship between pH and hydrogen ion concentration in water. It provides key formulas and definitions related to acids and bases.

Definition: pH = -log10 $H3O+$ and $H3O+$ = 10^-pH

These formulas show the inverse logarithmic relationship between pH and hydrogen ion concentration. In neutral water at 25°C, both $H3O+$ and $OH-$ are 10^-7 mol/L.

The Brønsted-Lowry definition of acids and bases is introduced:

Acids are proton donors
Bases are proton acceptors

Vocabulary: Conjugate base is the species left when an acid donates a proton. Conjugate acid is formed when a base accepts a proton.

The text distinguishes between strong and weak acids/bases:

Strong acids/bases fully dissociate in water $e.g., HCl, NaOH$
Weak acids/bases partially dissociate in water $e.g., ethanoic acid, ammonia$

A table compares properties of strong and weak acids/bases, including pH values, conductivity, and reaction rates.

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Acid Dissociation Constants and Salt Solutions

This page delves deeper into weak acids and bases, introducing the concept of acid dissociation constants $Ka$ and their relationship to pH.

Definition: Ka is the equilibrium constant for the dissociation of a weak acid in water.

The Ka value measures the strength of a weak acid. A smaller Ka indicates a weaker acid. The pKa, defined as the negative logarithm of Ka, is often used in calculations.

Highlight: pH = pKa - log C $where C is the concentration of the weak acid$

The formation of salts from acid-base reactions is discussed. The pH of salt solutions depends on the strength of the parent acid and base:

Strong acid + strong base = neutral solution
Weak acid + strong base = alkaline solution
Strong acid + weak base = acidic solution

Example: NaCl $from HCl + NaOH$ produces a neutral solution, while CH3COONa $from CH3COOH + NaOH$ produces an alkaline solution.

This information helps in understanding the behavior of various salt solutions and their applications in chemistry and related fields.

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Acid Dissociation Constants and pH Calculations

This section covers the mathematical relationships between acid strength, dissociation constants, and pH calculations.

Definition: Ka $acid dissociation constant$ measures the strength of weak acids.

Highlight: The pKa value converts Ka into a more manageable whole number for calculations.

Example: The relationship between pH and Ka is expressed as pH = pKa - logC

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Buffer Solutions

This section explains buffer solution behavior and mechanisms.

Definition: Buffer solutions resist pH changes when small amounts of acid or base are added.

Example: In ethanoic acid buffers, adding alkali causes OH- ions to react with H+ ions while more acid dissociates to maintain equilibrium.

Highlight: Basic buffers work similarly but with weak bases and their conjugate acids.

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Indicators and Equilibrium

This section covers indicator behavior and equilibrium constants.

Definition: The indicator equilibrium constant $KIn$ relates colored form concentrations to H+ concentration.

Example: KIn = $H+$ $In-$ / $HIn$ shows how indicator color depends on pH.

Highlight: Color change occurs theoretically when $HIn$ = $In-$ .

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Chemical Equilibrium and Equilibrium Constants

This section introduces the concept of chemical equilibrium and the equilibrium constant Kc. It explains how to interpret and calculate equilibrium constants.

Definition: Chemical equilibrium occurs when the composition of reactants and products remains constant indefinitely.

The equilibrium constant K characterizes the equilibrium composition of a reaction mixture. It is calculated as the ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients.

Vocabulary: Homogeneous equilibrium involves all species in the same state, while heterogeneous equilibrium involves species in different states.

The value of K indicates the position of equilibrium:

K > 1: Equilibrium favors products
K = 1: Equilibrium is balanced
K < 1: Equilibrium favors reactants

Temperature affects K for endothermic and exothermic reactions differently. Catalysts do not affect the equilibrium constant value.

Highlight: The equilibrium constant K is temperature-dependent but not affected by concentration or pressure changes.

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Understanding Equilibrium and Partition: Simple Chemistry for Kids!

Partition Coefficients and Solvent Extraction

pH and Hydrogen Ion Concentration

Acid Dissociation Constants and Salt Solutions

Acid Dissociation Constants and pH Calculations

Buffer Solutions

Indicators and Equilibrium

Similar content

Can't find what you're looking for? Explore other subjects.

Knowunity is the #1 education app in five European countries

Knowunity has been named a featured story on Apple and has regularly topped the app store charts in the education category in Germany, Italy, Poland, Switzerland, and the United Kingdom. Join Knowunity today and help millions of students around the world.

4.9+

21 M

#1

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Still not convinced? See what other students are saying...

I love this app so much, I also use it daily. I recommend Knowunity to everyone!!! I went from a D to an A with it :D

The app is very simple and well designed. So far I have always found everything I was looking for :D

I love this app ❤️ I actually use it every time I study.

Understanding Equilibrium and Partition: Simple Chemistry for Kids!

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Partition Coefficients and Solvent Extraction

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pH and Hydrogen Ion Concentration

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Acid Dissociation Constants and Salt Solutions

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Acid Dissociation Constants and pH Calculations

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Buffer Solutions

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Indicators and Equilibrium

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Chemical Equilibrium and Equilibrium Constants

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