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Fun with Chemistry: Understanding Acids and Bases!

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gracie keenan

01/04/2023

Chemistry

CCEA ALEVEL CHEMISTRY ACID-BASE

Fun with Chemistry: Understanding Acids and Bases!

Understanding acid-base equilibria in chemistry is fundamental to grasping how acids and bases interact, including the significance of Ka in acid dissociation and methods for calculating pH of strong and weak acids.

  • Brønsted-Lowry theory defines acids as proton donors and bases as proton acceptors
  • Water plays a crucial role in acid-base reactions, forming hydronium ions (H₃O⁺)
  • Buffer solutions maintain stable pH levels through weak acid and conjugate base interactions
  • Ka values determine acid strength and dissociation extent
  • Blood pH regulation through buffer systems demonstrates real-world applications
...

01/04/2023

252

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

View

Page 2: Acid Strength and Dissociation Constants

This page delves deeper into the differences between strong and weak acids, introducing Ka aciddissociationconstantacid dissociation constant and its relationship to acid strength. The content explains how to calculate pH using equilibrium equations.

Definition: Ka aciddissociationconstantacid dissociation constant measures the extent of acid dissociation in solution, with units of moldm⁻³.

Highlight: A high Ka value indicates greater acid dissociation and lower pH, while a low Ka value suggests less dissociation and higher pH.

Example: For a weak acid HA, the equilibrium equation is HAaqaq ⇌ H⁺aqaq + A⁻aqaq, with Ka = H+H⁺AA⁻/HAHA.

Vocabulary: pKa is the negative logarithm of Ka, providing a more manageable scale for comparing acid strengths.

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

View

Page 3: Titration and Neutralization

This page focuses on titration procedures and the interpretation of titration curves, explaining how pH changes during acid-base neutralization reactions.

Definition: The equivalence point is where the volume of one solution has exactly reacted with the volume of the second solution according to stoichiometry.

Highlight: Titration curves show three distinct regions: initial gradual pH change, rapid change near equivalence point, and final gradual change.

Example: During acid-base titration, pH changes slowly at first, then rapidly near the equivalence point, creating a characteristic S-shaped curve.

Vocabulary: Neutralization refers to the reaction between an acid and base to form water and a salt.

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

View

Page 3: Acid-Base Titrations and Indicators

This page details the behavior of pH during titrations and the mechanism of indicators.

Definition: Indicators are weak acids that change color at specific pH values due to their own acid-base equilibria.

Example: When base is added to an acidic solution containing phenolphthalein, the indicator changes from colorless to pink.

Highlight: The equivalence point occurs at the center of the vertical section in a titration curve.

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

View

Page 4: Buffer Solutions and Indicators

This page covers buffer solutions and indicator selection criteria.

Definition: A buffer solution consists of a weak acid and its conjugate base, maintaining stable pH when small amounts of acid or base are added.

Example: The ethanoic acid/sodium ethanoate system demonstrates buffer behavior.

Vocabulary: Conjugate base refers to the species formed when an acid loses a proton.

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Chemistry

252

1 Apr 2023

5 pages

Fun with Chemistry: Understanding Acids and Bases!

user profile picture

gracie keenan

@graciekeenan_

Understanding acid-base equilibria in chemistry is fundamental to grasping how acids and bases interact, including the significance of Ka in acid dissociation and methods for calculating pH of strong and weak acids.

  • Brønsted-Lowry theory defines acids as proton donors... Show more

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

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Page 2: Acid Strength and Dissociation Constants

This page delves deeper into the differences between strong and weak acids, introducing Ka aciddissociationconstantacid dissociation constant and its relationship to acid strength. The content explains how to calculate pH using equilibrium equations.

Definition: Ka aciddissociationconstantacid dissociation constant measures the extent of acid dissociation in solution, with units of moldm⁻³.

Highlight: A high Ka value indicates greater acid dissociation and lower pH, while a low Ka value suggests less dissociation and higher pH.

Example: For a weak acid HA, the equilibrium equation is HAaqaq ⇌ H⁺aqaq + A⁻aqaq, with Ka = H+H⁺AA⁻/HAHA.

Vocabulary: pKa is the negative logarithm of Ka, providing a more manageable scale for comparing acid strengths.

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

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Improve your grades

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By signing up you accept Terms of Service and Privacy Policy

Page 3: Titration and Neutralization

This page focuses on titration procedures and the interpretation of titration curves, explaining how pH changes during acid-base neutralization reactions.

Definition: The equivalence point is where the volume of one solution has exactly reacted with the volume of the second solution according to stoichiometry.

Highlight: Titration curves show three distinct regions: initial gradual pH change, rapid change near equivalence point, and final gradual change.

Example: During acid-base titration, pH changes slowly at first, then rapidly near the equivalence point, creating a characteristic S-shaped curve.

Vocabulary: Neutralization refers to the reaction between an acid and base to form water and a salt.

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

Sign up to see the contentIt's free!

Access to all documents

Improve your grades

Join milions of students

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Page 3: Acid-Base Titrations and Indicators

This page details the behavior of pH during titrations and the mechanism of indicators.

Definition: Indicators are weak acids that change color at specific pH values due to their own acid-base equilibria.

Example: When base is added to an acidic solution containing phenolphthalein, the indicator changes from colorless to pink.

Highlight: The equivalence point occurs at the center of the vertical section in a titration curve.

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

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Access to all documents

Improve your grades

Join milions of students

By signing up you accept Terms of Service and Privacy Policy

Page 4: Buffer Solutions and Indicators

This page covers buffer solutions and indicator selection criteria.

Definition: A buffer solution consists of a weak acid and its conjugate base, maintaining stable pH when small amounts of acid or base are added.

Example: The ethanoic acid/sodium ethanoate system demonstrates buffer behavior.

Vocabulary: Conjugate base refers to the species formed when an acid loses a proton.

Acid-Base equilibria
Brønsted-Lowry acid is a proton, H+, donor
Brønsted-Lowry base is a proton, H+, acceptor
An alkali is a base that disso

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Access to all documents

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By signing up you accept Terms of Service and Privacy Policy

Page 1: Fundamental Concepts of Acid-Base Chemistry

This page introduces core concepts in acid-base chemistry, focusing on the Brønsted-Lowry theory and water's role in acid-base reactions. The text explains how acids and bases interact in aqueous solutions and introduces the concept of calculating pH of strong and weak acids.

Definition: A Brønsted-Lowry acid is a proton H+H⁺ donor, while a Brønsted-Lowry base is a proton acceptor.

Highlight: Water molecules accept protons from acids to form hydronium ions H3O+H₃O⁺, demonstrating water's role as a base in acid dissociation.

Example: The dissociation of hydrochloric acid is written as HClaqaq + H₂Oll → H₃O⁺aqaq + Cl⁻aqaq, showing water's active role.

Vocabulary: Kw ionicproductofwaterionic product of water represents the product of H⁺ and OH⁻ concentrations in aqueous solutions.

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Thomas R

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Just amazing. Let's me revise 10x better, this app is a quick 10/10. I highly recommend it to anyone. I can watch and search for notes. I can save them in the subject folder. I can revise it any time when I come back. If you haven't tried this app, you're really missing out.

Basil

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This app has made me feel so much more confident in my exam prep, not only through boosting my own self confidence through the features that allow you to connect with others and feel less alone, but also through the way the app itself is centred around making you feel better. It is easy to navigate, fun to use, and helpful to anyone struggling in absolutely any way.

David K

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Greenlight Bonnie

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Rohan U

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I know a lot of apps use fake accounts to boost their reviews but this app deserves it all. Originally I was getting 4 in my English exams and this time I got a grade 7. I didn’t even know about this app three days until the exam and it has helped A LOT. Please actually trust me and use it as I’m sure you too will see developments.

Xander S

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THE QUIZES AND FLASHCARDS ARE SO USEFUL AND I LOVE THE SCHOOLGPT. IT ALSO IS LITREALLY LIKE CHATGPT BUT SMARTER!! HELPED ME WITH MY MASCARA PROBLEMS TOO!! AS WELL AS MY REAL SUBJECTS ! DUHHH 😍😁😲🤑💗✨🎀😮

Elisha

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