Chemistry Acids and Bases Overview

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Questions and Answers

What is the primary characteristic of a strong acid?

  • It has a low pKa value.
  • It has a high pH value.
  • It does not completely ionize in solution.
  • It completely ionizes in solution. (correct)

Which of the following statements about pH is correct?

  • pH is a measure of the concentration of hydroxide ions.
  • A pH of 7 is considered acidic.
  • pH values can range from -1 to 15.
  • pH decreases as the concentration of hydrogen ions increases. (correct)

How does the pKa of a weak acid relate to its strength?

  • pKa can only be calculated for strong acids.
  • The lower the pKa value, the stronger the acid. (correct)
  • pKa is not related to acid strength.
  • The higher the pKa value, the stronger the acid.

What role do buffers play in the bicarbonate buffer system?

<p>They resist changes in pH when acids or bases are added. (B)</p> Signup and view all the answers

What is the relationship between drug solubility and pH?

<p>Lower pH increases solubility of weak acids. (D)</p> Signup and view all the answers

Which statement about weak acids is true?

<p>Weak acids only ionize partially in solution. (A)</p> Signup and view all the answers

What does pKa represent in relation to acids?

<p>The acid dissociation constant in logarithmic form. (D)</p> Signup and view all the answers

In the bicarbonate buffer system, which component acts to neutralize excess acids?

<p>Bicarbonate ions (A)</p> Signup and view all the answers

How does chemical equilibrium relate to weak acids?

<p>Weak acids establish an equilibrium between dissociated and undissociated forms. (C)</p> Signup and view all the answers

What effect does a lower pH have on drug solubility?

<p>Increases solubility of weak acids. (D)</p> Signup and view all the answers

Flashcards

Acids and Bases

Substances that release or accept protons (H+ ions) in a solution.

Strong Acids

Acids that completely dissociate in water.

Chemical Equilibrium

A state where the forward and reverse reaction rates are equal.

Weak Acids

Acids that only partially dissociate in water.

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pH Scale

A scale used to measure the acidity or basicity of a solution.

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pKa

The negative logarithm of the acid dissociation constant.

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pH, pKa, Solubility, Diffusion

Factors influencing drug behavior in the body.

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Buffers

Solutions that resist changes in pH.

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Bicarbonate Buffer System

A crucial buffer in blood, maintaining its pH.

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Acid-Base definitions

Describes how acids and bases are categorized.

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Strong Acids

Acids that completely dissociate in water.

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Chemical Equilibrium

Reaction rates are equal; balanced.

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Weak Acids

Partially dissociate in water; less proton release.

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pH Scale

Measures acidity/alkalinity (basicity).

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pKa

Acid dissociation constant's negative log.

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pH, pKa, Solubility, Diffusion

Factors influencing drug movement.

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Buffers

Resist pH changes.

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Bicarbonate Buffer

Crucial buffer for blood pH.

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Study Notes

Acids and Bases—Definitions

  • Covers the fundamental definitions of acids and bases.

Strong Acids and Bases

  • Discusses strong acids and bases.

Chemical Equilibrium

  • Explores chemical equilibrium.

Weak Acids and Bases

  • Focuses on weak acids and bases.

pH and the pH Scale

  • Addresses the pH scale and its significance.

pKa

  • Examines the concept of pKa.

The Relationship Between pH, pKa, Drug Solubility, and Diffusion

  • Investigates the correlation between pH, pKa, drug solubility, and diffusion.

Buffers and Blood—The Bicarbonate Buffer System

  • Details buffers, particularly the bicarbonate buffer system in blood.

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Acids and Bases Definitions PDF

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