Acid-Base Chemistry Quiz

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Questions and Answers

What is the definition of an acid in acid-base chemistry?

A substance that donates a proton (H+)

What is the pH of a neutral solution?

7

What is the formula for calculating pH?

pH = -log[H+]

What is the main difference between a strong acid and a weak acid?

<p>A strong acid completely dissociates in water, releasing all H+ ions, while a weak acid partially dissociates, releasing some H+ ions.</p> Signup and view all the answers

What is the product of a neutralization reaction between an acid and a base?

<p>Salt and water</p> Signup and view all the answers

What is the normal pH range of human blood?

<p>7.35-7.45</p> Signup and view all the answers

What are the three main mechanisms that regulate blood pH?

<p>Respiratory system, renal system, and buffers</p> Signup and view all the answers

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Study Notes

Acid-Base Chemistry

Definition

  • Acid: a substance that donates a proton (H+)
  • Base: a substance that accepts a proton (H+)

pH Scale

  • pH: a measure of acidity/basicity, ranging from 0-14
  • pH 7: neutral (neither acidic nor basic)
  • pH < 7: acidic
  • pH > 7: basic

pH Calculation

  • pH = -log[H+]
  • [H+] = concentration of hydrogen ions (in moles per liter)

Strong and Weak Acids/Bases

  • Strong acids: completely dissociate in water, releasing all H+ ions
    • Examples: HCl, HNO3, H2SO4
  • Weak acids: partially dissociate in water, releasing some H+ ions
    • Examples: CH3COOH, HCO3-
  • Strong bases: completely dissociate in water, releasing all OH- ions
    • Examples: NaOH, KOH
  • Weak bases: partially dissociate in water, releasing some OH- ions
    • Examples: NH3, CH3NH2

Acid-Base Reactions

  • Neutralization reaction: acid + base → salt + water
    • Example: HCl + NaOH → NaCl + H2O
  • Acid-base conjugate pairs: acid + base ⇌ conjugate acid + conjugate base
    • Example: HCl + H2O ⇌ H3O+ + Cl-

Blood pH Regulation

  • Blood pH range: 7.35-7.45
  • Regulation mechanisms:
    • Respiratory system: controls CO2 levels, which affect pH
    • Renal system: controls H+ and HCO3- levels
    • Buffers: help maintain pH homeostasis

Acid-Base Chemistry

Definition and pH Scale

  • Acid: a substance that donates a proton (H+)
  • Base: a substance that accepts a proton (H+)
  • pH: a measure of acidity/basicity, ranging from 0-14
  • pH 7: neutral (neither acidic nor basic)
  • pH < 7: acidic
  • pH > 7: basic

pH Calculation

  • pH = -log[H+], where [H+] is the concentration of hydrogen ions (in moles per liter)

Strong and Weak Acids/Bases

  • Strong acids:
    • Completely dissociate in water, releasing all H+ ions
    • Examples: HCl, HNO3, H2SO4
  • Weak acids:
    • Partially dissociate in water, releasing some H+ ions
    • Examples: CH3COOH, HCO3-
  • Strong bases:
    • Completely dissociate in water, releasing all OH- ions
    • Examples: NaOH, KOH
  • Weak bases:
    • Partially dissociate in water, releasing some OH- ions
    • Examples: NH3, CH3NH2

Acid-Base Reactions

  • Neutralization reaction:
    • Acid + base → salt + water
    • Example: HCl + NaOH → NaCl + H2O
  • Acid-base conjugate pairs:
    • Acid + base ⇌ conjugate acid + conjugate base
    • Example: HCl + H2O ⇌ H3O+ + Cl-

Blood pH Regulation

  • Blood pH range: 7.35-7.45
  • Regulation mechanisms:
    • Respiratory system: controls CO2 levels, which affect pH
    • Renal system: controls H+ and HCO3- levels
    • Buffers: help maintain pH homeostasis

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