Acids, Bases, and Salts Quiz

Acids, Bases, and Salts

Strong and Weak Acids

• Strong acids:
  • Completely dissociate in water to produce H+ ions
  • Examples: HCl, HNO3, H2SO4, HClO4
  • High concentration of H+ ions, resulting in a low pH
• Weak acids:
  • Partially dissociate in water to produce H+ ions
  • Examples: CH3COOH, HCO3-, H2CO3
  • Low concentration of H+ ions, resulting in a higher pH

pH Calculation

• pH = -log[H+]
• pH scale: 0-14
  • Acidic: pH < 7
  • Neutral: pH = 7
  • Basic: pH > 7
• pH calculation examples:
  • If [H+] = 0.01 M, pH = -log(0.01) = 2
  • If [H+] = 1 x 10^-5 M, pH = -log(1 x 10^-5) = 5

Alkalis and Bases

• Alkalis:
  • Soluble bases that contain the hydroxide (OH-) ion
  • Examples: NaOH, KOH, Ca(OH)2
  • Strong bases, completely dissociate in water to produce OH- ions
• Bases:
  • Accept H+ ions to form a conjugate acid
  • Examples: NH3, H2O, CO3^2-
  • Can be strong or weak, depending on the extent of dissociation

Indicators

• pH indicators:
  • Substances that change color in response to changes in pH
  • Examples: litmus, phenolphthalein, methyl orange
  • Used to determine the pH of a solution
• Acid-base indicators:
  • Substances that change color in response to the presence of acidic or basic substances
  • Examples: bromothymol blue, Congo red
  • Used to determine the presence of acids or bases in a solution

Acids, Bases, and Salts

Strong and Weak Acids

• Strong acids completely dissociate in water to produce H+ ions, resulting in a high concentration of H+ ions and a low pH.
• Examples of strong acids include HCl, HNO3, H2SO4, and HClO4.
• Weak acids partially dissociate in water to produce H+ ions, resulting in a low concentration of H+ ions and a higher pH.
• Examples of weak acids include CH3COOH, HCO3-, and H2CO3.

pH Calculation

• pH is calculated using the formula pH = -log[H+].
• The pH scale ranges from 0-14, with acidic solutions having a pH < 7, neutral solutions having a pH = 7, and basic solutions having a pH > 7.
• Examples of pH calculations include:
  • If [H+] = 0.01 M, pH = -log(0.01) = 2.
  • If [H+] = 1 x 10^-5 M, pH = -log(1 x 10^-5) = 5.

Alkalis and Bases

• Alkalis are soluble bases that contain the hydroxide (OH-) ion and completely dissociate in water to produce OH- ions.
• Examples of alkalis include NaOH, KOH, and Ca(OH)2.
• Bases are substances that accept H+ ions to form a conjugate acid.
• Examples of bases include NH3, H2O, and CO3^2-.
• Bases can be strong or weak, depending on the extent of dissociation.

Indicators

• pH indicators are substances that change color in response to changes in pH, used to determine the pH of a solution.
• Examples of pH indicators include litmus, phenolphthalein, and methyl orange.
• Acid-base indicators are substances that change color in response to the presence of acidic or basic substances, used to determine the presence of acids or bases in a solution.
• Examples of acid-base indicators include bromothymol blue and Congo red.