7 Questions
Which characteristic distinguishes strong acids from weak acids?
Weak acids partially dissociate in water
Which of these compounds is an example of an alkali?
NaOH
Which statement correctly describes the nature of pH indicators?
They change color in response to specific pH changes.
Why does a strong base like NaOH significantly alter the pH of a solution?
It completely dissociates in water to produce a high concentration of OH- ions.
Which acid only partially dissociates in water?
CH3COOH
What pH value would you expect for a neutral solution?
7
Which of the following is an example of a strong acid?
HClO4
Study Notes
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.
Test your knowledge of strong and weak acids, pH calculation, and acid-base chemistry. Learn about the difference between strong and weak acids, how to calculate pH, and more!
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