9 Questions
Acids are substances that accept a proton in a solution, decreasing the concentration of H+ ions.
False
The Arrhenius theory defines acids as substances that dissociate in water to produce OH- ions.
False
Bronsted-Lowry theory defines acids as substances that can accept a proton.
False
The pH of a solution is directly proportional to the concentration of H+ ions.
False
Weak acids completely dissociate in water, releasing all H+ ions.
False
The reaction between an acid and a base always results in the formation of a salt and water.
True
A strong base is a substance that partially dissociates in water, releasing some OH- ions.
False
The sum of pH and pOH is always equal to 12.
False
A conjugate acid is the species that forms after a base has donated a proton.
False
Study Notes
Acids and Bases
Definition of Acids and Bases
- Acids: Substances that donate a proton (H+ ion) in a solution, increasing the concentration of H+ ions.
- Bases: Substances that accept a proton (H+ ion) in a solution, decreasing the concentration of H+ ions.
Arrhenius Theory
- Acids: substances that dissociate in water to produce H+ ions (e.g., HCl, H2SO4)
- Bases: substances that dissociate in water to produce OH- ions (e.g., NaOH, KOH)
Bronsted-Lowry Theory
- Acids: substances that can donate a proton (H+ ion)
- Bases: substances that can accept a proton (H+ ion)
- Conjugate acid: the species that remains after an acid has donated a proton
- Conjugate base: the species that forms after a base has accepted a proton
pH and pOH
- pH: the negative logarithm of the H+ ion concentration (pH = -log[H+])
- pOH: the negative logarithm of the OH- ion concentration (pOH = -log[OH-])
- pH + pOH = 14 (at 25°C)
Strong and Weak Acids and Bases
- Strong acids: completely dissociate in water, releasing all H+ ions (e.g., HCl, H2SO4)
- Weak acids: partially dissociate in water, releasing some H+ ions (e.g., CH3COOH, HCN)
- Strong bases: completely dissociate in water, releasing all OH- ions (e.g., NaOH, KOH)
- Weak bases: partially dissociate in water, releasing some OH- ions (e.g., NH3, CO3^2-)
Acid-Base Reactions
- Neutralization: reaction between an acid and a base to form a salt and water
- Acid-base equilibrium: equilibrium between an acid and its conjugate base, or a base and its conjugate acid
Acids and Bases
Definition of Acids and Bases
- Acids donate a proton (H+ ion) in a solution, increasing H+ ion concentration
- Bases accept a proton (H+ ion) in a solution, decreasing H+ ion concentration
Arrhenius Theory
- Acids dissociate in water to produce H+ ions (e.g., HCl, H2SO4)
- Bases dissociate in water to produce OH- ions (e.g., NaOH, KOH)
Bronsted-Lowry Theory
- Acids can donate a proton (H+ ion)
- Bases can accept a proton (H+ ion)
- Conjugate acid is the species remaining after an acid donates a proton
- Conjugate base is the species formed after a base accepts a proton
pH and pOH
- pH is the negative logarithm of H+ ion concentration (pH = -log[H+])
- pOH is the negative logarithm of OH- ion concentration (pOH = -log[OH-])
- pH + pOH = 14 at 25°C
Strong and Weak Acids and Bases
- Strong acids completely dissociate in water, releasing all H+ ions (e.g., HCl, H2SO4)
- Weak acids partially dissociate in water, releasing some H+ ions (e.g., CH3COOH, HCN)
- Strong bases completely dissociate in water, releasing all OH- ions (e.g., NaOH, KOH)
- Weak bases partially dissociate in water, releasing some OH- ions (e.g., NH3, CO3^2-)
Acid-Base Reactions
- Neutralization reaction occurs between an acid and a base to form a salt and water
- Acid-base equilibrium is reached between an acid and its conjugate base, or a base and its conjugate acid
Learn about the definitions and theories of acids and bases, including Arrhenius and Bronsted-Lowry theories. Understand the characteristics of acids and bases in a solution.
Make Your Own Quizzes and Flashcards
Convert your notes into interactive study material.
Get started for free
