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Questions and Answers
What is the definition of an acid?
What is the definition of an acid?
What is the pH of a neutral solution?
What is the pH of a neutral solution?
Which acid-base theory defines an acid as a proton donor?
Which acid-base theory defines an acid as a proton donor?
What is the relationship between pH and pOH at 25°C?
What is the relationship between pH and pOH at 25°C?
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What is the difference between a strong acid and a weak acid?
What is the difference between a strong acid and a weak acid?
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What is the purpose of pKa?
What is the purpose of pKa?
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Study Notes
Acid-Base Chemistry
Definitions
- Acid: a substance that donates a proton (H+ ion)
- Base: a substance that accepts a proton (H+ ion)
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pH: a measure of acidity or basicity, ranging from 0-14
- pH 7: neutral
- pH < 7: acidic
- pH > 7: basic
Acid-Base Theories
- Arrhenius Theory: acids dissociate in water to produce H+ ions, bases dissociate to produce OH- ions
- Bronsted-Lowry Theory: acids are proton donors, bases are proton acceptors
- Lewis Theory: acids are electron pair acceptors, bases are electron pair donors
pH Calculation
- pH = -log[H+]: pH is the negative logarithm of the hydrogen ion concentration
- pOH = -log[OH-]: pOH is the negative logarithm of the hydroxide ion concentration
- pH + pOH = 14: at 25°C, the sum of pH and pOH is always 14
Acid-Base Equilibrium
- K_a: acid dissociation constant, measures the strength of an acid
- K_b: base dissociation constant, measures the strength of a base
- pK_a: negative logarithm of K_a, used to compare acid strengths
- pK_b: negative logarithm of K_b, used to compare base strengths
Strong and Weak Acids/Bases
- Strong Acids: completely dissociate in water, e.g. HCl, H2SO4
- Weak Acids: partially dissociate in water, e.g. CH3COOH, HNO2
- Strong Bases: completely dissociate in water, e.g. NaOH, KOH
- Weak Bases: partially dissociate in water, e.g. NH3, CH3NH2
Acid-Base Chemistry
Definitions
- An acid is a substance that donates a proton (H+ ion).
- A base is a substance that accepts a proton (H+ ion).
- pH is a measure of acidity or basicity, ranging from 0-14, with 7 being neutral, below 7 being acidic, and above 7 being basic.
Acid-Base Theories
- Arrhenius Theory states that acids dissociate in water to produce H+ ions, while bases dissociate to produce OH- ions.
- Bronsted-Lowry Theory defines acids as proton donors and bases as proton acceptors.
- Lewis Theory describes acids as electron pair acceptors and bases as electron pair donors.
pH Calculation
- pH is calculated as the negative logarithm of the hydrogen ion concentration (pH = -log[H+]).
- pOH is calculated as the negative logarithm of the hydroxide ion concentration (pOH = -log[OH-]).
- At 25°C, the sum of pH and pOH is always 14 (pH + pOH = 14).
Acid-Base Equilibrium
- K_a is the acid dissociation constant, which measures the strength of an acid.
- K_b is the base dissociation constant, which measures the strength of a base.
- pK_a is the negative logarithm of K_a, used to compare acid strengths.
- pK_b is the negative logarithm of K_b, used to compare base strengths.
Strong and Weak Acids/Bases
- Strong acids completely dissociate in water, such as HCl and H2SO4.
- Weak acids partially dissociate in water, such as CH3COOH and HNO2.
- Strong bases completely dissociate in water, such as NaOH and KOH.
- Weak bases partially dissociate in water, such as NH3 and CH3NH2.
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Description
Test your knowledge of acid-base chemistry, including definitions, pH levels, and acid-base theories such as Arrhenius, Bronsted-Lowry, and Lewis.
