Podcast
Questions and Answers
What is the definition of an acid in acid-base chemistry?
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?
What is the pH of a neutral solution?
7
What is the formula for calculating pH?
What is the formula for calculating pH?
pH = -log[H+]
What is the main difference between a strong acid and a weak acid?
What is the main difference between a strong acid and a weak acid?
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What is the product of a neutralization reaction between an acid and a base?
What is the product of a neutralization reaction between an acid and a base?
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What is the normal pH range of human blood?
What is the normal pH range of human blood?
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What are the three main mechanisms that regulate blood pH?
What are the three main mechanisms that regulate blood pH?
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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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Description
Test your knowledge of acid-base chemistry, including the definition of acids and bases, pH scale, pH calculation, and strong and weak acids/bases.
