Textbook Question
Sometimes, during stress or trauma, a person can start to hyperventilate. Then the person might breathe into a paper bag to avoid fainting.
b. How does breathing into a paper bag help return blood pH to normal?
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Table of contents
- 1. Matter and Measurements4h 29m
- What is Chemistry?7m
- The Scientific Method9m
- Classification of Matter16m
- States of Matter8m
- Physical & Chemical Changes19m
- Chemical Properties8m
- Physical Properties5m
- Intensive vs. Extensive Properties13m
- Temperature (Simplified)9m
- Scientific Notation13m
- SI Units (Simplified)5m
- Metric Prefixes24m
- Significant Figures (Simplified)11m
- Significant Figures: Precision in Measurements7m
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- Conversion Factors (Simplified)15m
- Dimensional Analysis22m
- Density12m
- Specific Gravity9m
- Density of Geometric Objects19m
- Density of Non-Geometric Objects8m
- 2. Atoms and the Periodic Table5h 22m
- The Atom (Simplified)9m
- Subatomic Particles (Simplified)12m
- Isotopes17m
- Ions (Simplified)22m
- Atomic Mass (Simplified)18m
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- Electronic Structure4m
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- The Electron Configuration: Exceptions (Simplified)12m
- Ions and the Octet Rule9m
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- Valence Electrons of Elements (Simplified)5m
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- Periodic Trend: Metallic Character4m
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- 3. Ionic Compounds2h 20m
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- Periodic Trend: Ionization Energy (Simplified)9m
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- Ionic Bonding6m
- Naming Monoatomic Cations6m
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- Polyatomic Ions25m
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- 4. Molecular Compounds2h 18m
- Covalent Bonds6m
- Naming Binary Molecular Compounds6m
- Molecular Models4m
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- Lewis Dot Structures: Neutral Compounds (Simplified)8m
- Multiple Bonds4m
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- Lewis Dot Structures: Multiple Bonds10m
- Lewis Dot Structures: Ions (Simplified)8m
- Lewis Dot Structures: Exceptions (Simplified)12m
- Resonance Structures (Simplified)5m
- Valence Shell Electron Pair Repulsion Theory (Simplified)4m
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- Molecular Geometry (Simplified)11m
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- 5. Classification & Balancing of Chemical Reactions3h 17m
- Chemical Reaction: Chemical Change5m
- Law of Conservation of Mass5m
- Balancing Chemical Equations (Simplified)13m
- Solubility Rules16m
- Molecular Equations18m
- Types of Chemical Reactions12m
- Complete Ionic Equations18m
- Calculate Oxidation Numbers15m
- Redox Reactions17m
- Spontaneous Redox Reactions8m
- Balancing Redox Reactions: Acidic Solutions17m
- Balancing Redox Reactions: Basic Solutions17m
- Balancing Redox Reactions (Simplified)13m
- Galvanic Cell (Simplified)16m
- 6. Chemical Reactions & Quantities2h 34m
- 7. Energy, Rate and Equilibrium3h 45m
- Nature of Energy6m
- First Law of Thermodynamics7m
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- Entropy (Simplified)9m
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- 8. Gases, Liquids and Solids3h 27m
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- Solutions6m
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- Parts per Million (ppm)13m
- Solubility: Temperature Effect8m
- Intro to Henry's Law4m
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- 10. Acids and Bases3h 10m
- Acid-Base Introduction11m
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- Ka and Kb16m
- The pH Scale16m
- Auto-Ionization9m
- pH of Strong Acids and Bases9m
- Acid-Base Equivalents14m
- Acid-Base Reactions7m
- Gas Evolution Equations (Simplified)6m
- Ionic Salts (Simplified)11m
- Buffers11m
- Henderson-Hasselbalch Equation16m
- Strong Acid Strong Base Titrations (Simplified)13m
- 11. Nuclear Chemistry1h 1m
- BONUS: Lab Techniques and Procedures1h 38m
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- 12. Introduction to Organic Chemistry1h 34m
- 13. Alkenes, Alkynes, and Aromatic Compounds2h 30m
- Spatial Orientation of Bonds3m
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- Hydrogenation Reaction3m
- Hydrohalogenation Reaction7m
- Hydration Reaction10m
- Naming Benzene19m
- Benzene Reactions10m
- Benzene Reaction: Nitration6m
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- 14. Compounds with Oxygen or Sulfur1h 22m
- 15. Aldehydes and Ketones1h 1m
- 16. Carboxylic Acids and Their Derivatives1h 11m
- 17. Amines40m
- 18. Amino Acids and Proteins2h 2m
- 19. Enzymes1h 37m
- 20. Carbohydrates1h 46m
- Intro to Carbohydrates4m
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- Enantiomers vs Diastereomers7m
- D vs L Enantiomers9m
- Cyclic Hemiacetals8m
- Intro to Haworth Projections4m
- Cyclic Structures of Monosaccharides11m
- Mutarotation4m
- Reduction of Monosaccharides10m
- Oxidation of Monosaccharides7m
- Glycosidic Linkage14m
- Disaccharides7m
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- 21. The Generation of Biochemical Energy2h 9m
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- 23. Lipids2h 26m
- Intro to Lipids6m
- Fatty Acids25m
- Physical Properties of Fatty Acids6m
- Waxes4m
- Triacylglycerols12m
- Triacylglycerol Reactions: Hydrogenation8m
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- Triacylglycerol Reactions: Oxidation7m
- Glycerophospholipids15m
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- Steroids15m
- Cell Membranes7m
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- 24. Lipid Metabolism1h 45m
- 25. Protein and Amino Acid Metabolism1h 37m
- 26. Nucleic Acids and Protein Synthesis2h 54m
- Intro to Nucleic Acids4m
- Nitrogenous Bases16m
- Nucleoside and Nucleotide Formation9m
- Naming Nucleosides and Nucleotides13m
- Phosphodiester Bond Formation7m
- Primary Structure of Nucleic Acids11m
- Base Pairing10m
- DNA Double Helix6m
- Intro to DNA Replication20m
- Steps of DNA Replication11m
- Types of RNA10m
- Overview of Protein Synthesis4m
- Transcription: mRNA Synthesis9m
- Processing of pre-mRNA5m
- The Genetic Code6m
- Introduction to Translation7m
- Translation: Protein Synthesis18m
10. Acids and Bases
Gas Evolution Equations (Simplified)
Multiple Choice
Predict the products formed from the following gas evolution equation.
A
KCl, H2CO3
B
CO2, H2O
C
KCl, CO2, H2O
D
KCl, H2, CO32–
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Verified step by step guidance1
Identify the reactants in the equation: Potassium bicarbonate (KHCO₃) and hydrochloric acid (HCl).
Recognize that this is a gas evolution reaction, where an acid reacts with a bicarbonate to produce carbon dioxide gas.
Write the balanced chemical equation for the reaction: KHCO₃(aq) + HCl(aq) → KCl(aq) + CO₂(g) + H₂O(l).
Understand that the bicarbonate ion (HCO₃⁻) reacts with the hydrogen ion (H⁺) from HCl to form carbonic acid (H₂CO₃), which decomposes into CO₂ and H₂O.
Note that the potassium ion (K⁺) from KHCO₃ combines with the chloride ion (Cl⁻) from HCl to form potassium chloride (KCl) in the solution.
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