Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

10. Acids and Bases

Acid-Base Introduction

GOB Chemistry

10. Acids and Bases

Acid-Base Introduction

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3:45 minutes

Problem 83

Textbook Question

How does normality compare to molarity for monoprotic and polyprotic acids?

Verified step by step guidance

Understand the definitions: Molarity (M) is the number of moles of solute per liter of solution, while Normality (N) is the number of equivalents of solute per liter of solution. An equivalent depends on the reaction being studied, such as the number of protons (H⁺) an acid can donate.

For monoprotic acids (e.g., HCl): Each molecule of the acid donates one proton (H⁺) in a reaction. Therefore, the number of equivalents is equal to the number of moles. In this case, Normality (N) is equal to Molarity (M).

For polyprotic acids (e.g., H₂SO₄): Each molecule of the acid can donate more than one proton (H⁺). For example, sulfuric acid (H₂SO₄) can donate two protons. In this case, the Normality (N) is equal to the Molarity (M) multiplied by the number of protons the acid can donate. Mathematically, N = M × number of protons donated.

To calculate Normality for a polyprotic acid, identify the number of protons the acid can donate in the reaction. For example, if 1 M H₂SO₄ is fully dissociated, it will have a Normality of 2 N because it donates 2 protons per molecule.

Summarize the relationship: For monoprotic acids, Normality equals Molarity (N = M). For polyprotic acids, Normality is greater than Molarity and is calculated as N = M × number of protons donated.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Normality

Normality is a measure of concentration equivalent to the number of equivalents of solute per liter of solution. It is particularly useful in acid-base reactions, where it accounts for the reactive capacity of an acid or base. For monoprotic acids, which donate one proton per molecule, normality equals molarity. However, for polyprotic acids, which can donate multiple protons, normality can be greater than molarity, reflecting the total number of protons available for reaction.

Molarity

Molarity is defined as the number of moles of solute per liter of solution. It is a fundamental unit of concentration in chemistry, allowing for the quantification of solute in a given volume. Molarity does not consider the reactivity of the solute, making it a straightforward measure for solutions. In the context of acids, molarity provides a basis for understanding the concentration of the acid itself, regardless of its ability to donate protons.

Monoprotic vs. Polyprotic Acids

Monoprotic acids are acids that can donate only one proton (H+) per molecule, such as hydrochloric acid (HCl). In contrast, polyprotic acids can donate more than one proton; for example, sulfuric acid (H2SO4) can donate two protons. This distinction is crucial when comparing normality and molarity, as the normality of polyprotic acids can be significantly higher than their molarity due to the multiple protons they can release in solution.

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Which of the following compounds would produce the greatest concentration of hydrogen ions when dissolved?

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