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 Equivalents

GOB Chemistry

10. Acids and Bases

Acid-Base Equivalents

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3:45 minutes

Problem 91

Textbook Question

What are the molarity and the normality of a solution made by dissolving 25 g of citric acid (triprotic, C₆H₅O₇H₃) in enough water to make 800 mL of solution?

Verified step by step guidance

Step 1: Calculate the molar mass of citric acid (C₆H₈O₇). Add the atomic masses of all the atoms in the formula: 6 carbons, 8 hydrogens, and 7 oxygens. Use the periodic table to find the atomic masses (C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol).

Step 2: Determine the number of moles of citric acid in the solution. Use the formula: \( \text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \). Substitute the given mass of citric acid (25 g) and the molar mass calculated in Step 1.

Step 3: Calculate the molarity (M) of the solution. Use the formula: \( M = \frac{\text{moles of solute}}{\text{volume of solution in liters}} \). Convert the given volume of solution (800 mL) to liters by dividing by 1000, then substitute the moles of citric acid from Step 2 and the volume in liters.

Step 4: Understand the concept of normality (N) for a triprotic acid. Normality is defined as \( N = M \times \text{number of acidic protons per molecule} \). Since citric acid is triprotic, it can donate 3 protons (H⁺) per molecule. Multiply the molarity calculated in Step 3 by 3 to find the normality.

Step 5: Summarize the results. The molarity represents the concentration of citric acid in moles per liter, while the normality accounts for the total number of equivalents of H⁺ ions per liter. Ensure all units are consistent and clearly labeled.

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Key Concepts

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

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. To calculate molarity, you first need to determine the number of moles of the solute, which can be found by dividing the mass of the solute by its molar mass. In this case, citric acid's molar mass is approximately 192.13 g/mol, and the volume of the solution is 0.8 L.

Normality

Normality is another measure of concentration that accounts for the reactive capacity of a solute in a solution. It is defined as the number of equivalents of solute per liter of solution. For citric acid, which is triprotic, each molecule can donate three protons (H⁺ ions), so the normality will be three times the molarity when calculating the equivalents based on the acid's ability to donate protons.

Triprotic Acid

A triprotic acid is an acid that can donate three protons (H⁺ ions) per molecule in a solution. Citric acid (C₆H₅O₇H₃) is an example of a triprotic acid, which means that when calculating its normality, one must consider the total number of protons it can release. This characteristic is essential for determining the solution's acidity and its reactivity in various chemical reactions.

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