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

9. Solutions

Molarity

GOB Chemistry

9. Solutions

Molarity

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Multiple Choice

2.64 grams of an unknown compound was dissolved in water to yield 150 mL of solution. The concentration of the solution was 0.075 M. What was the molecular weight of the substance?

190 g/mol

30 g/mol

90 g/mol

230 g/mol

320 g/mol

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Verified step by step guidance

Start by understanding the relationship between molarity, moles, and volume. Molarity (M) is defined as moles of solute per liter of solution. The formula is: \( M = \frac{n}{V} \), where \( n \) is the number of moles and \( V \) is the volume in liters.

Convert the volume of the solution from milliliters to liters. Since there are 1000 mL in a liter, divide 150 mL by 1000 to get 0.150 L.

Use the molarity formula to find the number of moles of the unknown compound. Rearrange the formula to solve for \( n \): \( n = M \times V \). Substitute the given values: \( n = 0.075 \text{ M} \times 0.150 \text{ L} \).

Calculate the number of moles using the values from the previous step. This will give you the moles of the unknown compound present in the solution.

Finally, determine the molecular weight of the compound using the formula: \( ext{Molecular Weight} = \frac{ ext{mass}}{ ext{moles}} \). Substitute the mass of the compound (2.64 grams) and the moles calculated in the previous step to find the molecular weight.