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

Bronsted Lowry Acid and Base

GOB Chemistry

10. Acids and Bases

Bronsted Lowry Acid and Base

Previous problemNext problem

Struggling with GOB Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

Determine the chemical equation that would result when carbonate, CO3^2-, reacts with water.

Previous problemNext problem

Verified step by step guidance

Identify the reactants and products involved in the reaction. The reactants are carbonate ion (CO3^{2-}) and water (H2O). The products are bicarbonate ion (HCO3^{-}) and hydroxide ion (OH^{-}).

Recognize that this is an acid-base reaction where the carbonate ion acts as a base and water acts as an acid. The carbonate ion accepts a proton from water, forming bicarbonate ion and hydroxide ion.

Write the balanced chemical equation for the reaction: CO3^{2-} (aq) + H2O (l) \rightleftharpoons HCO3^{-} (aq) + OH^{-} (aq).

Understand that the reaction is reversible, as indicated by the double arrow (\rightleftharpoons), meaning it can proceed in both forward and reverse directions.

Consider the equilibrium state of the reaction, where the concentrations of reactants and products remain constant over time, and the reaction can shift depending on changes in conditions such as concentration, temperature, or pressure.