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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

17. Acid and Base Equilibrium

The pH Scale

General Chemistry

17. Acid and Base Equilibrium

The pH Scale

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Multiple Choice

What is the pH of a neutral solution at a temperature where Kw = 2.3 x 10^-14?

6.00

7.00

6.65

7.35

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Verified step by step guidance

Understand that the pH of a neutral solution is determined by the concentration of hydrogen ions [H⁺] which is equal to the concentration of hydroxide ions [OH⁻]. In a neutral solution, [H⁺] = [OH⁻].

Recall that the ion product of water (Kw) is the product of the concentrations of hydrogen ions and hydroxide ions: Kw = [H⁺][OH⁻].

Given that Kw = 2.3 x 10^-14, and knowing that [H⁺] = [OH⁻] in a neutral solution, set up the equation: [H⁺]^2 = Kw.

Solve for [H⁺] by taking the square root of Kw: [H⁺] = √(2.3 x 10^-14).

Calculate the pH using the formula pH = -log[H⁺]. Substitute the value of [H⁺] obtained from the previous step into this formula to find the pH of the neutral solution.