Table of contents

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

pH of Strong Acids and Bases

General Chemistry

17. Acid and Base Equilibrium

pH of Strong Acids and Bases

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Multiple Choice

Calculate the concentration of a NaOH solution that has a pH of 11.3.

2.0 x 10^-3 M

1.0 x 10^-2 M

5.0 x 10^-3 M

7.9 x 10^-3 M

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Verified step by step guidance

Understand that pH is a measure of the hydrogen ion concentration in a solution. The pH scale is logarithmic, and a pH of 7 is neutral. A pH greater than 7 indicates a basic solution.

Recall the relationship between pH and pOH: \( \text{pH} + \text{pOH} = 14 \). Since the pH is given as 11.3, calculate the pOH by subtracting the pH from 14.

Use the formula \( \text{pOH} = -\log[\text{OH}^-] \) to find the hydroxide ion concentration. Rearrange this formula to solve for \([\text{OH}^-]\): \([\text{OH}^-] = 10^{-\text{pOH}}\).

Substitute the calculated pOH value into the equation \([\text{OH}^-] = 10^{-\text{pOH}}\) to find the concentration of hydroxide ions in the solution.

The concentration of NaOH in the solution is equal to the concentration of \([\text{OH}^-]\) because NaOH dissociates completely in water. Therefore, the concentration of NaOH is the same as the \([\text{OH}^-]\) concentration calculated in the previous step.