Textbook Question
If you know the [OH-], how can you determine the pH of a solution?
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Ch.10 Acids and Bases and Equilibrium
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249
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Table of contents
- Ch.1 Chemistry in Our Lives19
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy53
- Ch.4 Atoms and Elements58
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions38
- Ch.8 Gases30
- Ch.9 Solutions50
- Ch.10 Acids and Bases and Equilibrium64
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons77
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones82
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides91
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis86
- Ch.18 Metabolic Pathways and ATP Production73
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 10, Problem 39d
Calculate the pH of each solution given the following:
f. [OH-] = 8.2 × 10-4 M
Verified step by step guidance1
Step 1: Recall the relationship between pH, pOH, and the concentration of hydroxide ions ([OH⁻]). The formula to calculate pOH is: .
Step 2: Substitute the given [OH⁻] value (8.2 × 10⁻⁴ M) into the formula for pOH. This will give you the pOH of the solution.
Step 3: Use the relationship between pH and pOH, which is: . Subtract the calculated pOH from 14 to find the pH.
Step 4: Ensure that your final pH value is reasonable. For a solution with a relatively high [OH⁻], the pH should be greater than 7, indicating a basic solution.
Step 5: Double-check your calculations for accuracy, especially when using logarithms and subtraction, to ensure the correct pH value is obtained.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
pH Scale
The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is considered neutral, while values below 7 indicate acidity and values above 7 indicate alkalinity. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration.
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Hydroxide Ion Concentration
Hydroxide ions (OH⁻) are negatively charged ions that play a crucial role in determining the basicity of a solution. The concentration of hydroxide ions can be used to calculate the pOH of a solution, which is related to pH through the equation pH + pOH = 14. Understanding the concentration of OH⁻ is essential for calculating the corresponding pH.
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Relationship Between pH and pOH
The relationship between pH and pOH is defined by the equation pH + pOH = 14 at 25°C. This means that if you know the pOH of a solution, you can easily find its pH by subtracting the pOH from 14. This relationship is fundamental in acid-base chemistry and is crucial for solving problems involving pH calculations.
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