Calculate the pH of each solution given the following: f. [OH⁻] = 8.2 x 10⁻⁴ M

Verified step by step guidance

1. insert step 1> Calculate the pOH of the solution using the formula $\text{pOH}=-\log [{\text{OH}}^{-}]$.
2. insert step 2> Substitute the given hydroxide ion concentration $[{\text{OH}}^{-}]=8.2\times {10}^{-4}\text{ M}$ into the formula.
3. insert step 3> Use a calculator to find the value of $\text{pOH}$.
4. insert step 4> Use the relationship between pH and pOH: $\text{pH}+\text{pOH}=14$.
5. insert step 5> Solve for pH by subtracting the calculated pOH from 14.

Key Concepts

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.

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 hydroxide ion concentration is essential for calculating pH in basic solutions.

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.