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Ch.10 Acids and Bases and Equilibrium
Timberlake - Chemistry: An Introduction to General, Organic, and Biological Chemistry 13th Edition
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Tutti i libri di testoTimberlake 13th EditionCh.10 Acids and Bases and EquilibriumProblema 107b
Capitolo 10, Problema 107b

Determine each of the following for a 0.050 M KOH solution:
b. pH

Guida verificata passo dopo passo
1
Step 1: Recognize that KOH is a strong base, meaning it completely dissociates in water. The concentration of OH⁻ ions in the solution will be equal to the concentration of KOH, which is 0.050 M.
Step 2: Use the relationship between pOH and the hydroxide ion concentration [OH⁻]. The formula is: pOH=-log(OH-). Substitute [OH⁻] = 0.050 M into the formula.
Step 3: Calculate the pOH value using the logarithmic expression. This step involves taking the negative logarithm of 0.050.
Step 4: Use the relationship between pH and pOH to find the pH. The formula is: pH=14-pOH. Substitute the calculated pOH value into this formula.
Step 5: Simplify the expression to determine the pH of the solution. This will give you the final pH value for the 0.050 M KOH solution.

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pH Scale

The pH scale measures the acidity or basicity of a solution, ranging from 0 to 14. A pH of 7 is neutral, below 7 indicates acidity, and above 7 indicates basicity. The scale is logarithmic, meaning each whole number change represents a tenfold change in hydrogen ion concentration.
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02:33
The pH Scale

Strong Bases

Strong bases, like potassium hydroxide (KOH), completely dissociate in water to produce hydroxide ions (OH-). This complete dissociation means that the concentration of hydroxide ions in a solution directly corresponds to the concentration of the base, allowing for straightforward calculations of pH.
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Strong Acids and Bases

Calculating pH from pOH

To find the pH of a solution, one can first calculate the pOH, which is derived from the concentration of hydroxide ions. The relationship between pH and pOH is given by the equation pH + pOH = 14. Thus, knowing the pOH allows for easy conversion to pH, essential for determining the acidity or basicity of the solution.
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pH and pOH Example
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