Th pH of a 0.050 M weak acid is 3.00. What is the percentage ionization?

To calculate the percentage ionization of the weak acid, we use the following steps:

1. **Step 1: Determine the concentration of hydrogen ions ([H⁺])** using the given pH.

\[
\text{pH} = 3.00
\]
The concentration of hydrogen ions, \([H^+]\), is found using the formula:
\[
[H^+] = 10^{-\text{pH}} = 10^{-3.00} = 1.00 \times 10^{-3} \, \text{M}
\]

2. **Step 2: Calculate the ionization of the weak acid.**

The percentage ionization is given by:
\[
\text{Percentage ionization} = \left(\frac{[H^+]}{\text{Initial concentration of the acid}}\right) \times 100
\]

Given that the initial concentration of the weak acid is 0.050 M, we plug in the values:
\[
\text{Percentage ionization} = \left(\frac{1.00 \times 10^{-3}}{0.050}\right) \times 100 = 2.00\%
\]

Thus, the percentage ionization of the weak acid is **2.00%**.

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Would you like further details or have any other questions? Here are 5 related questions you could explore:

1. How does the initial concentration of a weak acid affect its percentage ionization?
2. What is the relationship between Ka (acid dissociation constant) and pH for weak acids?
3. How does the pH of a solution change if the weak acid concentration is doubled?
4. Can a weak base exhibit a similar ionization behavior? How is it different?
5. How do strong acids differ from weak acids in terms of percentage ionization?

**Tip**: Percentage ionization increases as the concentration of the weak acid decreases, because the acid dissociates more in dilute solutions.

The pH of a 0.050 M weak acid is 3.00. What is the percentage ionization?

Learn how to calculate the percentage ionization of a weak acid with a concentration of 0.050 M and a pH of 3.00. This detailed solution covers the relationship between pH, hydrogen ion concentration, and percentage ionization. Suitable for high school students in Grades 10-12.

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