What is the theoretical pH of a 0.01 M HCl solution

The pH of a solution is calculated using the formula:

\[
\text{pH} = -\log[\text{H}^+]
\]

For a strong acid like HCl, it completely dissociates in water, meaning the concentration of hydrogen ions \([\text{H}^+]\) is equal to the concentration of the HCl solution.

Given:
- Concentration of HCl = 0.01 M
- \([\text{H}^+] = 0.01\text{ M} = 1 \times 10^{-2}\text{ M}\)

Now, using the pH formula:

\[
\text{pH} = -\log(1 \times 10^{-2})
\]

\[
\text{pH} = 2
\]

Therefore, the theoretical pH of a 0.01 M HCl solution is **2**.

Would you like further explanation on pH calculations or dissociation of acids?

Here are 5 related questions for further understanding:
1. How does pH change if the concentration of HCl is doubled?
2. What is the pH of a 0.001 M HCl solution?
3. How does temperature affect the pH of acidic solutions?
4. What is the difference between strong and weak acids in terms of pH?
5. How can we experimentally measure the pH of a solution?

**Tip:** Always remember that strong acids like HCl dissociate completely, making pH calculations straightforward based on concentration.

What is the theoretical pH of a 0.01 M HCl solution?

Find out how to calculate the theoretical pH of a 0.01 M HCl solution. This step-by-step explanation covers key concepts in acid-base chemistry, the use of logarithms, and the dissociation of strong acids. Suitable for high school students studying chemistry.

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