Determine both the  [H^+] and the pH in a 0.0541 M solution of HNO_3 at 25 °C

Nitric acid (HNO₃) is a strong acid, meaning it dissociates completely in water. Therefore, the concentration of \([H^+]\) ions in the solution will be equal to the concentration of the acid itself.

### Step 1: Find the \([H^+]\)
Given that HNO₃ dissociates completely:
\[
\text{HNO}_3 \rightarrow \text{H}^+ + \text{NO}_3^-
\]
The concentration of \([H^+]\) will be equal to the concentration of HNO₃:
\[
[H^+] = 0.0541 \text{ M}
\]

### Step 2: Calculate the pH
The pH is calculated using the formula:
\[
\text{pH} = -\log[H^+]
\]
Substituting the value:
\[
\text{pH} = -\log(0.0541)
\]
\[
\text{pH} \approx 1.267
\]

### Final Answer:
- \([H^+] = 0.0541 \text{ M}\)
- \(\text{pH} \approx 1.267\)

Would you like further details or have any questions?

Here are 5 related questions:
1. How does the pH change if the concentration of HNO₃ is doubled?
2. What is the pOH of this solution?
3. How do you determine the pH of a weak acid solution?
4. How does temperature affect the dissociation of strong acids like HNO₃?
5. What happens to the pH when a strong base is added to this solution?

**Tip:** For strong acids, the \([H^+]\) concentration is equal to the molarity of the acid since they dissociate completely in water.

Determine both the [H^+] and the pH in a 0.0541 M solution of HNO_3 at 25 °C

Find the [H^+] and pH of a 0.0541 M HNO₃ solution at 25°C with this detailed guide. Understand how to determine the hydrogen ion concentration and calculate the pH using logarithms and acid-base principles. Perfect for Grades 10-12 students studying chemistry and logarithmic functions.

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