Sure! Let's solve the problem step by step.
### Step-by-Step Solution:
1. Understanding pH:
- The pH of a solution is a measure of its acidity or basicity.
- pH is defined as the negative logarithm (base 10) of the hydrogen ion [tex]\([H^+]\)[/tex] concentration.
- In mathematical terms, this relationship is expressed as:
[tex]\[
\text{pH} = -\log[H^+]
\][/tex]
2. Given Information:
- We are given the pH of the HBr solution, which is 2.88.
3. Finding the hydrogen ion concentration [tex]\([H^+]\)[/tex]:
- To find [tex]\([H^+]\)[/tex], we need to rearrange the pH formula to solve for [tex]\([H^+]\)[/tex].
- Starting from the pH definition:
[tex]\[
\text{pH} = -\log[H^+]
\][/tex]
- We can rearrange this to solve for [tex]\([H^+]\)[/tex]:
[tex]\[
[H^+] = 10^{-\text{pH}}
\][/tex]
- Here, pH is given as 2.88, so substitute this value into the formula:
[tex]\[
[H^+] = 10^{-2.88}
\][/tex]
4. Calculating the numerical value:
- Evaluating this expression provides the hydrogen ion concentration:
[tex]\[
[H^+] = 10^{-2.88} \approx 0.0013182567385564075
\][/tex]
### Final Answer:
- The hydrogen ion concentration [tex]\([H^+]\)[/tex] for a solution with a pH of 2.88 is approximately [tex]\(0.0013182567385564075\, \text{M}\)[/tex].
So, the [tex]\([H^+]\)[/tex] concentration is [tex]\(0.0013182567385564075\, \text{M}\)[/tex].
