Calculate The Ph of A 0.00234 M Hbr Solution
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Reviewed by Calculator Editorial Team
This guide explains how to calculate the pH of a 0.00234 M HBr (hydrobromic acid) solution. We'll cover the formula, assumptions, and how to interpret the result.
How to Calculate the pH of a 0.00234 M HBr Solution
The pH of a solution is a measure of its acidity or alkalinity. For a strong acid like HBr, we can calculate the pH directly from the concentration using the formula:
The pH Formula
pH = -log₁₀[H⁺]
Where [H⁺] is the concentration of hydrogen ions in moles per liter (M).
For a strong acid like HBr, the concentration of hydrogen ions [H⁺] is equal to the concentration of the acid itself, since the acid completely dissociates in water.
Assumptions
This calculation assumes:
- The solution is at 25°C (room temperature)
- HBr is a strong acid (completely dissociates in water)
- No other acids or bases are present
- The solution is dilute enough that activity coefficients are near 1
Worked Example
Let's calculate the pH of a 0.00234 M HBr solution step by step.
- Identify the concentration of H⁺ ions: [H⁺] = 0.00234 M
- Apply the pH formula: pH = -log₁₀(0.00234)
- Calculate the logarithm: log₁₀(0.00234) ≈ -2.630
- Multiply by -1: pH ≈ 2.630
The pH of a 0.00234 M HBr solution is approximately 2.63.
Interpreting the Result
A pH of 2.63 indicates a strongly acidic solution. This is characteristic of:
- Stomach acid
- Vinegar
- Battery acid
- Lemon juice
In the context of a 0.00234 M HBr solution:
- The solution will feel very sour to the touch
- It will turn blue litmus paper red
- It will react with metals to produce hydrogen gas
- It will neutralize bases until the pH reaches 7
Safety Note
Hydrobromic acid is corrosive and can cause severe burns. Always handle with proper protective equipment and in a well-ventilated area.
FAQ
What is the pH of a 0.00234 M HBr solution?
The pH is approximately 2.63, indicating a strongly acidic solution.
Why is the pH of HBr different from other strong acids?
The pH depends on the concentration of hydrogen ions. For HBr, [H⁺] = [HBr] because it's a strong acid.
Can I use this formula for other strong acids?
Yes, this formula applies to any strong acid where [H⁺] = [acid].
What happens if the temperature changes?
The pH calculation assumes 25°C. For other temperatures, you would need to account for temperature effects on dissociation.
How accurate is this calculation?
This calculation is accurate for dilute solutions where activity coefficients are near 1. For concentrated solutions, more advanced methods are needed.