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Chapter 15: Problem 215

Is a solution that contains \(0.10 \mathrm{M} \mathrm{HBr}\) and \(0.10 \mathrm{M}\) NaBr a buffered solution? Why or why not?

Short Answer

Expert verified
The solution containing 0.10 M HBr and 0.10 M NaBr is not a buffered solution because it does not contain a weak acid with its conjugate base or a weak base with its conjugate acid. HBr is a strong acid and cannot act as a buffer, while NaBr is the salt of a strong acid and a strong base, and its dissociation does not affect the pH of the solution.

Step by step solution

01

Identify the substances in the solution.

In the solution, there are two substances: HBr (hydrobromic acid) and NaBr (sodium bromide). HBr is a strong acid, and its conjugate base is Br⁻ (bromide ion). NaBr is the salt of a strong acid (HBr) and a strong base (NaOH); it will ionize completely into Na⁺ (sodium ion) and Br⁻ (bromide ion) in the solution.
02

Determine the nature of the substances in the solution.

HBr, as a strong acid, dissociates completely in the solution and yields a high concentration of H⁺ ions, resulting in a low pH. Since it is a strong acid, it cannot act as a buffer. NaBr, as mentioned earlier, is the salt of a strong acid and a strong base, and its dissociation will not affect the pH of the solution. Therefore, NaBr cannot act as a buffer either.
03

Analyze the solution's buffering capability.

For a solution to be a buffered solution, it needs to contain a weak acid and its conjugate base OR a weak base and its conjugate acid. In our case, the solution contains neither a weak acid with its conjugate base nor a weak base with its conjugate acid. HBr is a strong acid, and NaBr is a salt that does not contribute to the buffering system.
04

Conclude whether the solution is a buffered solution or not.

Based on the analysis, neither HBr nor NaBr can act as buffers in the solution. Thus, the solution containing 0.10 M HBr and 0.10 M NaBr is not a buffered solution.

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