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Chapter 15: Problem 4

Could a buffered solution be made by mixing aqueous solutions of \(\mathrm{HCl}\) and \(\mathrm{NaOH}\) ? Explain. Why isn't a mixture of a strong acid and its conjugate base considered a buffered solution?

Short Answer

Expert verified
A buffered solution cannot be made by mixing aqueous solutions of HCl and NaOH, as they undergo a neutralization reaction to form water and NaCl without forming a proper conjugate system. The solution lacks buffering capacity, which is required to resist changes in pH upon the addition of small amounts of acid or base. This is why a mixture of a strong acid and its conjugate base is not considered a buffered solution.

Step by step solution

01

Identify the nature of the given compounds

HCl is a strong acid, and NaOH is a strong base. When these two compounds are mixed in an aqueous solution, they will undergo complete ionization.
02

Chemical reaction between HCl and NaOH

When HCl and NaOH are mixed in an aqueous solution, they will react together to form water and a salt (NaCl) through a neutralization reaction. The balanced chemical equation for this reaction is: \[ \mathrm{HCl} + \mathrm{NaOH} \rightarrow \mathrm{H_{2}O} + \mathrm{NaCl} \]
03

Determine the conjugate system

In the case of a strong acid and a strong base, there is no proper conjugate system formed. The reaction between HCl and NaOH produces water, in which the H+ ions from HCl and the OH- ions from NaOH combine to form neutral water molecules, not creating any additional buffer ions or molecules. The salt, NaCl, is not involved in any further reactions that can help maintain the pH of the solution.
04

Buffering capacity

Buffer solutions should be able to maintain their pH upon the addition of small amounts of acid or base. In the case of a mixture of HCl and NaOH, the solution has no buffering capacity, as there is no weak acid or weak base present, which typically shows resistance to changes in pH when small amounts of acid or base are added.
05

Conclusion

A buffered solution cannot be made by mixing aqueous solutions of HCl and NaOH, as they completely react with each other in a neutralization reaction with no proper conjugate system formed. A mixture of a strong acid and its conjugate base is not considered a buffered solution because it lacks the buffering capacity needed to resist changes in pH upon the addition of small amounts of acid or base.

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Most popular questions from this chapter

Amino acids are the building blocks for all proteins in our bodies. A structure for the amino acid alanine is All amino acids have at least two functional groups with acidic or basic properties. In alanine, the carboxylic acid group has \(K_{\mathrm{a}}=4.5 \times 10^{-3}\) and the amino group has \(K_{\mathrm{b}}=\) \(7.4 \times 10^{-5}\). Because of the two groups with acidic or basic properties, three different charged ions of alanine are possible when alanine is dissolved in water. Which of these ions would predominate in a solution with \(\left[\mathrm{H}^{+}\right]=1.0 M ?\) In a solution with \(\left[\mathrm{OH}^{-}\right]=1.0 M ?\)

Calculate the \(\mathrm{pH}\) of a solution that is \(0.60 \mathrm{M} \mathrm{HF}\) and \(1.00 M \mathrm{KF}\).

Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major species, and explain how you would go about calculating the \(\mathrm{pH}\) of the solution at various points, including the halfway point and the equivalence point.

Consider the titration of \(150.0 \mathrm{~mL}\) of \(0.100 \mathrm{M}\) HI by \(0.250 \mathrm{M}\) \(\mathrm{NaOH} .\) a. Calculate the \(\mathrm{pH}\) after \(20.0 \mathrm{~mL}\) of \(\mathrm{NaOH}\) has been added. b. What volume of \(\mathrm{NaOH}\) must be added so that the \(\mathrm{pH}=\) \(7.00 ?\)

A buffer solution is prepared by mixing \(75.0 \mathrm{~mL}\) of \(0.275 \mathrm{M}\) fluorobenzoic acid \(\left(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{O}_{2} \mathrm{~F}\right)\) with \(55.0 \mathrm{~mL}\) of \(0.472 \mathrm{M}\) so- dium fluorobenzoate. The \(\mathrm{p} K_{\mathrm{a}}\) of this weak acid is \(2.90\). What is the \(\mathrm{pH}\) of the buffer solution?
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