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Chapter 15: Problem 100

Can you neutralize a strong acid solution by adding an equal volume of a weak base having the same molarity as the acid? Support your position.

Short Answer

Expert verified
No, it is not possible to neutralize a strong acid solution by adding an equal volume of a weak base having the same molarity as the acid, because the weak base will not ionize completely leaving excess hydrogen ions and making the solution acidic.

Step by step solution

01

Understanding acids and bases

An acid is a substance that increases the concentration of hydrogen ions (\(H^+\)) in a solution, while a base is a substance that increases the concentration of hydroxide ions (\(OH^-\)). Acidity or alkalinity of a solution is measured by its pH, where low pH indicates an acidic solution and a high pH an alkaline (or basic) solution. A neutral solution has a pH of 7.
02

Comparing the strength of the acid and the base

In this question, a strong acid (almost fully ionized giving more \(H^+\)) is mixed with a weak base (partially ionizes giving fewer \(OH^-\)). When an acid reacts with a base, it results in a neutralization reaction. The acid’s \(H^+\) ions combine with the base’s \(OH^-\) ions to produce water.
03

Formulating the conclusion

Since the base is weak, and thus produces less \(OH^-\) ions, there will not be enough \(OH^-\) ions to react with all the \(H^+\) ions from the strong acid. Hence, even with equal volumes, the solution will still be acidic because there will be excess \(H^+\) ions.

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Most popular questions from this chapter

What volume of 0.100 \(\mathrm{M} \mathrm{NaOH}\) is required to neutralize 25.00 \(\mathrm{mL}\) of 0.150 \(\mathrm{M} \mathrm{HCl}\) ?

Identify each of the following compounds as an acid or a base according to the Bronsted-Lowry classification. For each species, write the formula and the name of its conjugate. \begin{equation} \begin{array}{l}{\text { a. } \mathrm{CH}_{3} \mathrm{COO}^{-}} \\ {\text { b. HCN }} \\ {\text { c. HOOCCOOH }} \\ {\text { d. } C_{6} \mathrm{H}_{5} \mathrm{NH}_{3}^{+}}\end{array} \end{equation}

If 133.73 \(\mathrm{mL}\) of a standard solution of \(\mathrm{KOH}\) , of concentration \(0.298 \mathrm{M},\) exactly neutralized 50.0 \(\mathrm{mL}\) of an acidic solution, what was the acid concentration?

To standardize a hydrochloric acid solution, it was used as titrant with a solid sample of sodium hydrogen carbonate, NaHCO \(_{3} .\) The sample had a mass of \(0.3967 \mathrm{g},\) and 41.77 \(\mathrm{mL}\) of acid was required to reach the equivalence point. Calculate the concentration of the standard solution.

What is the pH of a neutral solution?
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