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Chapter 15: Problem 102

The \(\mathrm{pH}\) of a \(0.0642 \mathrm{M}\) solution of a monoprotic acid is \(3.86 .\) Is this a strong acid?

Short Answer

Expert verified
No, the given acid is not a strong acid.

Step by step solution

01

Identify Known Variables

We know:1. The solution's \(\mathrm{pH}\) is \(3.86\).2. The molarity (\(\mathrm{M}\)) of the solution is \(0.0642 \mathrm{M}\).
02

Calculating the Concentration of Hydronium Ions

First, we calculate the concentration of hydronium ions, \([H^+]\). The pH of a solution is calculated using the negative logarithmic formula \(pH = -\log[H^+]\). Therefore, rearranging the formula to find \([H^+]\), we get \([H^+] = 10^{-pH} = 10^{-3.86}\).
03

Comparing the Concentration of Hydronium Ions with Initial Concentration of Acid

Next, we compare the \([H^+]\) concentration to the initial concentration of the acid. If the \([H^+]\) concentration is equal to the initial concentration of the acid, then the acid is strong because all of it has ionized. If the \([H^+]\) concentration is less than the initial concentration of the acid, the acid is weak because only part of it has ionized.
04

Draw Conclusion

In this case, after calculation we find that \([H^+]\) is significantly less than the initial concentration of the acid, indicating that the acid is weak, not strong.

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Most popular questions from this chapter

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