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Chapter 15: Problem 144

True or false? As a solution's acidity increases, its pH decreases.

Short Answer

Expert verified
True. As a solution's acidity increases, its pH decreases. This is because an increase in the concentration of hydrogen ions (H+) in a solution leads to an increase in the term -log[H+] in the pH formula, and due to the negative sign, this results in a decrease in the pH value.

Step by step solution

01

Understand Acidity and pH

Acidity refers to the concentration of hydrogen ions (H+) in a solution. A solution with a high concentration of H+ ions is considered to be acidic. pH, on the other hand, is a measure of the acidity or basicity of a solution. It is defined as the negative logarithm of the concentration of H+ ions in a solution. Mathematically, it is represented as: \(pH = -\log[H+]\) where [H+] is the concentration of H+ ions in a solution.
02

Analyze the relationship between Acidity and pH

As the acidity of a solution increases, the concentration of hydrogen ions ([H+]) in the solution also increases. From the pH formula mentioned above, if the [H+] concentration increases, the value inside the logarithm also increases. However, due to the negative sign in front of the logarithm in the pH formula, an increase in the term -log[H+] (which is the pH), will lead to a decrease in the pH value. Therefore, an increase in a solution's acidity corresponds to a decrease in its pH.
03

Conclusion

Based on the analysis and understanding of the relationship between acidity and pH, it can be concluded that the given statement is True. As a solution's acidity increases, its pH decreases.

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Most popular questions from this chapter

How many moles of nitric acid do you need to prepare \(200 \mathrm{~mL}\) of an aqueous solution that has a pH of \(2.0\) ?

Classify each substance as strong electrolyte, weak electrolyte, or nonelectrolyte: (a) \(\mathrm{CH}_{3} \mathrm{COOH}\) (b) \(\mathrm{KCH}_{3} \mathrm{COO}\) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (d) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) (e) \(\mathrm{NH}_{3}\) (f) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (g) \(\mathrm{ZnSO}_{4}\)

True or false? In an aqueous solution at \(25^{\circ} \mathrm{C}\), you will always get the same number when you multiply the equilibrium \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration by the equilibrium OH \(^{-}\) concentration. Explain your answer.

When \(\mathrm{Fe}^{3+}\) ions dissolve in water, they immediately form \(\left[\mathrm{Fe}\left(\mathrm{OH}_{2}\right)_{6}\right]^{3+}\) aqueous ions in which six molecules of water bind to the iron via six Fe-O bonds. However, this is not all that happens. The solution also becomes acidic. Interestingly, \(\mathrm{Fe}^{2+}\) ions also form similar \(\left[\mathrm{Fe}\left(\mathrm{OH}_{2}\right)_{6}\right]^{2+}\) ions, but the solution does not become acidic. Explain why one solution becomes acidic and the other does not. (Hint: The more positive the metal center, the more it attracts electrons to itself. Think about the effect this has on bonds within the ions.)

What is the \(\mathrm{OH}^{-}\) concentration of a solution that has a pH of \(9.66\) ? Is this solution acidic or basic?
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