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Chapter 15: Problem 80

In a certain experiment a student finds that the \(\mathrm{pHs}\) of \(0.10 M\) solutions of three potassium salts \(\mathrm{KX}\), \(\mathrm{KY},\) and \(\mathrm{KZ}\) are \(7.0,9.0,\) and \(11.0,\) respectively. Arrange the acids \(\mathrm{HX}, \mathrm{HY},\) and \(\mathrm{HZ}\) in the order of increasing acid strength.

Short Answer

Expert verified
The order of increasing acid strength is: HZ < HX < HY.

Step by step solution

01

Understanding the relationship between pH and acidity

Firstly, understand that the pH of a solution is inversely proportional to the concentration of hydronium ions (\(H_3O^+\)). A low pH means a high concentration of \(H_3O^+\) ions and thus a strong acid. Whereas, a high pH indicates a low concentration of \(H_3O^+\) ions, implying a weak acid.
02

Discussing the significance of potassium salts

Potassium salts such as KX, KY, and KZ are strong electrolytes. They will dissociate completely in water to give their corresponding anions and potassium ions. These anions are the conjugate bases of the respective acids HX, HY, and HZ. If the conjugate base is strong, it means the acid is weak and vice versa.
03

Arranging acids in the order of their strengths

From the pH values given, KX gives a pH of 7, implying that X^- is a neutral species and HX is a neutral acid. KY gives a pH of 9, meaning Y^- is a weak base and thus HY is a slightly stronger acid than HX. KZ gives a pH of 11, indicating that Z^- is a strong base and hence HZ is the weakest acid. Thus, the acids in order of increasing strength are HZ < HX < HY.

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Most popular questions from this chapter

Use Le Châtelier's principle to predict the effect of the following changes on the extent of hydrolysis of sodium nitrite \(\left(\mathrm{NaNO}_{2}\right)\) solution: (a) \(\mathrm{HCl}\) is added, (b) \(\mathrm{NaOH}\) is added, (c) \(\mathrm{NaCl}\) is added, (d) the solution is diluted.

Explain why small, highly charged metal ions are able to undergo hydrolysis.

Define salt hydrolysis. Categorize salts according to how they affect the \(\mathrm{pH}\) of a solution.

Write the equation relating \(K_{\mathrm{a}}\) for a weak acid and \(K_{\mathrm{b}}\) for its conjugate base. Use \(\mathrm{NH}_{3}\) and its conjugate acid \(\mathrm{NH}_{4}^{+}\) to derive the relationship between \(K_{\mathrm{a}}\) and \(K_{\mathrm{b}}\).

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