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Chapter 15: Problem 219

\(\mathrm{HClO}_{4}\) is a strong acid, and \(\mathrm{HClO}_{2}\) is a weak acid. If you had a \(1.0 \mathrm{M}\) solution of \(\mathrm{NaClO}_{4}\) and a \(1.0 \mathrm{M}\) solution of \(\mathrm{NaClO}_{2}\), which would have the higher pH? Explain.

Short Answer

Expert verified
The 1.0 M NaClO2 solution would have a higher pH than the 1.0 M NaClO4 solution because HClO2 is a weak acid, producing fewer H3O+ ions in solution than the strong acid HClO4.

Step by step solution

01

NaClO4 is the sodium salt of HClO4, which is a strong acid, whereas NaClO2 is the sodium salt of HClO2, which is a weak acid. #Step 2: Write the dissociation equation for each salt#

When NaClO4 and NaClO2 dissociate in water, they form their corresponding acidic species and Na+ ions. The equation for the dissociation of NaClO4 and NaClO2 can be represented by: \( NaClO_4 \rightarrow ClO_4^- + Na^+ \) \( NaClO_2 \rightarrow ClO_2^- + Na^+ \) #Step 3: Determine the degree of dissociation for each salt#
02

For NaClO4, ClO4- comes from a strong acid HClO4, and it is completely dissociated in water. Therefore, the degree of dissociation is 100%. With 1.0 M concentration of NaClO4, the resulting concentration of ClO4- is also 1.0 M. For NaClO2, ClO2- comes from a weak acid HClO2; it does not dissociate completely in water. However, we can assume a significant dissociation, leading to a certain concentration of ClO2- based on the Ka of HClO2. #Step 4: Assess the pH of the solutions and compare#

Since ClO4- has a higher concentration and comes from a strong acid, it contributes more H3O+ ions to the water than ClO2- does, resulting in a lower pH for the NaClO4 solution. Inversely, as NaClO2 comes from a weak acid, there will be fewer H3O+ ions produced by the ClO2- ions; this will result in a higher pH for the NaClO2 solution compared to the NaClO4 solution. Conclusion:
03

Conclusion

The 1.0 M NaClO2 solution would have a higher pH than the 1.0 M NaClO4 solution because HClO2 is a weak acid, producing fewer H3O+ ions in solution than the strong acid HClO4.

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Most popular questions from this chapter

Suppose \(2.0\) moles of sodium acetate, \(\mathrm{NaO}_{2} \mathrm{CCH}_{3}\), are dissolved in some water and then \(1.0 \mathrm{~L}\) of a \(1.0 \mathrm{M} \mathrm{HCl}\) solution is added. (a) Write the chemical reaction that occurs. (b) After the reaction, what are the predominant species in solution? How many moles of each species are there? (c) Is the resulting solution a buffer? If yes, explain why.

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

Consider the autoionization of water. (a) What do we mean by autoionization of water (b) Write a balanced equation to go along with your explanation. (c) An alternate name for autoionization of water is autodissociation. Exactly how is water dissociating?

An ionic compound with the formula \(\operatorname{NaX}(\mathrm{X}\) is an unknown anion) is dissolved in water, and the resulting solution is basic. Is HX a strong acid or a weak acid? Explain.

If pure water has both hydronium ions (acid) and hydroxide ions (base) in it, how can it be neutral?
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