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Chapter 14: Problem 32

Consider a \(0.10-M \mathrm{H}_{2} \mathrm{CO}_{3}\) solution and a \(0.10-M \mathrm{H}_{2} \mathrm{SO}_{4}\) solution. Without doing any detailed calculations, choose one of the following statements that best describes the \(\left[\mathrm{H}^{+}\right]\) of each solution and explain your answer. a. The \(\left[\mathrm{H}^{+}\right]\) is less than \(0.10 \mathrm{M}\). b. The \(\left[\mathrm{H}^{+}\right]\) is \(0.10 \mathrm{M}\). c. The \(\left[\mathrm{H}^{+}\right]\) is between \(0.10 \mathrm{M}\) and \(0.20 \mathrm{M}\). d. The \(\left[\mathrm{H}^{+}\right]\) is \(0.20 \mathrm{M}\).

Short Answer

Expert verified
The best statement to describe the [H+] of both the $0.10\mathrm{M}$ H₂CO₃ solution and the $0.10\mathrm{M}$ H₂SO₄ solution is c, which claims that the [H+] is between $0.10\mathrm{M}$ and $0.20\mathrm{M}$. This is because H₂CO₃, a weak diprotic acid, and H₂SO₄, a strong diprotic acid, release different amounts of H+ ions upon dissociation. The H₂CO₃ solution has a slightly higher H+ concentration than its initial concentration, while the H₂SO₄ solution has an H+ concentration between $0.10\mathrm{M}$ and $0.20\mathrm{M}$ due to more complete dissociation.

Step by step solution

01

Determine the dissociation process for H2CO3

H2CO3 is a weak diprotic acid, meaning it can donate two H+ ions, but it does not fully dissociate in solution. Its dissociation reactions are as follows: 1. H2CO3 ⇌ HCO3- + H+ 2. HCO3- ⇌ CO32- + H+ Since H2CO3 is a weak acid, the first dissociation reaction does not go to completion and only contributes a small amount of H+ ions. The second dissociation reaction involving HCO3- contributes an even smaller number of H+ ions. Hence, the concentration of H+ in the H2CO3 solution would be slightly more than the initial 0.10 M concentration of H2CO3.
02

Determine the dissociation process for H2SO4

H2SO4 is a strong diprotic acid, meaning it can donate two H+ ions and it fully dissociates in solution. Its dissociation reactions are as follows: 1. H2SO4 → HSO4- + H+ 2. HSO4- → SO42- + H+ The first dissociation reaction of H2SO4 goes to completion because it is a strong acid, contributing 0.10 M of H+ ions. The second dissociation of HSO4- does not go to completion, but it still releases a smaller amount of H+ ions. The concentration of H+ in the H2SO4 solution would be somewhere between 0.10 M (from the first dissociation) and 0.20 M (if both dissociations went to completion).
03

Compare H+ concentrations and choose the correct statement

We determined in step 1 that the concentration of H+ in the H2CO3 solution is slightly more than the initial 0.10 M H2CO3 concentration. In step 2, we determined that the H2SO4 solution has an H+ concentration between 0.10 M and 0.20 M. Comparing these results, we can choose the statement that the H+ concentration for each solution is: c. The [H+] is between 0.10 M and 0.20 M. This statement is the best description for both the 0.10 M H2CO3 solution and the 0.10 M H2SO4 solution.

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