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Chapter 14: Problem 36

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\(M\) b. The \(\left[\mathrm{H}^{+}\right]\) is 0.10\(M .\) c. The \(\left[\mathrm{H}^{+}\right]\) is between 0.10\(M\) and 0.20 \(\mathrm{M}\) d. The \(\left[\mathrm{H}^{+}\right]\) is 0.20 \(\mathrm{M}\)

Short Answer

Expert verified
For the 0.10 M H₂CO₃ solution, the [H⁺] is less than 0.10 M (option a) because it is a weak acid and only partially dissociates. For the 0.10 M H₂SO₄ solution, the [H⁺] is 0.20 M (option d) because it is a strong acid and completely dissociates, contributing 2 H⁺ ions per molecule.

Step by step solution

01

Acid Dissociation and Types of Acids

We are dealing with two acids, H₂CO₃ (carbonic acid) and H₂SO₄ (sulfuric acid). To find the [H⁺] of each solution, we need to understand how each acid dissociates in water. Carbonic acid (H₂CO₃) is a weak acid, which means it only partially dissociates in water: \(H_{2}CO_{3} \rightleftharpoons H^{+} + HCO_{3}^{-}\) Sulfuric acid (H₂SO₄) is a strong acid, which means it completely dissociates in water: \(H_{2}SO_{4} \rightarrow 2H^{+} + SO_{4}^{2-}\)
02

Comparison of [H⁺] Concentrations

For the 0.10 M H₂CO₃ solution: Since H₂CO₃ is a weak acid, it only partially dissociates, meaning that the [H⁺] will not reach 0.10 M. Thus, the [H⁺] is less than 0.10 M for the H₂CO₃ solution, which corresponds to option a. For the 0.10 M H₂SO₄ solution: Since H₂SO₄ is a strong acid, each molecule of H₂SO₄ will contribute 2 H⁺ ions to the solution. Therefore, the [H⁺] would be double the initial concentration, which is 2*(0.10 M) = 0.20 M. This corresponds to option d. So the best answer for this exercise is a combination of option a for the H₂CO₃ solution and option d for the H₂SO₄ solution.

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Most popular questions from this chapter

Consider 1000 . mL of a \(1.00 \times 10^{-4}-M\) solution of a certain acid HA that has a $K_{\text { a value equal to } 1.00 \times 10^{-4} . \text { How much }}$ water was added or removed (by evaporation) so that a solution remains in which 25.0\(\%\) of \(\mathrm{HA}\) is dissociated at equilibrium? Assume that HA is nonvolatile.

a. The principal equilibrium in a solution of \(\mathrm{NaHCO}_{3}\) is $$ \mathrm{HCO}_{3}^{-}(a q)+\mathrm{HCO}_{3}^{-}(a q) \rightleftharpoons \mathrm{H}_{2} \mathrm{CO}_{3}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ Calculate the value of the equilibrium constant for this reaction. b. At equilibrium, what is the relationship between $\left[\mathrm{H}_{2} \mathrm{CO}_{3}\right]\( and \)\left[\mathrm{CO}_{3}^{2-}\right] ?$ c. Using the equilibrium $$ \mathrm{H}_{2} \mathrm{CO}_{3}(a q) \rightleftharpoons 2 \mathrm{H}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q) $$ derive an expression for the pH of the solution in terms of \(K_{\mathrm{a}_{1}}\) and \(K_{\mathrm{a}_{2}}\) using the result from part b. d. What is the pH of a solution of \(\mathrm{NaHCO}_{3} ?\)

Phosphoric acid is a common ingredient in traditional cola drinks. It is added to provide the drinks with a pleasant tart taste. Assuming that in cola drinks the concentration of phosphoric acid is \(0.007 M,\) calculate the \(\mathrm{pH}\) of this solution.

Identify the Lewis acid and the Lewis base in each of the following reactions. a. $\mathrm{Fe}^{3+}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}(a q)$ b. $\mathrm{H}_{2} \mathrm{O}(l)+\mathrm{CN}^{-}(a q) \Longrightarrow \mathrm{HCN}(a q)+\mathrm{OH}^{-}(a q)$ c. $\mathrm{HgI}_{2}(s)+2 \mathrm{I}^{-}(a q) \rightleftharpoons \mathrm{Hgl}_{4}^{2-}(a q)$

Monochloroacetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{2} \mathrm{ClO}_{2},\) is a skin irritant that is used in "chemical peels" intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of \(K_{\mathrm{a}}\) for monochloroacetic acid is \(1.35 \times 10^{-3}\) Calculate the pH of a \(0.10-M\) solution of monochloroacetic acid.
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