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Chapter 6: Problem 34

Write the autoprotolysis reaction of \(\mathrm{H}_{2} \mathrm{SO}_{4}\).

Short Answer

Expert verified
The autoprotolysis reaction of \(\mathrm{H}_{2}\mathrm{SO}_{4}\) is \(2\, \mathrm{H}_{2}\mathrm{SO}_{4} \rightleftharpoons \mathrm{HSO}_{4}^{-} + \mathrm{H}_{3}\mathrm{SO}_{4}^{+}\).

Step by step solution

01

Understand Autoprotolysis

Autoprotolysis is a process where a substance reacts with itself to form ions. It often involves the transfer of a proton from one molecule to another.
02

Identify Molecules

Identify the substance involved which is sulfuric acid \(\mathrm{H}_{2}\mathrm{SO}_{4}\). This is a diprotic acid capable of donating two protons, but we consider its behavior as a proton donor and acceptor in this context.
03

Write Reaction Components

For the autoprotolysis of \(\mathrm{H}_{2}\mathrm{SO}_{4}\), one \(\mathrm{H}_{2}\mathrm{SO}_{4}\) molecule donates a proton (\(\mathrm{H}^{+}\)) to another \(\mathrm{H}_{2}\mathrm{SO}_{4}\) molecule, forming \(\mathrm{HSO}_{4}^{-}\) and \(\mathrm{H-O-SO}_{3}H^{+}\).
04

Balance the Reaction

Ensure that the chemical equation is balanced in terms of both atoms and charges. The equation becomes: \[ 2\, \mathrm{H}_{2}\mathrm{SO}_{4} \rightleftharpoons \mathrm{HSO}_{4}^{-} + \mathrm{H}_{3}\mathrm{SO}_{4}^{+} \]This represents the transfer of a proton between two sulfuric acid molecules.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sulfuric Acid
Sulfuric acid, chemically represented as \(\mathrm{H}_{2}\mathrm{SO}_{4}\), is a strong mineral acid known for its diverse industrial applications. It is a colorless, odorless, and syrupy liquid that plays a crucial role in the chemical industry. One of its most notable properties is its ability to dissociate completely in water, making it a strong acid.
In the context of autoprotolysis, sulfuric acid acts both as a proton donor and a proton acceptor. This dual functionality is essential for understanding certain reactions where it participates in transferring protons between molecules that are identical. Due to this capability, sulfuric acid is extensively used in the production of fertilizers, in battery acid, and as a reagent in various chemical synthesis processes.
  • Colorless and odorless
  • Strong mineral acid
  • Used in multiple industrial applications
Diprotic Acid
Sulfuric acid is classified as a diprotic acid, meaning it has two protons that it can donate in a chemical reaction. This characteristic is different from monoprotic acids, which can donate only one proton. The diprotic nature of sulfuric acid makes it particularly potent, allowing it to undergo a two-step ionization process in water.
In the first ionization step, sulfuric acid donates one proton, forming the bisulfate ion \(\mathrm{HSO}_{4}^{-}\). In the second ionization step, it can further dissociate to give another proton, resulting in \(\mathrm{SO}_{4}^{2-}\). During autoprotolysis, these dissociation steps facilitate proton transfer between identical sulfuric acid molecules.
  • Two-step ionization process
  • Forms bisulfate and sulfate ions
  • Significant role in proton donation and acceptance
Proton Transfer
Proton transfer is an essential mechanism in chemical reactions, particularly in acids like sulfuric acid. This process involves the transfer of a hydrogen ion (proton) from one molecule to another. In the context of autoprotolysis, sulfuric acid molecules exchange protons, demonstrating their ability to both donate and accept protons.
The process occurs when one \(\mathrm{H}_{2}\mathrm{SO}_{4}\) molecule donates a proton to another, forming \(\mathrm{HSO}_{4}^{-}\) and \(\mathrm{H}_{3}\mathrm{SO}_{4}^{+}\). This showcases the chemical potential of sulfuric acid to participate in internal proton exchange, influencing the acidity and chemical behavior of the solution.
  • Involves hydrogen ion transfer
  • Facilitates acid strength and reactivity
  • Key in internal molecular interactions
Chemical Equation Balancing
Balancing chemical equations is crucial for representing reactions accurately. It ensures that the number of atoms and the charges on both sides of the equation are equal, reflecting the conservation of mass and charge.
In the autoprotolysis of sulfuric acid, the process involves balancing the equation to correctly depict the proton transfer. The balanced chemical equation for the autoprotolysis reaction is: \[ 2 \, \mathrm{H}_{2}\mathrm{SO}_{4} \rightleftharpoons \mathrm{HSO}_{4}^{-} + \mathrm{H}_{3}\mathrm{SO}_{4}^{+} \]This balanced equation indicates that two molecules of sulfuric acid participate in the reaction, ensuring that the end products \(\mathrm{HSO}_{4}^{-}\) and \(\mathrm{H}_{3}\mathrm{SO}_{4}^{+}\) maintain the balance of atoms and charges. Balancing requires careful counting of hydrogen and sulfur atoms, as well as the overall charge on each side.
  • Ensures conservation of mass and charge
  • Depicts accurate chemical interactions
  • Essential for understanding reaction mechanics

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Most popular questions from this chapter

Identify the Bronsted-Lowry acids among the reactants in the following reactions: (a) \(\mathrm{KCN}+\mathrm{HI} \rightleftharpoons \mathrm{HCN}+\mathrm{KI}\) (b) \(\mathrm{PO}_{4}^{3-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{OH}^{-}\)

Write the expression for the equilibrium constant for each of the following reactions. Write the pressure of a gaseous molecule, \(\mathrm{X}\), as \(P_{\mathrm{X}}\) - (a) \(3 \mathrm{Ag}^{+}(a q)+\mathrm{PO}_{4}^{3-}(a q) \rightleftharpoons \mathrm{Ag}_{3} \mathrm{PO}_{4}(s)\) (b) \(\mathrm{C}_{6} \mathrm{H}_{6}(l)+\frac{15}{2} \mathrm{O}_{2}(g) \rightleftharpoons 3 \mathrm{H}_{2} \mathrm{O}(l)+6 \mathrm{CO}_{2}(g)\)

The planet Aragonose (which is made mostly of the mineral aragonite, whose composition is \(\mathrm{CaCO}_{3}\) ) has an atmosphere containing methane and carbon dioxide, each at a pressure of \(0.10\) bar. The oceans are saturated with aragonite and have a concentration of \(\mathrm{H}^{+}\)equal to \(1.8 \times 10^{-7} \mathrm{M}\). Given the following equilibria, calculate how many grams of calcium are contained in \(2.00 \mathrm{~L}\) of Aragonose seawater. $$ \begin{aligned} \mathrm{CaCO}_{3}(s, \text { aragonite }) & \rightleftharpoons \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q) & & K_{\text {sp }}=6.0 \times 10^{-9} \\ \mathrm{CO}_{2}(g) & \rightleftharpoons \mathrm{CO}_{2}(a q) & & K_{\mathrm{CO}_{2}}=3.4 \times 10^{-2} \\ \mathrm{CO}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) & \rightleftharpoons \mathrm{HCO}_{3}^{-}(a q)+\mathrm{H}^{+}(a q) & & K_{1}=4.5 \times 10^{-7} \\ \mathrm{HCO}_{3}^{-}(a q) & \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{CO}_{3}^{2-}(a q) & & K_{2}=4.7 \times 10^{-11} \end{aligned} $$ Don't panic! Reverse the first reaction, add all the reactions together, and see what cancels.

The equilibrium constant for the reaction \(\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{H}^{+}+\mathrm{OH}^{-}\) is \(1.0 \times 10^{-14}\) at \(25^{\circ} \mathrm{C}\). What is the value of \(K\) for the reaction \(4 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons 4 \mathrm{H}^{+}+4 \mathrm{OH}^{-} ?\)

\(\mathrm{BaCl}_{2} \cdot \mathrm{H}_{2} \mathrm{O}(s)\) loses water when it is heated in an oven: $$ \begin{gathered} \mathrm{BaCl}_{2} \cdot \mathrm{H}_{2} \mathrm{O}(s) \rightleftharpoons \mathrm{BaCl}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(g) \\ \Delta H^{\circ}=63.11 \mathrm{~kJ} / \mathrm{mol} \text { at } 25^{\circ} \mathrm{C} \\ \Delta S^{\circ}=+148 \mathrm{~J} /(\mathrm{K} \cdot \mathrm{mol}) \text { at } 25^{\circ} \mathrm{C} \end{gathered} $$ (a) Write the equilibrium constant for this reaction. Calculate the vapor pressure of gaseous \(\mathrm{H}_{2} \mathrm{O}\left(P_{\mathrm{H}_{2} \mathrm{O}}\right)\) above \(\mathrm{BaCl}_{2} \cdot \mathrm{H}_{2} \mathrm{O}\) at \(298 \mathrm{~K}\). (b) If \(\Delta H^{\circ}\) and \(\Delta S^{\circ}\) are not temperature dependent (a poor assumption), estimate the temperature at which \(P_{\mathrm{H}_{2} \mathrm{O}}\) above \(\mathrm{BaCl}_{2} \cdot \mathrm{H}_{2} \mathrm{O}(s)\) will be 1 bar.
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