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Chapter 4: Problem 19

When carbon dioxide dissolves in water, it is in equilibrium with carbonic acid \(\mathrm{H}_{2} \mathrm{CO}_{3},\) which is a weak electrolyte. What solutes are present in aqueous solution of this compound? Write the chemical equation for the ionization of \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Short Answer

Expert verified
The solutes present in the aqueous solution of carbonic acid (H₂CO₃) are H⁺ ions and HCO₃⁻ ions. The chemical equation for the ionization of carbonic acid is: \[H_2CO_3 \rightleftharpoons H^+ + HCO_3^-\]

Step by step solution

01

Identify the solutes present in the aqueous solution of carbonic acid.

Carbonic acid is a weak acid, and when it dissolves in water, it partially ionizes, meaning it splits into its constituent ions. In the case of H₂CO₃, the solutes present in an aqueous solution will be H⁺ ions and HCO₃⁻ ions.
02

Write the chemical equation for the ionization of carbonic acid.

To write the chemical equation, we will begin with the chemical formula of carbonic acid (H₂CO₃) and show it ionizing into its constituent ions: \[H_2CO_3 \rightleftharpoons H^+ + HCO_3^-\] This equation represents the ionization of carbonic acid when it dissolves in water, forming H⁺ and HCO₃⁻ ions. The double arrow (\(\rightleftharpoons\)) indicates that the reaction is in equilibrium, meaning it's both forward (ionization) and reverse (recombination) reactions occur simultaneously.

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Most popular questions from this chapter

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