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Chapter 8: Problem 4

\(\mathrm{HCl}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NaCl}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\)

Short Answer

Expert verified
The reaction between hydrochloric acid (HCl) and sodium carbonate (Na2CO3) is an acid-base or double displacement reaction, forming sodium chloride (NaCl), carbon dioxide (CO2), and water (H2O). The balanced chemical equation for this reaction is: \(\mathrm{HCl}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NaCl}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\).

Step by step solution

01

Write the balanced chemical equation

The given balanced chemical equation for the reaction between hydrochloric acid and sodium carbonate is: \(\mathrm{HCl}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NaCl}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\)
02

Identify the type of reaction

This reaction is an example of an acid-base reaction, also known as a double displacement or metathesis reaction. In this type of reaction, the hydrogen ion (H+) from the acid reacts with the carbonate ion (CO3 2-) from the base, forming water (H2O) and carbon dioxide (CO2). The sodium ion (Na+) from the base reacts with the chloride ion (Cl-) from the acid, forming sodium chloride (NaCl).
03

Describe the reaction

During the reaction, hydrochloric acid (HCl) donates a proton (H+) to the carbonate ion (CO3 2-) from sodium carbonate (Na2CO3). This results in the formation of water (H2O) and carbon dioxide (CO2). The balanced equation for this part of the reaction is: \(\mathrm{2HCl}+\mathrm{CO}_{3}^{2-} \rightarrow \mathrm{2Cl}^{-}+\mathrm{CO}_{2}+\mathrm{2H}_{2} \mathrm{O}\) Simultaneously, the sodium ions (Na+) from sodium carbonate react with the chloride ions (Cl-) from hydrochloric acid, forming sodium chloride (NaCl). The balanced equation for this part of the reaction is: \(\mathrm{2Na}^{+}+\mathrm{2Cl}^{-} \rightarrow \mathrm{2 NaCl}\)
04

Combine the reactions

Now, we can combine the two individual reactions to obtain the overall balanced equation: \(\mathrm{HCl}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NaCl}+\mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O}\) The balanced chemical equation represents the reaction between hydrochloric acid and sodium carbonate, resulting in the formation of sodium chloride, carbon dioxide, and water.

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Most popular questions from this chapter

Sulfur dioxide and water are formed when hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\), reacts with oxygen gas. Write the balanced equation for the reaction.

Balance this chemical equation and assign it a reaction type: \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Na}_{2} \mathrm{~S}(a q) \rightarrow \mathrm{Fe}_{2} \mathrm{~S}_{3}(s)+\mathrm{NaNO}_{3}(a q)\)

Aqueous solutions of calcium chloride and potassium carbonate are combined. (a) Write the formulas for both reactants. (b) Does a precipitation reaction occur? Explain. (c) If it does, write a net ionic equation for the reaction.

In the chapter, we saw the combustion reaction for methane. This was actually a complete combustion reaction because carbon ended up as carbon dioxide. If the same reaction is carried out where the oxygen supply is limited, incomplete combustion takes place, yielding toxic carbon monoxide, CO, instead of \(\mathrm{CO}_{2}\). Write the balanced reaction for the incomplete combustion of methane. Make sure it is balanced.

Consider the ionic bonds between \(\mathrm{Na}^{+}\) ions and \(\underline{\mathrm{Cl}}^{-}\) ions in \(\mathrm{NaCl}(\mathrm{s}) .\) Why must energy be added to break these bonds (in other words, what is the added energy used for)?
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