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Chapter 8: Problem 74

Write the intact-molecule equation and the net ionic equation for the neutralization reaction between perchloric acid, \(\mathrm{HClO}_{4}(a q)\), and \(\mathrm{NaOH}(a q)\). What salt is in solution once the reaction is run?

Short Answer

Expert verified
The intact-molecule equation for the neutralization reaction between perchloric acid, $\mathrm{HClO}_{4}(a q)$, and $\mathrm{NaOH}(a q)$ is: \[\mathrm{HClO}_4(aq) + \mathrm{NaOH}(aq) \rightarrow \mathrm{NaClO}_4(aq) + \mathrm{H}_2\mathrm{O}(l)\] The net ionic equation is: \[\mathrm{H}^+(aq) + \mathrm{OH}^-(aq) \rightarrow \mathrm{H}_2\mathrm{O}(l)\] The salt in solution once the reaction is run is sodium perchlorate, $\mathrm{NaClO}_4$.

Step by step solution

01

1. Write the chemical equation for the reaction with intact molecules

First, we need to write the chemical reaction between perchloric acid, HClO4, and sodium hydroxide, NaOH. We know that acids and bases react with each other to form water and a salt. Therefore, the intact-molecule equation will be: HClO4(aq) + NaOH(aq) -> NaClO4(aq) + H2O(l)
02

2. Write the complete ionic equation

Next, we need to write the complete ionic equation by dissociating the soluble ionic compounds into their individual ions: H+(aq) + ClO4^-(aq) + Na+(aq) + OH^-(aq) -> Na+(aq) + ClO4^-(aq) + H2O(l)
03

3. Write the net ionic equation

Now, we can write the net ionic equation by eliminating spectator ions (ions that appear on both sides of the equation). In this case, the spectator ions are Na+(aq) and ClO4^-(aq). Thus, the net ionic equation will be: H+(aq) + OH^-(aq) -> H2O(l)
04

4. Identify the salt formed in the solution

The salt formed in the solution after the reaction between perchloric acid and sodium hydroxide is sodium perchlorate (NaClO4). In conclusion, the intact-molecule equation is: HClO4(aq) + NaOH(aq) -> NaClO4(aq) + H2O(l) The net ionic equation is: H+(aq) + OH^-(aq) -> H2O(l) And the salt formed in the solution once the reaction is run is sodium perchlorate (NaClO4).

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