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Chapter 4: Problem 136

Someone spilled concentrated sulfuric acid on the floor of a chemistry laboratory. To neutralize the acid, would it be preferable to pour concentrated sodium hydroxide solution or spray solid sodium bicarbonate over the acid? Explain your choice and the chemical basis for the action.

Short Answer

Expert verified
The preferable choice is Sodium Hydroxide because it neutralizes the sulfuric acid without releasing any gas unlike Sodium Bicarbonate which releases carbon dioxide during the reaction process.

Step by step solution

01

Understand Acid-Base Neutralization

Acid-base neutralization is a chemical process in which an acid and a base react to form water and a salt. In this case, sulfuric acid is the acid we need to neutralize. The base could be either sodium hydroxide or sodium bicarbonate.
02

Analyze reaction of Sulfuric Acid with Sodium Hydroxide

The chemical formula of sulfuric acid is \(H_2SO_4\), and that for sodium hydroxide is \(NaOH\). When they react, the reaction could be represented as: \(H_2SO_4 + 2NaOH \rightarrow Na_2SO_4 + 2H_2O\). In this process, water and Sodium sulfate, a salt, are produced.
03

Analyze reaction of Sulfuric Acid with Sodium Bicarbonate

The chemical formula for sodium bicarbonate is \(NaHCO_3\). The reaction of sulfuric acid and sodium bicarbonate could be represented as: \(H_2SO_4 + 2NaHCO_3 \rightarrow Na_2SO_4 + 2H_2O + 2CO_2\). This process also produces a salt, water but in addition, it releases carbon dioxide gas.
04

Evaluating preferable choice

Both Sodium Hydroxide and Sodium Bicarbonate, are capable of neutralizing the acid. However, the reaction with sodium bicarbonate releases carbon dioxide gas which may add some risks, whereas Sodium Hydroxide neutralizes the acid without releasing any gas. Therefore, using Sodium Hydroxide is a more preferable method.

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Most popular questions from this chapter

A 22.02-mL solution containing \(1.615 \mathrm{~g} \mathrm{Mg}\left(\mathrm{NO}_{3}\right)_{2}\) is mixed with a 28.64-mL solution containing \(1.073 \mathrm{~g}\) \(\mathrm{NaOH}\). Calculate the concentrations of the ions remaining in solution after the reaction is complete. Assume volumes are additive.

Acetylsalicylic acid ( \(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\) ) is a monoprotic acid commonly known as "aspirin." A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took \(12.25 \mathrm{~mL}\) of \(0.1466 \mathrm{M} \mathrm{NaOH}\) to neutralize the solution. Calculate the number of grains of aspirin in the tablet. (One grain \(=0.0648\) g.)

The molecular formula of malonic acid is \(\mathrm{C}_{3} \mathrm{H}_{4} \mathrm{O}_{4}\). If a solution containing \(0.762 \mathrm{~g}\) of the acid requires \(12.44 \mathrm{~mL}\) of \(1.174 \mathrm{M} \mathrm{NaOH}\) for neutralization, how many ionizable \(\mathrm{H}\) atoms are present in the molecule?

Describe how to prepare \(1.00 \mathrm{~L}\) of \(0.646 \mathrm{M} \mathrm{HCl}\) solution, starting with a \(2.00 M \mathrm{HCl}\) solution.

A quantity of \(18.68 \mathrm{~mL}\) of a KOH solution is needed to neutralize \(0.4218 \mathrm{~g}\) of \(\mathrm{KHP}\). What is the concentration (in molarity) of the KOH solution?
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