Question

Challenge Sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) and sodium hydroxide solutions react to produce aqueous sodium sulfate and water.

Short answer

The balanced chemical equation for the reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH) is: H2SO4 + 2NaOH -> Na2SO4 + 2H2O From this reaction, 1 mole of H2SO4 will fully react with 2 moles of NaOH, producing 1 mole of Na2SO4 and 2 moles of H2O. If we have 'x' moles of H2SO4, then '2x' moles of NaOH are needed. Similarly, the reaction will produce 'x' moles of Na2SO4 and '2x' moles of H2O.

Step-by-step solution

Write the unbalanced chemical equation

Before solving the problem, we should write the chemical equation representing the reaction between H2SO4 and NaOH: H2SO4 + NaOH -> Na2SO4 + H2O

Balance the chemical equation

Now, we need to balance the chemical equation, so that the number of atoms of each element on both sides of the equation is equal: H2SO4 + 2NaOH -> Na2SO4 + 2H2O Here, we can see that there are 2 moles of NaOH reacting with 1 mole of H2SO4 to produce 1 mole of Na2SO4 and 2 moles of H2O.

Calculating the number of moles

The balanced chemical equation provides the stoichiometry of the reaction. For example, if we had a given amount of sulfuric acid (in moles) and wanted to know how much sodium hydroxide would be required to completely react with it, we could use the stoichiometry to calculate the amount of sodium hydroxide needed. Suppose we have 'x' moles of H2SO4, then we need '2x' moles of NaOH to react completely with it, as per the balanced equation. This can be expressed as: Moles of NaOH = 2 × Moles of H2SO4 Similarly, the moles of products can be calculated: Moles of Na2SO4 = Moles of H2SO4 Moles of H2O = 2 × Moles of H2SO4

Key concepts

Balancing Chemical Equations

In a chemical reaction, the law of conservation of mass states that mass cannot be created or destroyed. This means the number of atoms for each element must be the same on both sides of the equation. Balancing chemical equations ensures this law is obeyed.
In our example, sulfuric acid (\(\mathrm{H}_{2} \mathrm{SO}_{4}\)) reacts with sodium hydroxide (\(\mathrm{NaOH}\)). Initially, the equation was unbalanced:
\[ \mathrm{H}_{2} \mathrm{SO}_{4} + \mathrm{NaOH} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4} + \mathrm{H}_{2} \mathrm{O} \]
To balance it, we equalize the number of atoms on each side. We notice that we need two sodium (Na) atoms to match the sodium sulfate (\(\mathrm{Na}_{2}\mathrm{SO}_{4}\)). Therefore, we add a coefficient of 2 in front of \(\mathrm{NaOH}\) and \(\mathrm{H}_{2} \mathrm{O}\) to balance the hydrogen and sodium atoms. This gives us:
\[ \mathrm{H}_{2} \mathrm{SO}_{4} + 2\mathrm{NaOH} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4} + 2\mathrm{H}_{2} \mathrm{O} \]
This equation is now balanced as there are equal numbers of each type of atom on both sides.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to calculate the quantities of reactants and products. It relies on the mole concept — where a mole is \(6.022 \times 10^{23}\) particles, such as atoms or molecules. This helps us understand the proportional relationships in a reaction. In our balanced equation, stoichiometry tells us that:

• 1 mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) reacts with 2 moles of \(\mathrm{NaOH}\)
• This produces 1 mole of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) and 2 moles of \(\mathrm{H}_{2} \mathrm{O}\)

For example, to find out how much \(\mathrm{NaOH}\) is needed for a given amount of \(\mathrm{H}_{2} \mathrm{SO}_{4}\), multiply the moles of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) by 2. Likewise, to find products from a given amount of \(\mathrm{H}_{2} \mathrm{SO}_{4}\), you multiply by their respective coefficients in the balanced equation. Stoichiometry provides the bridge between chemical equations and real-world quantities.

Sulfuric Acid

Sulfuric acid (\(\mathrm{H}_{2} \mathrm{SO}_{4}\)) is a strong mineral acid known for its highly corrosive properties. It is widely used in industry for a variety of applications, including the manufacture of fertilizers, in oil refining, and in wastewater processing.
In our reaction, sulfuric acid acts as an acid that donates protons (\(\mathrm{H}^{+}\)) to the base, sodium hydroxide. It is important to handle sulfuric acid with care due to its corrosive nature; it can cause severe chemical burns and damage to materials. Always follow safety protocols when working with it in a lab environment. Remember that understanding its reactive properties helps us predict and manage chemical reactions more effectively.

Sodium Hydroxide

Sodium hydroxide (\(\mathrm{NaOH}\)), also known as lye or caustic soda, is a strong base commonly used in the manufacture of soaps, paper, and various cleaning agents. In chemical reactions, it typically acts as a base, able to neutralize acids by accepting protons (\(\mathrm{H}^{+}\)) from acids like \(\mathrm{H}_{2} \mathrm{SO}_{4}\).
In our example, sodium hydroxide reacts with sulfuric acid to form sodium sulfate and water. When using \(\mathrm{NaOH}\), it's crucial to utilize protective gear, as it can cause burns similar to those caused by sulfuric acid. Understanding how bases like sodium hydroxide react with acids allows chemists to utilize these reactions to create a variety of useful compounds and manage acidity in different contexts effectively.