Question

Sulfuric acid is commonly used as an electrolyte in car batteries. Suppose you spill some on your garage floor. Before cleaning it up, you wisely decide to neutralize it with sodium bicarbonate (baking soda) from your kitchen. The reaction of sodium bicarbonate and sulfuric acid is $$ 2 \mathrm{NaHCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \underset{\mathrm{Na}_{2} \mathrm{SO}_{4}(a q)}{\longrightarrow}+2 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ You estimate that your acid spill contains about \(2.0 \mathrm{~mol}\) \(\mathrm{H}_{2} \mathrm{SO}_{4}\). What mass of \(\mathrm{NaHCO}_{3}\) do you need to neutralize the acid?

Short answer

Therefore, one needs 336 grams of Sodium Bicarbonate to neutralize 2 moles of Sulfuric Acid.

Step-by-step solution

Find the Molar Ratio

Based on the balanced chemical equation, one can see that it takes 2 moles of Sodium Bicarbonate to neutralize 1 mole of Sulfuric Acid (\(2 \mathrm{NaHCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)\). The molar ratio of Sodium Bicarbonate to Sulfuric Acid is thus 2:1.

Calculate the Moles of Sodium Bicarbonate

Because the molar ratio is 2:1, one will therefore need \(2*2 = 4\) moles of Sodium Bicarbonate to neutralize 2 moles of Sulfuric Acid.

Convert Moles to Mass

The molar mass of Sodium Bicarbonate (\(NaHCO_3\)) is approximately 84 g/mol. Hence, the required mass of Sodium Bicarbonate is \(4 \text{ moles} * 84 \text{ g/mol} = 336 \text{ grams}\).

Key concepts

Chemical Reactions

In the world of chemistry, chemical reactions are processes where substances are transformed into new substances. These are depicted using chemical equations, like the one representing the interaction between sulfuric acid and sodium bicarbonate. Simplifying this, the equation describes how substances on the left-hand side (reactants) produce new substances on the right-hand side (products). Here, the reactants are sulfuric acid ( H_2SO_4 ) and sodium bicarbonate ( NaHCO_3 ). A key part of understanding chemical reactions is recognizing that atoms are not created or destroyed—just rearranged. This principle forms the basis of stoichiometry, which helps calculate amounts of reactants and products. In the given reaction, the balanced equation tells us the exact proportions needed—2 moles of sodium bicarbonate react with 1 mole of sulfuric acid. Recognizing the need to balance chemical equations is essential because it ensures the law of conservation of mass is obeyed. By correctly balancing equations, chemists can predict the results of chemical reactions and know exactly how much of each reactant is required to form a specific amount of product.

Acid-Base Reactions

Acid-base reactions are a specific type of chemical reaction where an acid reacts with a base to produce a salt and water. Understanding this concept is crucial because it includes everyday substances and processes, like neutralizing spills in your garage! The reaction between sulfuric acid and sodium bicarbonate is a classic example. Here, sulfuric acid acts as the acid, and sodium bicarbonate acts as the base. When they react, sodium sulfate (a salt), carbon dioxide, and water are produced. This is why you may notice fizzing or bubbling, as carbon dioxide gas is released. Neutralization reactions are not only important in academic scenarios but also in practical, everyday situations. By using sodium bicarbonate to neutralize sulfuric acid, you effectively reduce the harmful acidic qualities of the spill, making it safer to clean. This balances out the pH level, showcasing the base's ability to counteract or 'neutralize' the acid's properties.

Molar Calculations

Molar calculations are essential to determining the correct quantities needed in chemical reactions. These calculations help us quantify the number of reactants and products in a chemical equation. To solve the exercise, first, understand molar ratios, derived from the balanced chemical equation. Here, the ratio is 2:1 for sodium bicarbonate to sulfuric acid. This means two moles of sodium bicarbonate are required for each mole of sulfuric acid. The exercise states we need to neutralize 2.0 moles of sulfuric acid. Using the molar ratio, we calculate: - We need 4 moles of sodium bicarbonate (because 2 moles of sodium bicarbonate per mole of sulfuric acid, resulting in 2 * 2 = 4). The next step in molar calculations is to convert these moles into a measurable mass. Given the molar mass of sodium bicarbonate ( NaHCO_3 ) is 84 g/mol, you then calculate the required mass: - Mass = Number of moles * Molar mass = 4 moles * 84 g/mol = 336 grams. This meticulous calculation ensures that you have precisely the right amount of sodium bicarbonate to handle the spill effectively, without excess waste or deficit. Understanding molar calculations makes chemistry practical, helping transform theoretical equations into tangible actions.