Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resulting solution. The sodium bicarbonate reacts with sulfuric acid according to: 2 NaHCO3(s) + H2SO4(aq) → Na2SO4(aq) + 2 H2O(l) + 2 CO2(g). Sodium bicarbonate is added until the fizzing due to the formation of CO2(g) stops. If 27 mL of 6.0 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?

Verified step by step guidance

Calculate the moles of H2SO4 spilled using the formula: moles = molarity × volume. Convert the volume from mL to L before using it in the calculation.

Use the balanced chemical equation to determine the stoichiometric ratio between H2SO4 and NaHCO3. According to the equation, 1 mole of H2SO4 reacts with 2 moles of NaHCO3.

Calculate the moles of NaHCO3 required by multiplying the moles of H2SO4 by the stoichiometric ratio (2 moles of NaHCO3 per mole of H2SO4).

Determine the mass of NaHCO3 needed using the formula: mass = moles × molar mass. Look up the molar mass of NaHCO3 (sodium bicarbonate) from the periodic table.

Ensure all units are consistent and check calculations for accuracy. The result will give you the minimum mass of NaHCO3 required to neutralize the spilled H2SO4.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances involved in a reaction. In this case, the stoichiometric coefficients from the balanced equation indicate that two moles of sodium bicarbonate are required to neutralize one mole of sulfuric acid.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is crucial for calculating how much of a substance is needed to react with another. In this scenario, the molarity of sulfuric acid (6.0 M) helps us find the number of moles present in the spilled solution, which is essential for determining the amount of sodium bicarbonate required for neutralization.

Gas Evolution Reaction

A gas evolution reaction occurs when a gas is produced as a product of a chemical reaction. In this case, the reaction between sodium bicarbonate and sulfuric acid produces carbon dioxide gas (CO2), which is observed as fizzing. Understanding this concept is important for recognizing the completion of the reaction and ensuring that enough sodium bicarbonate has been added to fully neutralize the acid.

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