Final answer:
The reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH) is an acid-base neutralization. When 100cc of 1M H2SO4 is mixed with 20cc of 5M NaOH, an equal number of moles for both substances will fully react, producing Sodium Sulfate (Na2SO4) and water.
Step-by-step explanation:
This question is about the reaction between sulfuric acid (H₂SO₄) and sodium hydroxide (NaOH). This is an example of acid-base neutralization. The balanced chemical equation of this reaction is:
H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O
Since the molarity and volume of both substances are provided, we can calculate the number of moles in each solution and determine the ratio of reactants. The reaction’s stoichiometry suggests that one mole of H₂SO₄ reacts with 2 moles of NaOH.
To figure out whether we have enough NaOH, we need to calculate the number of moles in 100cc of 1M H₂SO₄ and 20cc of 5M NaOH. Here's how to do that:
- For H₂SO₄: (100/1000) L * 1 mol/L = 0.1 mol
- For NaOH: (20/1000) L * 5 mol/L = 0.1 mol
So, you have an equal amount of moles for both H₂SO₄ and NaOH, suggesting that all reactants will completely react. Hence, the resulting solution contains Sodium Sulfate (Na₂SO₄) and water (H₂O).
Learn more about Acid-Base Neutralization