Sure, let's tackle this problem step-by-step.
Step-by-Step Solution:
1. Determine the Nature of Both Substances:
- H₂SO₄ (Sulfuric Acid): This is a strong diprotic acid, meaning it can release two hydrogen ions (H⁺) per molecule.
- KOH (Potassium Hydroxide): This is a strong monoprotic base, meaning it releases one hydroxide ion (OH⁻) per molecule.
2. Calculate the Moles of Each Substance:
- Given the molarity (M) and volume (V) for each solution, calculate the moles:
- Moles of H₂SO₄ (n₁) = Molarity × Volume:
[tex]\( n₁ = 0.0100 \, \text{M} \times 1 \, \text{L} = 0.0100 \, \text{moles} \)[/tex]
- Moles of KOH (n₂) = Molarity × Volume:
[tex]\( n₂ = 0.0100 \, \text{M} \times 1 \, \text{L} = 0.0100 \, \text{moles} \)[/tex]
3. Account for Proton Release/Absorption:
- Since H₂SO₄ is diprotic, each mole produces 2 moles of H⁺ ions. Therefore:
- Moles of H⁺ from H₂SO₄ = 0.0100 \, \text{moles} \times 2 = 0.0200 \, \text{moles} \)
- KOH produces hydroxide ions (OH⁻) on a one-to-one basis:
- Moles of OH⁻ from KOH = 0.0100 \, \text{moles} \)
4. Compare the Moles of H⁺ and OH⁻ Ions:
- H⁺ ions from H₂SO₄: 0.0200 moles
- OH⁻ ions from KOH: 0.0100 moles
5. Determine the Type of Solution:
- If the number of H⁺ ions is more than the number of OH⁻ ions, the solution will be acidic.
- If the number of H⁺ ions is less than the number of OH⁻ ions, the solution will be basic.
- If the number of H⁺ ions is equal to the number of OH⁻ ions, the solution will be neutral.
In this case, there are more H⁺ ions (0.0200 moles) than there are OH⁻ ions (0.0100 moles). Therefore, the solution will be acidic.
Conclusion:
Mixing equal volumes of 0.0100 M H₂SO₄ and 0.0100 M KOH results in an acidic solution.
