What volume of distilled water should be added to 400cm3 of 2.0 mole dm-3 \(H_{2}SO_{4}\) to obtain 0.20 mole dm-3 of solution>

What volume of distilled water should be added to 400cm3 of 2.0 mole dm-3 \(H_{2}SO_{4}\) to obtain 0.20 mole dm-3 of solution>

Answer Details

This is a dilution problem in chemistry. The formula for dilution is C₁V₁ = C₂V₂, where C₁ and V₁ are the initial concentration and volume, respectively, and C₂ and V₂ are the final concentration and volume, respectively. We can rearrange the formula to solve for V₂: V₂ = (C₁V₁)/C₂ Substituting the values given in the question, we get: V₂ = (2.0 mol dm^-3 x 400 cm³)/0.20 mol dm^-3 Simplifying the expression, we get: V₂ = 4,000 cm³ Therefore, 4,000cm³ of solution is needed. However, the question is asking for the volume of distilled water to add, so we need to subtract the initial volume from the final volume to get the volume of distilled water needed: Volume of distilled water = V₂ - V₁ = 4,000 cm³ - 400 cm³ = 3,600 cm³ Hence, the correct option is 3,600 cm³.