What volume of 0.200 N H2SO4 is required to neutralize a solution containing 8.00 equivalents of NaOH?
L x N = equivalents
To solve this problem, we need to use the concept of equivalents and the balanced chemical equation. Here's how you can find the volume of 0.200 N H2SO4 required to neutralize the solution containing 8.00 equivalents of NaOH:
Step 1: Write the balanced chemical equation for the reaction between H2SO4 and NaOH:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
Step 2: Determine the mole ratio between H2SO4 and NaOH from the balanced equation:
From the equation, we see that 1 mole of H2SO4 reacts with 2 moles of NaOH.
Step 3: Calculate the moles of NaOH from the given equivalent value:
Since we are given that the solution contains 8.00 equivalents of NaOH, we can convert this to moles by multiplying the equivalent value by the equivalent weight of NaOH.
Equivalent weight of NaOH = molar mass / number of equivalents
For NaOH, the molar mass is 22.99 + 16.00 + 1.01 = 40.00 g/mol, and the number of equivalents is 1 (since NaOH is monovalent).
Equivalent weight of NaOH = 40.00 g/mol / 1 = 40.00 g-equiv
Moles of NaOH = 8.00 equiv x (1 mol NaOH / 40.00 g-equiv)
Step 4: Determine the moles of H2SO4 required using the mole ratio from step 2:
From the balanced equation, we know that 1 mole of H2SO4 reacts with 2 moles of NaOH. Therefore, the moles of H2SO4 required will be half of the moles of NaOH.
Moles of H2SO4 = 1/2 x moles of NaOH
Step 5: Calculate the volume of 0.200 N H2SO4 required:
To find the volume, you can use the equation:
Moles = Molarity x Volume (in liters)
First, rearrange the equation to solve for the volume:
Volume (in liters) = Moles / Molarity
Given that the concentration of H2SO4 is 0.200 N (which means 0.200 moles per liter), and the moles of H2SO4 calculated in step 4, you can substitute those values into the equation to find the volume.
Volume of 0.200 N H2SO4 = Moles of H2SO4 / Molarity of H2SO4