How many mL of 0.0875 M H2SO4 would you need to exactly neutralize 50.00 mL of 0.135 M NaOH?
H2SO4 + 2NaOH ==> Na2SO4 + 2H2O
moles NaOH = M x L
moles H2SO4 needed (from the equation) = 1/2 moles NaOH.
moles H2SO4 = M x L. YOu know moles and M, calculate L, then convert to mL.
Man Man
To determine how many milliliters of 0.0875 M H2SO4 are needed to neutralize 50.00 mL of 0.135 M NaOH, we need to use the concept of stoichiometry. Let's break down the steps:
Step 1: Write and balance the chemical equation.
The balanced chemical equation for the reaction between H2SO4 and NaOH is:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
This equation tells us that one mole of H2SO4 reacts with two moles of NaOH.
Step 2: Calculate the number of moles of NaOH.
To calculate the number of moles of NaOH, we use the formula:
moles = concentration (M) × volume (L)
Given that the volume of NaOH is 50.00 mL and the concentration is 0.135 M, we have:
moles of NaOH = 0.135 M × (50.00 mL / 1000 mL/L) = 0.00675 mol
Step 3: Apply the stoichiometry.
Since the stoichiometry of the reaction is 1:2 for H2SO4 and NaOH, from the balanced equation, we know that for every 2 moles of NaOH, we need 1 mole of H2SO4.
Step 4: Calculate the volume of H2SO4.
Now, we can calculate the volume of 0.0875 M H2SO4 needed to neutralize the given amount of NaOH. We use the formula:
volume (L) = moles / concentration (M)
Since the stoichiometry is 1:2, we divide the moles of NaOH by 2:
moles of H2SO4 = 0.00675 mol / 2 = 0.003375 mol
Now, we can find the volume in liters:
volume (L) = 0.003375 mol / 0.0875 M = 0.03857 L
Since the volume is given in milliliters, we multiply by 1000:
volume (mL) = 0.03857 L × 1000 = 38.57 mL
Therefore, you would need approximately 38.57 mL of 0.0875 M H2SO4 to exactly neutralize 50.00 mL of 0.135 M NaOH.