How many milliliters of 0.205 M NaOH solution are needed to completely neutralize 5.50 mL of 0.865 M H2SO4 solution?
2NaOH + H2SO4 ==> Na2SO4 + 2H2O
mols H2SO4 = M x L = ?
Using the coefficients in the balanced equation, convert mols H2SO4 to mols NaOH. That's mols H2SO4 x (2 mols NaOH/1 ml H2SO4) = ?
Then M NaOH = mols NaOH/L NaOH. YOu know M NaOH and mols NaOH, solve for L NaOH and convert to mL.
To find the number of milliliters of NaOH solution needed to neutralize the H2SO4 solution, we can use stoichiometry, which is based on the balanced chemical equation for the reaction between NaOH and H2SO4.
The balanced chemical equation for the reaction is:
2 NaOH + H2SO4 -> Na2SO4 + 2 H2O
From the balanced equation, we can see that 2 moles of NaOH react with 1 mole of H2SO4. This means that the ratio of NaOH to H2SO4 is 2:1.
First, we need to calculate the moles of H2SO4 present in 5.50 mL of the 0.865 M H2SO4 solution.
Moles of H2SO4 = volume (in L) x concentration (in mol/L)
= (5.50 mL / 1000 mL/L) x 0.865 mol/L
= 0.0047675 mol
Since the ratio of NaOH to H2SO4 is 2:1, we divide the moles of H2SO4 by 2 to find the moles of NaOH needed.
Moles of NaOH needed = 0.0047675 mol / 2
= 0.00238375 mol
Now, we can calculate the volume of the 0.205 M NaOH solution needed to provide this amount of NaOH.
Volume (in L) of NaOH solution = moles of NaOH needed / concentration of NaOH (in mol/L)
= 0.00238375 mol / 0.205 mol/L
≈ 0.0116 L
Finally, we convert the volume from liters to milliliters.
Volume (in mL) of NaOH solution = 0.0116 L x 1000 mL/L
= 11.6 mL
Therefore, approximately 11.6 milliliters of the 0.205 M NaOH solution are needed to completely neutralize 5.50 milliliters of the 0.865 M H2SO4 solution.