Sodium hydroxide (NaOH) reacts with

Question

sulphuric acid
(H 2 SO 4 ) according to the following
2NaOH (
aq H 2 SO 4 aq ))→ 2H 2 O (l) + Na 2 SO 4 aq
Find the volume of 0.112 M NaOH solution required to
completely react with 10.0 mL of H 2 SO 4 solution.

Answer 1

First, we need to determine the number of moles of H2SO4 present in the 10.0 mL solution. We can use the concentration and volume to do this:

moles H2SO4 = concentration x volume
moles H2SO4 = 1 M x 0.010 L
moles H2SO4 = 0.010 moles

Next, we can use the stoichiometry of the balanced chemical equation to determine the number of moles of NaOH needed to react with the H2SO4:

1 mole H2SO4 reacts with 2 moles NaOH

moles NaOH = 0.010 moles H2SO4 x (2 moles NaOH / 1 mole H2SO4)
moles NaOH = 0.020 moles

Finally, we can use the concentration and number of moles to calculate the volume of the NaOH solution needed:

moles NaOH = concentration x volume
0.020 moles = 0.112 M x volume
volume = 0.178 L or 178 mL

Therefore, we need 178 mL of the 0.112 M NaOH solution to completely react with 10.0 mL of the H2SO4 solution.