Question

What volume (in mL) of a 0.150 M solution of sodium hydroxide is needed to react

completely with 45 mL of a 0.250 M solution of H₂SO4?
2 NaOH(aq) + H₂SO4(aq) →→→ Na₂SO4(aq) + 2 H₂O(1)
O 5.6 mL
O 37.5 mL
O 150 mL
O22.5 mL
O 11.3 mL

Answer 1

150 mL

Step-by-step explanation:

Recall that

`Molarity = (moles)/(volume)`

Now, we are given a Molarity of 0.250 M H2SO4 with a volume of 45 mL. We will convert this to moles

`mol = (M)/(L)`

Then, since the mole ratio from H2SO4 to NAOH is 1:2, we will multiply by 2

Finally, we will get the volume by dividing by the Molarity of NaOH which is 0.150 M.

The setup for the answer is as follow

`(0.25 M H_2SO_4)(45 mL H_2SO_4)((2 mol NaOH)/(1 mol H_2SO_4) )((1)/(0.15MNaOH))`

The final answer is 0.150 L or 150 mL.