How many moles of NaOH is needed to neutralize 45.0 ml of 0.30M H2SeO4? Question 2 options: A) 0.00675 B) 27.0 C) 0.027 D) 0.0135

C) 0.027

Explanation:

In this case we can start with the reaction between and , so:

We have an acid () and a base (), therefore we will have an acid-base reaction in which a salt is produced () and water ().

Now we can balance the reaction:

If we have the volume (45 mL= 0.045 L) and the concentration (0.3 M) of the acid we can calculate the moles using the molarity equation:

In the balanced reaction, we have a 2:1 molar ratio between the acid and the base (for each mol of 2 moles of are consumed), with this in mind we can calculate the moles of NaOH:

I hope it helps!