How many moles of NaOH is needed to neutralize 45.0ml of 0.30M H2SeO4?

0.027 mole of NaOH.

Explanation:

We'll begin by obtaining the number of mole H2SeO4 in 45mL of 0.30M H2SeO4

This is illustrated below:

Molarity of H2SeO4 = 0.3M

Volume of solution = 45mL = 45/1000 = 0.045L

Mole of H2SeO4 =...?

Mole = Molarity x Volume

Mole of H2SeO4 = 0.3 x 0.045

Mole of H2SeO4 = 0.0135 mole

Next, the balanced equation for the reaction. This is given below:

H2SeO4 + 2NaOH –> Na2SeO4 + 2H2O

From the balanced equation above,

1 mole of H2SeO4 required 2 moles of NaOH.

Therefore, 0.0135 mole of H2SeO4 will require = 0.0135 x 2 = 0.027 mole of NaOH.

Therefore, 0.027 mole of NaOH is needed for the reaction.

u i forgot the answer?

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.