How many milliliters of 0.60 H₂SO₄ are required to neutralize 90 mL of 0.40 NaOH?

The answer to your question is 30 ml of H₂SO₄

Explanation:

Data

the volume of H₂SO₄ = ?

[H₂SO₄] = 0.6 M

volume of NaOH = 90 ml

[NaOH] = 0.4

Process

1.- Write the balanced chemical equation

             H₂SO₄  +  2NaOH  ⇒  Na₂SO₄  +  2H₂O

2.- Calculate the moles of NaOH

Molarity = moles/volume

moles = Molarity x volume

-Substitution

moles = 0.4 x 0.09

-result

moles = 0.036 of NaOH

3.- Calculate the moles of H₂SO₄

            1 mol of H₂SO₄ 2 moles of NaOH

             x                       0.036 moles of NaOH

                   x = (0.036 x 1)/2

                   x = 0.018 moles of H₂SO₄

4.- Calculate the volume of H₂SO₄

Volume = moles / Molarity

-Substitution

Volume = 0.018 / 0.6

-Result

Volume = 0.03 ml or 30 ml

"hydrogen bonding is the attraction of h atoms in the water molecule (slight + charge) to o atoms in a neighboring water molecule (slight - charge); it is a weak interatomic force. but it is still strong enough to the water molecules "stick" together."

answer:

the reaction is type of combination reaction.

explanation:

on the product side, there are 2 molecules of bonded to fe   which means one atom of fe are combined two molecules of . so, balanced chemical equation becomes :

this reaction follows the reaction type of combination reaction. a combination reaction is defined as chemical reaction in which reactants combines together to form a single product.