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

1. 1 mole of anything contains 6.022x10^23 pieces  

d  

2. a  

3. c, number  

5. 1.24x10^24atoms / 6.022x10^23atoms/mole = 2moles h2 atoms  

6. fe2br3 mass = 2moles x mass fe + 3 moles x mass br  

molar mass = grams / number of moles = g/mole  

to find moles = g / molar mass  

to find mass = g = molar mass / moles